A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb2+ half-cell. Measurement shows that the silver electrode is positive.
(a) Write balanced half-reactions and the overall spontaneous reaction. (Type your answer using the format [NH4]+ for NH4+. Use the lowest possible coefficients.)
reduction:
__Ag+(aq) + __e- -> ___(s)
oxidation:
__(s) ->__Pb2+(aq) +__e-
overall reaction:
__Ag+(aq) +__(s) ->__(s) + __ Pb2+(aq)

(b) The cation flow is towards which electrode?
lead OR silver
What process occurs at the lead electrode?
oxidation OR reduction
In which direction do the electrons flow?
from the lead electrode to the silver electrode OR from the silver electrode to the lead electrode

Final answer:

To find the volume of diethylamine needed for an experiment, dividing the required mass (65.0 g) by the density of diethylamine (0.706 g/cm3) calculates a volume of 92.1 mL that the student should measure out.

Explanation:

To calculate the volume of diethylamine that a student needs for an experiment, use the formula that relates mass, density, and volume: volume = mass / density. Here, the mass required is 65.0 g, and the density of diethylamine is given as 0.706 g/cm3.

Substitute the given values into the formula:

Volume = 65.0 g / 0.706 g/cm3 = 92.1 cm3 or 92.1 mL, since 1 cm3 = 1 mL.

Therefore, the student should pour out 92.1 mL of diethylamine for their experiment.

Answer:

CaCO3 (s)  → CaO (s) + CO2 (g)

The mass of carbonate that must have reacted was 43.03 grams

Explanation:

CaCO3  → CaO + CO2

Relation between reactant and product is 1:1

Let's apply the Ideal Gas Law to find out the moles of CO2 which were produced.

P . V = n . R . T

1 atm . 23 L = n . 0.082 L.atm/mol.K . 653K

(1atm . 23L) / (0.082 mol.K/L.atm . 653K) = n

0.43 moles = n

0.43 moles of CO2, were produced from 0.43 moles of CaCO3.

Molar weight of CaCO3 = 100.08 g/m

Mass = Molar weight . moles

Mass = 100.08 g/m 0.43 m = 43.03 g

The decomposition of calcium carbonate (CaCO₃) can be represented by the equation: CaCO₃(s) → CaO(s) + CO₂(g). Using the ideal gas law, we calculate that approximately 43.1 grams of CaCO₃ reacted to produce 23.0 liters of CO₂ at 380.0 °C and 1 atm pressure.

Decomposition of Calcium Carbonate:

The balanced chemical equation for the decomposition of solid calcium carbonate (CaCO₃) into solid calcium oxide (CaO) and gaseous carbon dioxide (CO₂) is:

CaCO₃(s) → CaO(s) + CO₂(g)

To calculate the mass of calcium carbonate that reacted to produce 23.0 L of CO₂ gas at 380.0 °C and 1 atm, we use the ideal gas law. The ideal gas law is expressed as:

PV = nRT

Where:

Rearranging the ideal gas law to solve for n (moles of CO₂) gives:

n = PV / RT

Substituting the known values:

n = (1 atm * 23.0 L) / (0.0821 L·atm/mol·K * 653.15 K) ≈ 0.431 moles of CO₂

From the balanced equation, 1 mole of CaCO₃ produces 1 mole of CO₂. Hence, the moles of CaCO₃ that reacted is also 0.431 mol.

The molar mass of CaCO₃ is approximately 100.09 g/mol.

The mass of CaCO₃ that reacted is:

mass = moles * molar mass

mass = 0.431 mol * 100.09 g/mol ≈ 43.1 g

Thus, about 43.1 grams of calcium carbonate must have reacted.

Answer:

The partial pressure of N2O is 143.6 kPa

Explanation:

Step 1: Data given

Moles O2 = 2.83 mol

Moles N2O = 8.41 mol

Total pressure = 192 kPa

Step 2: Calculate total number of moles

Total numberof moles = moles O2  + molesN2O = 2.83 + 8.41 = 11.24 mol

Step 3: Calculate mole fraction of N2O

Mole fraction N2O = mole N2O / Total moles

Mole fraction N2O = 8.41 / 11.24 = 0.748

Step 4: Calculate partial pressure of N2O

pN2O = 0.748 * 192 kPa

pN2O = 143.6 kPa

The partial pressure of N2O is 143.6 kPa

Answer: 144 kPa

Explanation:

To determine the partial pressure of N2O, first determine the mole fraction of N2O in the mixture, then multiply the mole fraction of N2O by the total pressure.

XN2O = nN2O/ ntotal = 8.41 mol / 2.83 mol + 8.41 mol = 0.7482

PN2O=XN2O×Ptotal = 0.7482 × 192 kPa = 143.7 kPa

Rounding the answer to three significant figures, the partial pressure of N2O is 144kPa.

Answer:

True

Explanation:

Carbon dioxide is transported by the blood in the dissolved form. carbonic anhydrase is the enzyme which is a metalloenzyme having zinc at active site converts carbon dioxide into carbonic acid which dissolves in the blood.

Thus,  

H₂O (l) + CO₂ (g) ⇔ H⁺(aq) + HCO₃²⁻(aq)

The kidneys in the body help to control the acid base balance. The hydrogen ion secretion in the body leads to the generation and reabsorption of the bicarbonate ions to form carbon dioxide in order to nullify the effect of the acid generated and thus the pH of the blood is maintained.

Explanation:

LeChatlier's principle states that any  change in pressure, temperature, or concentration of a reactant applied to a system in equilibrium, the equilibrium will shift so as to tend to counteract the effect of the change.

In our question,[tex]AgCl[/tex] is added.

[tex]AgCl[/tex] is a product.

When product concentration increases,the reaction goes to the left so as to decrease the product concentration.

Adding more silver chloride (AgCl) to the system in equilibrium causes the equilibrium to shift to the left, producing more reactants (AgNO3 and NaCl) and reducing the AgCl.

According to Le Chatelier's Principle, when a change in concentration, pressure, or temperature is applied to a system in equilibrium, the system will adjust itself to counteract the effect of the change. The reaction equation provided is AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq).

If additional silver chloride (AgCl) is added to the beaker, the equilibrium will shift to the left (reactants) to reduce this excess. More reactants AgNO3 and NaCl will be produced, reducing the amount of AgCl. This is because the system strives to maintain equilibrium by utilising the 'extra' AgCl to form more reactants.

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You may find bellow the association of therms with the definitions.

Explanation:

1. standard metric unit of length  - e. meter

2. a proposed explanation for a scientific problem  - b. hypothesis

3. standard unit of volume  - c. liter

4. the curved top surface of a liquid column  - f. meniscus

5. a quantity in an experiment that remains unchanged or constant  - d. control

6. amount of matter in an object  - a. mass

Learn more about:

standard units of measurement

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Answer: ORGANIC ACIDS  

Explanation:

CAM PLANTS CARBOXYLATE ORGANICS ACIDS through the addition of  CO2 to PEP Carboxylase(  a phosphoenolpyruvate carboxylase enzyme present in the mesophyll cells of the cytoplasm in a green plant) to produce Oxaloacetate (organic compound).

CO2 + PEP  ⇒ C4H4O5 (oxaloacetate)

Oxaloacetate is then converted to a similar molecule, Malate (C4H6O5,  another form of organic compound) that can be transported in to the bundle-sheath cells. Malate enters the plasmodesmata and releases the CO2. The CO2 then fixed by rubisco and made into sugars via the Calvin cycle.

Answer:

4.3 x 10⁶ kJ are released

Explanation:

From the balanced chemical equation we know that when 2 moles of hydrogen peroxide decompose, 191 kJ of heat are released. So what we need to calculate is the number of moles the 765 kg of H2O2 represent and calculate the heat released.

Molar Mass H2O2 = 34.01 g/mol

Mass H2O2 = 765 Kg x 1000 g/Kg = 765000 g

moles H2O2 = 1 Mol / 34.01 g x 765000  grams = 22.5 Mol

(-196.1 kJ/ 2 mol H2O2 )  x 22.5 mol H2O2 = -4.3 x 10⁶ kJ

Answer:

Mass of hexamethylenediamine= 13,470.62 g

Mass of adipic acid =  16,940.13 g

Explanation:

Nylon -6,6 is synthesized by poly-condensation of hexamethylenediamine [NH₂-(CH₂)₆-NH₂] and adipic acid (C₆H₁₀O₄).

Both of these are taken in equal equivalents and reacted to form nylon 6,6 and by-product water is also formed.

Molecular mass of hexamethylenediamine [NH₂-(CH₂)₆-NH₂] =116.21 g/mol

Molecular mass of adipic acid (C₆H₁₀O₄) = 146.1412 g/mol

Molecular mass of Nylon 6,6 (C₁₂H₂₀N₂O₂) = 224.3 g/mol

Using unitary method :

Mass of hexamethylenediamine required for 26,000 g of Nylon 6,6 if 116.21 g/mol is required for 224.3 g/mol, is:

= [tex]\frac{26,000 *  116.21}{224.3}[/tex]

= 13,470.62 g

Mass of adipic acid required for 26,000 g of Nylon 6,6 if 146.1412 g/mol is required for 224.3 g/mol, is:

= [tex]\frac{26,000 *  146.1412}{224.3}[/tex]

= 16,940.13 g

Answer:

See the explanation

Explanation:

1) The Lewis structure for  [tex]CO_2[/tex] has a central Carbon atom attached to Oxygen atoms.

In the [tex]CO_2[/tex]  we will have a structure:  O=C=O the central atom "carbon" we will have 2 sigma bonds and 2 pi bonds, therefore, we have an Sp hybridization. For O we have 1 pi and 1 sigma bond, therefore, we have an Sp2 hybridization.

2) These atoms are held together by double bonds.

Again in the structure of [tex]CO_2[/tex]: O=C=O we only have double bonds.

3. Carbon dioxide has a Carbon dioxide has a Linear electron geometry.

Due to the double bonds we have to have a linear structure because in this geometry the atoms will be further apart from each other.

4. The carbon atom is Sp hybridized.

We will have for carbon 2 pi bonds, so we will have an Sp hybridization.

5. Carbon dioxide has two Carbon dioxide has two C(p) - O(p) π bonds and two C(sp) - O(Sp2) σ bonds.

(See figures)

Figure 1: Carbon hybridization

Figure 2: Oxygen hybridization

The Lewis structure of CO₂ has a central carbon atom with double bonds to two oxygen atoms, resulting in a linear geometry and sp hybridization. Each double bond contains one pi bond and one sigma bond.

The Lewis structure for CO₂ features a central carbon atom attached to two oxygen atoms. These atoms are held together by double bonds. The electron geometry of carbon dioxide is linear, which is determined by the Valence Shell Electron Pair Repulsion (VSEPR) theory.

The carbon atom in CO₂ is sp hybridized. In a molecule of carbon dioxide, there are two π (pi) bonds and two σ (sigma) bonds. Each double bond consists of one σ bond and one π bond, contributing to the overall structure and stability of the molecule.

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Answer:

The correct answer is D progesterone control muscle mass.

Explanation:

Progesterone is a steroid hormone synthesized from cholesterol and secreted from corpus lutenum and placenta.progesterone regulate the luteal phase of the menstrual cycle, progesterone helps in the development of secondary sexual characteristics such as breast development,pubic hair development etc.

    On the other hand muscle mass is controlled by the growth hormone released from the anterior lobe of the pituitary gland.

Answer:

efficiency of heating with this oven is 51 %

Explanation:

to raise the temp of 200 ml of coffee from 30°C to 60°C the energy input to microwave oven is:

1100 J/s x 45 = 49,500 J  

AT 100% efficiency

For 1°C the energy required to raise the temperature of 1 ml = 4.2 J

So for 30 C°, 1°C the energy required to raise the temperature of 200 ml =

Q = (4.2) (200)(30) = 25,200 J

efficiency = 25,200/49,500 = 0.51 = 51%  

Answer:

51%

Explanation:

To practice Problem-Solving Strategy 11.1 Energy efficiency problems. Suppose that you have left a 200-mL cup of coffee sitting until it has cooled to 30∘C , which you find totally unacceptable. Your microwave oven draws 1100 W of electrical power when it is running. If it takes 45 s for this microwave oven to raise the temperature of the coffee to 60∘C , what is the efficiency of heating with this oven?

Using the formula  Q=mCdT

Q=Energy (J)

m=mass

C=specific heat capacity

dT=temperature change

but Q=power xtime

to raise the coffee from 30∘C  to 60∘C  requires

1100 J/s x 45 = 49,500 J  

Energy to raise 200ml coffee to 30∘C  is at 4.2j/gC

Q = (4.2)(200)(30) = 25,200 J

Efficiency=output/input

efficiency = 25,200/49,500*100% = 0.51 = 51%

Answer:

[tex]specificheat=0.177J/g^{0}C[/tex]

Explanation:

The heat evolved by lead will be absorbed by water.

The heat evolved by lead will be:

[tex]Q1=massXspecificheatXchangeintemperature[/tex]

[tex]Q1=18.1X(Specificheat)X(99.50-23.67)[/tex]

Heat absorbed by water will be:

[tex]Q2=massXspecificheatX(changeintemperature)[/tex]

[tex]Q2=81.7X4.184(23.67-23)=229.03J[/tex]

We know that

Q1=Q2

[tex]18.1X(Specificheat)X(99.50-23.67)=229.03[/tex]

[tex]1372.523Xspecificheat=229.03[/tex]

[tex]specificheat=0.177J/g^{0}C[/tex]

Answer:

inertia

Explanation:

The principal of inertia explains why objects do not voluntarily change their speed or direction without the influence of an external force. Inertia is not unaffected by other forces in planetary systems such as Earth and is, as such, not really observable on planetary surfaces. This is due to the resistance forces of gravity and friction from both the air and the ground. The drag slows objects down and makes it appear as if a constant force were necessary to keep them in motion.

Answer:

c

Explanation:

Answer:

A. PpCH4 = 1.21 atm, Pp C2H6 = 1.46 atm,  Pp C3H6 = 1.93 atm

B. Pp O2 = 352.17 mmHg

Explanation:

A. First step: Get the total mols of mixture to know the mass of propane.

P . V = n . R . T

T° K = T°C + 273 → 23°C + 273 = 296K

4.60 atm . 10L = n . 0.082 L.atm/mol.K . 296K

(4.60 atm . 10L) / (0.082 mol.K/L.atm . 296K) = n

1.89 mol = n

Mass/Molar weight = mol

Mass CH4 = 16 g/m

Mol CH4: 8g / 16g/m = 0.5 mol

Mass C2H6 = 30 g/m

Mol C2H6 = 0.6 mol

Total mols - Mol CH4 - Mol C2H6 = Mol propane

1.89 mols - 0.5 mol - 0.6 mol = 0.79 mol propane

2nd step: We can use the molar fraction with the partial pressure.

Partial pressure gas / Total pressure = mols gas / total moles

Sum of molar fraction = 1

0.5 / 1.89 + 0.6 /1.89 + 0.79/1.89 = 1

Partial pressure CH4 → Pp CH4 /4.60 atm =  0.5 / 1.89

PpCH4 = (0.5 /1.89) . 4.60 atm = 1.21 atm

Partial pressure C2H6 → Pp C2H6 /4.60atm = 0.6 /1.89

Pp C2H6 = (0.6 /1.89) . 4.60atm = 1.46 atm

Partial pressure C3H6 → Pp C3H6 /4.60atm = 0.79/1.89

Pp C3H6 = (0.79/1.89) . 4.60atm = 1.93 atm

B. 39.8% means a percent of the molar fraction, so the fraction is 0.398

N2 mass /total mass = Partial pressure N2/ Total pressure

0.398 . 585 mmHg = Partial pressure N2

232.83 mmHg = Partial pressure N2

Total pressure - Pp N2 = Pp O2

585 mmHg - 232.82 mmHg = 352.17 mmHg

Answer:

Average atomic mass = 79.9034 amu

Explanation:

The formula for the calculation of the average atomic mass is:

[tex]Average\ atomic\ mass=(\frac {\%\ of\ the\ first\ isotope}{100}\times {Mass\ of\ the\ first\ isotope})+(\frac {\%\ of\ the\ second\ isotope}{100}\times {Mass\ of\ the\ second\ isotope})[/tex]

Given that:

For first isotope:

% = 50.69 %

Mass = 78.9183 amu

For second isotope:

% = 49.31 %

Mass = 80.9163 amu

Thus,  

[tex]Average\ atomic\ mass=\frac{50.69}{100}\times {78.9183}+\frac{49.31}{100}\times {80.9163}\ amu[/tex]

[tex]Average\ atomic\ mass=40.0036+39.8998\ amu[/tex]

Average atomic mass = 79.9034 amu

Final answer:

The average atomic mass of bromine is calculated by taking the sum of the products of each isotope's mass and its abundance in decimal form. The result is an average atomic mass of 79.898 amu for bromine.

Explanation:

To calculate the average atomic mass of bromine based on the given experimental results, we need to consider the masses and relative abundances of its isotopes. By multiplying the mass of each isotope by its abundance (converted to a decimal form) and adding these weighted masses together, we can determine the average atomic mass.

Calculation:

Adding the weighted masses of both isotopes gives us: 39.994 amu + 39.904 amu = 79.898 amu. Thus, the average atomic mass of bromine based on these experiments is 79.898 amu.

Checking for Accuracy:

It is important to make sure that this number makes sense and correlates with the given abundances, ensuring that no mathematical errors have been made.

Answer: the product of this reaction is option B which is carbondioxide and water.

Explanation:A chemical reaction involves the process in which one or more substances, the reactants, are converted to one or more different substances, the products. In the equation above, methane and oxygen gas are the reactants while carbondioxide and water are d products.

Answer:B

Explanation:

co 2 is the same as carbon dioxide and H 20 stand for water.

Answer:

D. 2Cu + O2 = 2CuO

Explanation:

Then CuO, which is black, reacts with CO2 to form CuCO3 which is green.

Answer : The correct chemical reaction is, (D)

Explanation :

Synthesis reaction : It is defined as a chemical reaction where multiple substances or reactants combine to form a single product.

It is represented as,

[tex]X+Y\rightarrow XY[/tex]

When copper react with an oxygen then it react to give copper oxide as a product.

The balanced chemical reaction will be:

[tex]2Cu+O_2\rightarrow 2CuO[/tex]

Hence, the correct chemical reaction is, (D)

Answer:

[tex]\large \text{IO$_{3}$$^{-}$(aq) + 3Sn$^{2+}$(aq) + 6H$^{+}$(aq) $\longrightarrow \,$ I$^{-}$(aq) + 3Sn$^{4+}$(aq) + 3H$_{2}$O(l)}[/tex]

Explanation:

IO₃⁻ + Sn²⁺ ⟶ I⁻ + Sn⁴⁺

1: Separate the equation into two half-reactions.

IO₃⁻ ⟶ I⁻

Sn²⁺ ⟶ Sn⁴⁺

2: Balance all atoms other than H and O.

Done

3: Balance O.

IO₃⁻ ⟶ I⁻ + 3H₂O

Sn²⁺ ⟶ Sn⁴⁺

4: Balance H

IO₃⁻ + 6H ⟶ I⁻ + 3H₂O  

Sn²⁺ ⟶ Sn⁴⁺

5: Balance charge.

IO₃⁻ + 6H⁺ + 6e⁻ ⟶ I⁻ + 3H₂O  

Sn²⁺ ⟶ Sn⁴⁺ + 2e⁻

6: Equalize electrons transferred.

1 × [IO₃⁻ + 6H⁺ + 6e⁻ ⟶ I⁻ + 3H₂O]

3 × [Sn²⁺ ⟶ Sn⁴⁺ + 2e⁻]

7: Add the two half-reactions.

1 × [IO₃⁻ + 6H⁺ + 6e⁻ ⟶ I⁻ + 3H₂O]

3 × [Sn²⁺ ⟶ Sn⁴⁺ + 2e⁻]                                  

      IO₃⁻ + 3Sn²⁺ + 6H⁺ ⟶ I⁻ + 3Sn⁴⁺ + 3H₂O

8: Check mass balance.

 On the left: 1 I, 3 O, 3 Sn, 6 H

On the right: 1 I, 3 O, 3 Sn, 6 H

Step 9: Check charge balance.

  On the left: 1- + 12+ = 11+

On the right: 1-  + 12+ = 11+

The equation is balanced.

[tex]\text{The balanced equation is }\\\large \textbf{IO$_{3}$$^{-}$(aq) + 3Sn$^{2+}$(aq) + 6H$^{+}$(aq) $\longrightarrow \,$ I$^{-}$(aq) + 3Sn$^{4+}$(aq) + 3H$_{2}$O(l)}[/tex]

The reaction in an acid solution involves IO3−(aq) reacting with Sn2+(aq) to form I−(aq) and Sn4+(aq). The complete balanced redox reaction is 2IO3−(aq) + 10H+(aq)+ 6Sn2+(aq) → I−(aq) + 4H2O(l) + 6Sn4+(aq). It is a redox reaction where iodate ions act as strong oxidizing agents.

The reaction under consideration involves the iodate ion (IO3−) reacting with a tin(II) ion (Sn2+) to create iodide (I−) and a tin(IV) ion (Sn4+) in an acidic solution. In an acid solution, water (H2O) and hydrogen ions (H+) play crucial roles, hence they have places in the reaction. The complete balanced redox reaction is:

2IO3−(aq) + 10H+(aq)+ 6Sn2+(aq) → I−(aq) + 4H2O(l) + 6Sn4+(aq)

. To balance this reaction, we consider the change in oxidation state, the law of conservation of charge, and the law of conservation of mass. This reaction is a prominent example of a redox reaction where iodate ions act as strong oxidizing agents, oxidizing Sn2+ to Sn4+.

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Answer:

When magma reaches the surface, its dissolved gas content increases is true

Explanation:

The volcanic eruptions happen because of magma that is expelled on the earth’s surface. At the earth’s depth, all magma have gas dissolved in liquid. When the pressure has decreased the magma rises towards the earth’s surface creating a separate vapour phase.  

As pressure reduces the volume of gas will  expands and giving magma its 'explosive character'. Thus, as magma reaches the surface the dissolved gas content decreases and magma comes out of earth’s surface.

The untrue statement is b, as the dissolved gas content in magma decreases as it reaches the surface due to reduced pressure. Basalt magma has higher temperatures than rhyolite magma. Water reduces the melting temperature of silicate rocks, and increased pressure raises it.

The subject here pertains to volcanic activity and magma characteristics. The statement that is not true is: b. When magma reaches the surface, its dissolved gas content increases. In fact, as magma rises to the surface, the pressure decreases which allows the dissolved gases to escape, thus its dissolved gas content actually decreases. Statements a, c and d are true - Basalt magmas do generally have higher temperatures than rhyolite magmas. Additionally, the presence of water does indeed lower the melting temperature of silicate rocks, and increased pressure results in a higher melting temperature for these rocks.

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Answer:

mass water = 347 x 0.992 = 344.2 g

moles water = 344.2 g / 18.02 g/mol= 19.1

moles C3H8O3 = 164 g / 92.097 g/mol= 1.78

mole fraction water = 19.1 / 19.1 + 1.78 = 0.915

p = 0.915 x 54.74 = 50.07 torr

Explanation:

Final answer:

The mole percent of CaCl2 in the solution would be 100% if we consider only the solute, but this does not account for the water's contribution. If water's contribution to total moles were considered, the mole percent for CaCl2 would be less than 100%.

Explanation:

To calculate the mole percent of CaCl2 in the solution, we must first determine the number of moles of CaCl2.

The molar mass of CaCl2 is approximately 110.98 g/mol (40.08 g/mol for calcium and 35.45 g/mol for each chlorine, with two chlorines). With 6.50 g of CaCl2, the number of moles of CaCl2 is:

6.50 g ÷ 110.98 g/mol = 0.05855 mol

To find the total mass of the solution, the mass of CaCl2 is added to the mass of water. With the water density given as 0.997 g/mL, the mass of 60.0 mL of water is:

60.0 mL × 0.997 g/mL = 59.82 g

The total mass of the solution is thus:

6.50 g (CaCl2) + 59.82 g (H2O) = 66.32 g

To find the mole fraction of CaCl2, we divide the moles of CaCl2 by the total moles (assuming the water in the solution contributes negligibly to the total moles):

Mole fraction of CaCl2 = 0.05855 mol ÷ 0.05855 mol = 1 (since there are no other solutes)

To express this as a mole percent, we multiply the mole fraction by 100%:

Mole percent of CaCl2 = 1 × 100% = 100%

However, this calculation does not account for the water's contribution to the mole fraction. To be precise, the mole fraction and mole percent should include the moles of water as well, but since the question seems to focus solely on CaCl2, the calculation reflects this perspective. If we were to include the moles of water, the mole percent would be significantly less than 100%.

Answer:

[tex]6.0\times 10^3 kJ[/tex] heat is released during the combustion of ethane gas when 14 moles of oxygen are consumed.

Explanation:

[tex]C_2H_6(g)+\frac{7}{2}O_2(g)\rightarrow 2CO_2(g)+3H_2O(l),\Delta H_{rxn}=-1.5\times 10^3 kJ/mol[/tex]

According to reaction, when 7/2 moles of oxygen is consumed by 1 mol of ethane [tex]1.5\times 10^3 kJ[/tex] energy is released.

Energy released when 1 mole of oxygen are consumed: [tex]\frac{1.5\times 10^3 kJ\times 2}{7}[/tex]

Then energy released when 14 moles of oxygen are consumed:

[tex]\frac{1.5\times 10^3 kJ\times 2}{7}\times 14=6.0\times 10^3 kJ[/tex]

[tex]6.0\times 10^3 kJ[/tex] heat is released during the combustion of ethane gas when 14 moles of oxygen are consumed.

Answer:

6.0×10^3 KJmol-1

Explanation:

Equation of the reaction

C2H6(g) + 7/2 O2(g) ------> 2CO2(g) + 3H2O(g)

From the balanced reaction equation:

1 mole of ethane reacts with 3.5 moles of oxygen

x moles of ethane will react with 14 moles of oxygen

x= 14/3.5 = 4 moles of ethane

If heat of combustion of ethane= -1.5*103 kJ/mol

Then for 4 moles of ethane= 4× -1.5*103 kJ/mol= 6.0×10^3 KJmol-1

Answer:

Heat realesed is - 2192.7 kJ

Explanation:

First lets have the chemical equation balanced, and then solve the question based on the fact that the enthalpy change for a reaction is the sum of the enthalpies of formation of products minus reactants.

    B₅H₉ (l) +     O₂ (g) ⇒       B₂O₃ (s) +      H₂O(l)

B atoms we have 5 reactants and 2 products, so the common mltiple is 10 and we have

  2  B₅H₉ (l) +     O₂ (g) ⇒      5 B₂O₃ (s) +      H₂O(l)

Now balance H  by multiplying by 9 the H₂O

  2  B₅H₉ (l) +     O₂ (g) ⇒      5 B₂O₃ (s) +    9 H₂O(l)

Finally, balance the O since we have 24 in products by multiplying by 12 the

O₂ ,

        2  B₅H₉ (l) +  12 O₂ (g) ⇒      5 B₂O₃ (s) +    9 H₂O

ΔHrxn = 5 x ΔHºf B₂O₃  + 9 x   ΔHºf H₂O  -  ( 2 x ΔHºf  B₅H₉ + 12 x  ΔHºf O₂  )

We have all the  ΔHºf s except oxygen but remember the enthalpy of formation of a pure element in its standard estate is cero.

ΔHrxn =  5 mol x ( -1272 kJ/mol )+ 9 mol  x ( -285.4 kJ/mol )   - (  2mol x 732 kJ/mol )

= -8928.6 kJ - 1464  kJ = -10,392 kJ

Now this enthalpy change was based in 2 mol  reacted according to the balanced equation, so for 0.211 mol of  B₅H₉  we will have:

-10,392 kJ/ 2 mol B₅H₉   x 0.211 mol B₅H₉ = - 2192.7 kJ

Answer:

ΔH=-957.41 kJ

Explanation:

The chemical equation is:

B₅H₉ (l) +     O₂ (g) ⇒       B₂O₃ (s) +      H₂O(l)

The law of conservation of matter states that since no atom can be created or destroyed in a chemical reaction, the number of atoms that are present in the reagents has to be equal to the number of atoms present in the products.

Then, you must balance the chemical equation. For that, you must first look at the subscripts next to each atom to find the number of atoms in the equation. If the same atom appears in more than one molecule, you must add its amounts

The coefficients located in front of each molecule indicate the amount of each molecule for the reaction. This coefficient can be modified to balance the equation, just as you should never alter the subscripts.

By multiplying the coefficient mentioned by the subscript, you get the amount of each element present in the reaction.  

So in first place you balance B

2 B₅H₉ (l) +     O₂ (g) ⇒   5 B₂O₃ (s) +      H₂O(l)

Then you balance H

2 B₅H₉ (l) +     O₂ (g) ⇒   5 B₂O₃ (s) +    9  H₂O(l)

Finally you balance O

2 B₅H₉ (l) +    12 O₂ (g) ⇒   5 B₂O₃ (s) +    9  H₂O(l)

Then

Left side: 2*5=10 boron (B), 2*9=18 hydrogen. and 12*2=24 oxygen

Right side: 5*2=10 boron (B), 9*2=18 hydrogen. and 5*3 + 9*1=24 oxygen

Since you have the same amount of elements on each side of the equation, the equation is balanced.

You want to calculate the ∆H (heat of reaction) of the combustion reaction, that is, the heat that accompanies the entire reaction. For that you must make the total sum of all the heats of the products and of the reagents affected by their stoichiometric coefficient (quantity of molecules of each compound that participates in the reaction) and finally subtract them:

Enthalpy of combustion = ΔH = ∑Hproducts - ∑Hreactants

Knowing that:

For the formation of one mole of a pure element the heat of formation is 0, in this case we have as a pure compound the oxygen O₂.

Then:

ΔH= 9 mol*(-285.4 kJ/mol) + 5 mol* (-1,272 kJ/mol) - [2 mol* 73.2 kJ/mol + 12 mol* 0 kJ/mol]

ΔH= -9,075 kJ

If you observe the previous balanced reaction, you can see that 2 moles of B₅H₉ (l) are necessary. And the calculation of the heat of reaction previously carried out is based on this reaction. This ultimately means that the energy that would result in the reaction of 2 moles of B₅H₉ (l) is -9,075 kJ.

To determine the heat that is released when 0.211 mol of B₅H₉ (l) react with excess oxygen, a rule of three is applied as follows: if 2 moles of B₅H₉ (l) produces a heat ΔH of -9,075 kJ, when reacting 0.211 mol of B₅H l (l) how much heat ΔH is released?

ΔH=[tex]\frac{0.211 moles*(-9075)kJ}{2 moles}[/tex]

ΔH=-957.41 kJ

The questioned tackled determining the temperature of gas in a Goodyear blimp using the provided specifications and the ideal gas law: PV=nRT.

The question is about determining the temperature of the helium gas in a Goodyear blimp given certain parameters. Using the ideal gas law: PV=nRT we can calculate the temperature (T). In this scenario, the volume (V) is 5600 m3, the pressure (P) is 1.10x105 Pa and the number of moles (n) can be calculated by dividing the total mass of helium gas by its molar mass. By rearranging the gas law formula, the temperature could be calculated as T=(PV)/(nR), where R is the gas constant.

Following these steps, we can substitute the known values into the equation to solve for the temperature inside the Goodyear blimp. This problem involves concepts of physics, specifically gas laws, and would be covered typically in a college-level physics course.

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Answer:

Cyanophtya

Explanation:

Cyanobacteria also known as Cyanophyta are responsible for fixing nitogen and raising phosphorus level through mineralization they are also called blu-green-algae. They commonly obtain their energy from 'oxygenic' photosynthesis.  

Answer: Solute or solvent

Explanation: A solute is the substance that dissolves to make a solution. The solvent is the solution that does the dissolving.

Answer:

Molarity of triiodide solution is 0.125M

Explanation:

According to balanced equation, 2 moles of [tex]S_{2}O_{3}^{2-}[/tex] completely react with 1 mol of [tex]I_{3}^{-}[/tex].

Moles of [tex]S_{2}O_{3}^{2-}[/tex] in 25.00 mL of 0.300 M of [tex]K_{2}S_{2}O_{3}[/tex] solution = [tex](0.300\times 0.02500)moles=0.0075moles[/tex]

So, 0.0075 moles of [tex]S_{2}O_{3}^{2-}[/tex] completely reacts with [tex](\frac{1}{2}\times 0.0075)moles[/tex] of [tex]I_{3}^{-}[/tex] or 0.00375 moles of [tex]I_{3}^{-}[/tex]

If molarity of [tex]KI_{3}[/tex] solution is S (M) then-

[tex]S\times 0.0300=0.00375[/tex]

or, [tex]S=0.125[/tex]

So, molarity of triiodide solution is 0.125M

To determine the molarity of the KI3 solution, calculate the moles of S2O32- that reacted and use the stoichiometry of the reaction to find the moles of I3-. Then, divide the moles of I3- by the volume of KI3 solution in liters to find the molarity.

The question asks for the molarity of a potassium triiodide (KI3) solution. To find the molarity of the KI3(aq) solution, we need to use the provided stoichiometry of the reaction between thiosulfate (S2O32-) and triiodide (I3-).

The reaction is given as: 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq). Since 25.00 mL of a 0.300 M thiosulfate solution is required to completely react with the KI3 solution, we first calculate the moles of S2O32- reacted.

Moles of S2O32- = 0.025 L * 0.300 mol/L = 0.0075 moles.

According to the balanced equation, 1 mole of I3- reacts with 2 moles of S2O32-. Therefore, we have:

Moles of I3- = 0.0075 moles S2O32- / 2 = 0.00375 moles.

Because 30.00 mL (or 0.03000 L) of KI3 solution contains 0.00375 moles I3-, the molarity of KI3 is calculated by:

Molarity of KI3 = 0.00375 moles / 0.03000 L = 0.125 M.

Answer:

The mole fractions:

[tex]x_{HBr}=\frac{100mol}{318.5}=0.314[/tex]

[tex]x_{Br_2}=\frac{78mol}{318.5}=0.245[/tex]

[tex]x_{H_2O}=\frac{78mol}{318.5}=0.245[/tex]

[tex]x_{O_2}=\frac{62.5mol}{318.5}=0.196[/tex]

Explanation:

The reaction described is:

[tex]2 HBr (g) + 1/2 O_2 (g) \longrightarrow Br_2 (g) + H_2O (g)[/tex]

The limiting reactant is the HBr (oxygen is in excess).

a) The mass (in moles) balance for this sistem:

[tex]n_{Br_2}=\frac{ 1 mol Br_2}{1 mol HBr} *n_{HBr}*0.78[/tex]

(the 0.78 is because of the fractional conversion)

[tex]n_{O_2}=\frac{ 0.5 mol O_2}{1 mol HBr} *n_{HBr}*1.25[/tex]

(the 1.25 is because of the oxygen excess)

[tex]n_{H_2O}=\frac{ 1 mol H_2O}{1 mol Br_2} *n_{Br_2}[/tex]

There is only one degree of freedom in this sistem, you can either deffine the moles of HBr you have or the moles of Br2 you want to produce. The other variables are all linked by the equations above.

b) Base of calculation 100 mol of HBr:

[tex]nn_{HBr}=100 mol HBr[/tex]

[tex]n_{Br_2}=\frac{ 1 mol Br_2}{1 mol HBr} *100mol HBr*0.78[/tex]

[tex]n_{Br_2}=78 mol Br2[/tex]

[tex]n_{O_2}=\frac{ 0.5 mol O_2}{1 mol HBr} *100 mol HBr*1.25[/tex]

[tex]n_{O_2}=62.5 mol O_2[/tex]

[tex]n_{H_2O}=n_{Br_2}= 78 mol[/tex]

[tex]n_{total}=(78+78+100+62.5)mol= 318.5mol[/tex]

The mole fractions:

[tex]x_{HBr}=\frac{100mol}{318.5}=0.314[/tex]

[tex]x_{Br_2}=\frac{78mol}{318.5}=0.245[/tex]

[tex]x_{H_2O}=\frac{78mol}{318.5}=0.245[/tex]

[tex]x_{O_2}=\frac{62.5mol}{318.5}=0.196[/tex]

Answer: Relative humidity

Explanation:

Relative humidity (RH) is the ratio of the partial pressure of water vapor to the equilibrium vapor pressure of water at a given temperature. Relative humidity depends on temperature and the pressure of the system of interest. The same amount of water vapor has higher relative humidity in cool air than in warm air. A related parameter to that regard is that of dew point.