An aluminum atom has a mass of 4.48 * 10-23 g and a small airplane has a mass of 5000 kg. Use this information to answer the questions below. Be sure your answers have the correct number of significant digits.

(a) What is the mass of 1 mole of aluminum atoms?
(b) How many moles of aluminum atoms have a mass equal to the mass of a small airplane?

Answer:

Q=7200 W

q=7200/72=100 [tex]W/m^2[/tex]

Explanation:

Given that

ΔT=15° C

Thickness ,t=15 cm

Thermal conductivity ,K=1 W/m.°C

Height,h=6 m

Length ,L=12 m

As we know that heat conduction through wall given as

[tex]Q=\dfrac{KA}{t}\Delta T[/tex]

Now by putting the values

A= 6 x 12 =72 [tex]m^2[/tex]

[tex]Q=\dfrac{KA}{t}\Delta T[/tex]

[tex]Q=\dfrac{1\times 72}{0.15}\times 15\ W[/tex]

Q=7200 W

Q is the total heat transfer.

Heat flux q

 q=Q/A [tex]W/m^2[/tex]

q=7200/72=100 [tex]W/m^2[/tex]

q is the heat flux.

As w know that heat flux(q) is the heat transfer rate from per unit area and on the other hand heat transfer(Q) is the total heat transfer from the surface.

Heat flux q=Q/A

That is why these both are different.

Answer:

The answer is 130.953 g of hydrogen gas.

Explanation:

Hydrogen gas is formed by two atoms of hydrogen (H), so its molecular formula is H₂. We can calculate is molecular weight as the product of the molar mass of H (1.008 g/mol):

Molecular weight H₂= molar mass of H x 2= 1.008 g/mol x 2= 2.01568 g

Finally, we obtain the number of mol of H₂ there is in the produced gas mass (264 g) by using the molecular weight as follows:

mass= 264 g x 1 mol H₂/2.01568 g= 130.9731703 g

The final mass rounded to 3 significant digits is 130.973 g

To find the number of moles of hydrogen gas produced from 264 grams, divide the mass by the molar mass of hydrogen (2.02 g/mol), resulting in approximately 130.7 moles of hydrogen gas to three significant digits.

To calculate the number of moles of hydrogen gas (H₂) produced from 264 grams of hydrogen gas, you would use the molar mass of H₂ which is approximately 2.02 g/mol (1 mole of H₂ = 2.02 grams). Using the formula:

number of moles = mass of substance (g) / molar mass (g/mol)

We find the number of moles of hydrogen gas to be:

number of moles = 264 g / 2.02 g/mol

After performing the division, this gives us approximately 130.7 moles of H₂.

This result is to three significant digits, aligned with the precision provided by the initial mass of the hydrogen gas.

Answer:

k = 0.0198 s⁻¹

t = 74.25 seconds

Explanation:

Given that:

Half life = 35.0 s

[tex]t_{1/2}=\frac {ln\ 2}{k}[/tex]

Where, k is rate constant

So,  

[tex]k=\frac {ln\ 2}{t_{1/2}}[/tex]

[tex]k=\frac {ln\ 2}{35.0}\ s^{-1}[/tex]

The rate constant, k = 0.0198 s⁻¹

Using integrated rate law for first order kinetics as:

[tex][A_t]=[A_0]e^{-kt}[/tex]

Where,  

[tex][A_t][/tex] is the concentration at time t

[tex][A_0][/tex] is the initial concentration

Given:

77.0 % is decomposed which means that 0.77 of [tex][A_0][/tex] is decomposed. So,

[tex]\frac {[A_t]}{[A_0]}[/tex] = 1 - 0.77 = 0.23

t = ?

[tex]\frac {[A_t]}{[A_0]}=e^{-k\times t}[/tex]

[tex]0.23=e^{-0.0198\times t}[/tex]

t = 74.25 seconds

When in a reaction heat is a reactant then the reaction is called thermal decomposition reaction. The first-order rate constant is 0.0198 per second and the time required is 74.25 seconds.

The rate constant is the specific rate that is the proportionality constant in a reaction and depicts the relation between the chemical reaction rate and the concentration of the reactants.

Rate constant can be given as,

[tex]\rm t\dfrac{1}{2} = \dfrac{ln 2}{k}[/tex]

The half-life of the reaction is 35 seconds.

Substituting values in the above equation:

[tex]\begin{aligned}\rm k &= \rm \dfrac{ln\;2}{t\frac{1}{2}}\\\\&= \dfrac{\rm ln\2}{35}\\\\&= 0.0198 \;\rm s^{-1}\end{aligned}[/tex]

The time taken can be calculated by the rate law for first order:

[tex]\rm [A_{t}] = [A_{o}]e^{-kt}[/tex]

Here,

Solving for time (t):

[tex]\begin{aligned}\rm \dfrac {[A_{t}]}{[A_{o}]} &= 1 - 0.77\\\\0.23 &= \rm e ^{-0.0198 \times t}\\\\\rm t &= 74.25\;\rm seconds\end{aligned}[/tex]

Therefore, the rate constant is 0.0198 per second and the time taken is 74.25 seconds.

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Answer:

pH of solution is 3.80

Explanation:

[tex]pH=pK_{a}(formic acid)+log(\frac{C_{formate}}{C_{formic acid}})[/tex]

where, C stands for concentration

So, [tex]pH=3.75+log(\frac{0.055}{0.049})=3.80[/tex]

Answer:

the correct answer is option 'b': More than

Explanation:

The 2 situations are represented in the attached figures below

When an object is placed in air it is acted upon by force of gravity of earth which is measured as weight of the object.

While as when any object is submerged partially or completely in any fluid the fluid exerts a force in upward direction and this force is known as force of buoyancy and it's magnitude is given by Archimedes law as equal to the weight of the fluid that the body displaces, hence the effective force in the downward direction direction thus the apparent weight of the object in water decreases.

Answer:

b)boiling water

Explanation:

Answer: Option (d) is the correct answer.

Explanation:

The given reaction will be as follows.

       [tex]Ba(OH)_{2}(aq) + H_{2}SO_{4}(aq) \rightarrow BaSO_{4}(s) + 2H_{2}O(l)[/tex]

In the ionic form, the equation will be as follows.

           [tex]Ba^{2+}(aq) + SO^{2-}_{4}(aq) \rightarrow BaSO_{4}(s)[/tex] ........ (1)

           [tex]H^{+}(aq) + OH^{-}(aq) \rightarrow H_{2}O(l)[/tex] ............ (2)

Hence, for the net ionic equation we need to add both equation (1) and (2). Therefore, the net ionic equation will be as follows.

     [tex]Ba^{2+}(aq) + SO^{2-}_{4}(aq) + H^{+}(aq) + OH^{-}(aq) \rightarrow BaSO_{4}(s) + H_{2}O(l)[/tex]        

Now, balancing the atoms on both the sides we get the net ionic equation as follows.

         [tex]Ba^{2+}(aq) + SO^{2-}_{4}(aq) + 2H^{+}(aq) + 2OH^{-}(aq) \rightarrow BaSO_{4}(s) + 2H_{2}O(l)[/tex]          

The correct net ionic reaction for the experiment is H+(aq) + OH-(aq) → H2O(l), an example of an acid-base neutralization reaction. The other options included the formation of a precipitate, which is not part of the net ionic reaction.

Based on the provided options, the correct net ionic reaction for the experiment seems to be H+(aq) + OH-(aq) → H2O(l). This reaction is a classic example of an acid-base neutralization reaction, where an acid (H+) and a base (OH-) react to form water. The other two reactions involve the formation of a precipitate (BaSO4), but the full reaction is simplified to leave out the precipitate ions on either side. This does not occur in the first reaction. Hence, the first reaction is the correct net ionic reaction for this experiment.

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Answer : The volume of [tex]CO_2[/tex] gas is 1.00 L

Explanation :

First we have to determine the moles of [tex]C_3H_4PO_7^{3-}[/tex].

Molar mass of [tex]C_3H_4PO_7^{3-}[/tex] = 182.9 g/mole

[tex]\text{ Moles of }C_3H_4PO_7^{3-}=\frac{\text{ Mass of }C_3H_4PO_7^{3-}}{\text{ Molar mass of }C_3H_4PO_7^{3-}}=\frac{15.0g}{182.9g/mole}=0.0820moles[/tex]

Now we have to calculate the moles of [tex]CO_2[/tex].

The given balanced chemical reaction is:

[tex]C_5H_8P_2O_{11}^{4-}(aq)+H_2O(aq)+CO_2(g)\rightarrow 2C_3H_4PO_7^{3-}(aq)+2H^+(aq)[/tex]

From the reaction we conclude that,

As, 2 moles of [tex]C_3H_4PO_7^{3-}[/tex] produce from 1 mole of [tex]CO_2[/tex]

So, 0.0820 moles of [tex]C_3H_4PO_7^{3-}[/tex] produce from [tex]\frac{0.0820}{2}=0.041moles[/tex] of [tex]CO_2[/tex]

Now we have to calculate the volume of [tex]CO_2[/tex] gas.

Using ideal gas equation:

[tex]PV=nRT[/tex]

where,

P = pressure of gas = 1.00 atm

V = volume of gas = ?

T = temperature of gas = 298 K

n = number of moles of gas = 0.041 mole

R = gas constant = 0.0821 L.atm/mole.K

Now put all the given values in the ideal gas equation, we get:

[tex](1.00atm)\times V=(0.041mole)\times (0.0821L.atmK^{-1}mol^{-1})\times (298K)[/tex]

[tex]V=1.00L[/tex]

Therefore, the volume of [tex]CO_2[/tex] gas is 1.00 L

Answer: The mass of decane produced is [tex]1.743\times 10^2g[/tex]

Explanation:

To calculate the number of moles, we use the equation:  

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]       ......(1)

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

[tex]\text{Moles of }H_2=\frac{2.45g}{2g/mol}=1.225mol[/tex]

The chemical equation for the hydrogenation of decene follows:

[tex]C_{10}H_{20}(l)+H_2(g)\rightarrow C_{10}H_{22}(s)[/tex]

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = [tex]\frac{1}{1}\times 1.225=1.225mol[/tex] of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

[tex]1.225mol=\frac{\text{Mass of decane}}{142.30g/mol}\\\\\text{Mass of carbon dioxide}=(1.225mol\times 142.30g/mol)=174.3g=1.743\times 10^2g[/tex]

Hence, the mass of decane produced is [tex]1.743\times 10^2g[/tex]

Answer:

6298702 potassium atoms would have to be laid side by side to span a distance of 2,91 mm

Explanation:

If the radius of a potassium atom is 231 pm, then the diameter would be:

d = 2r = 2*(231) = 462 pm

So each potassium atom occupies a space of 462 pm, we can express this relationship as follows:

[tex]\frac{1 potassium atom}{462 pm}[/tex]

To solve this problem, we'll use the following conversion factors:

1 pm = 1×E−12 m

1000 mm = 1 m

We begin to accommodate all our relationships starting from that numerical expression that is not written as a relationship (usually the one in the question), and in such a way that the units are eliminated between them.

[tex]2, 91 mm * \frac{1 m}{1000 mm}*\frac{ 1 pm}{1*10^{-12}m }*\frac{1 potassium atom}{462 pm}= 6298701.3[/tex] potassium atoms

So, we'll need 6298702 potassium atoms to span a distance of 2,91 mm

Explanation:

The electronegativity values of the 5d series are very high because the size of the 5d orbitals are much larger as compared to the size of the 3d and 4d orbitals. As a consequence of this, the shielding capacity of 5d elements are low or these elements are not effective at shielding the nuclear charge . Thus, this causes the increase in the effective nuclear charge which makes the electronegativity values to increase steeply from the Lutetium (1.27) to the Gold (2.54).

Answer:

Math expression: [tex]=\frac{0.77\ g/ml*5200\ ml}{1\ g} *45.0\ kJ[/tex]

Explanation:

Given:

Energy produced per gram of gasoline = 45.0 kJ

Density of gasoline = 0.77 g/ml

Volume of gasoline = 5.2  L=5200 ml

To determine:

The amount of energy produced by burning 5.2 L gasoline

Calculation set-up:

1. Calculate the mass (m) of gasoline given the density (d) and volume (v)

[tex]m = d*v\\\\m = 0.77 g/ml*5200 ml[/tex]

2. Calculate the amount of energy produced

[tex]=\frac{0.77\ g/ml*5200\ ml}{1\ g} *45.0\ kJ=180180 kJ[/tex]

Answer: The correct answer is Option d.

Explanation:

We are given:

Mass percentage of [tex]CH_4[/tex] = 20 %

So, mole fraction of [tex]CH_4[/tex] = 0.2

Mass percentage of [tex]C_2H_4[/tex] = 30 %

So, mole fraction of [tex]C_2H_4[/tex] = 0.3

Mass percentage of [tex]C_2H_2[/tex] = 35 %

So, mole fraction of [tex]C_2H_2[/tex] = 0.35

Mass percentage of [tex]C_2H_2O[/tex] = 15 %

So, mole fraction of [tex]C_2H_2O[/tex] = 0.15

We know that:

Molar mass of [tex]CH_4[/tex] = 16 g/mol

Molar mass of [tex]C_2H_4[/tex] = 28 g/mol

Molar mass of [tex]C_2H_2[/tex] = 26 g/mol

Molar mass of [tex]C_2H_2O[/tex] = 48 g/mol

To calculate the average molecular mass of the mixture, we use the equation:

[tex]\text{Average molecular weight of mixture}=\frac{_{i=1}^n\sum{\chi_im_i}}{n_i}[/tex]

where,

[tex]\chi_i[/tex] = mole fractions of i-th species

[tex]m_i[/tex] = molar masses of i-th species

[tex]n_i[/tex] = number of observations

Putting values in above equation:

[tex]\text{Average molecular weight}=\frac{(\chi_{CH_4}\times M_{CH_4})+(\chi_{C_2H_4}\times M_{C_2H_4})+(\chi_{C_2H_2}\times M_{C_2H_2})+(\chi_{C_2H_2O}\times M_{C_2H_2O})}{4}[/tex]

[tex]\text{Average molecular weight of mixture}=\frac{(0.20\times 16)+(0.30\times 28)+(0.35\times 26)+(0.15\times 42)}{4}\\\\\text{Average molecular weight of mixture}=6.75[/tex]

Hence, the correct answer is Option d.

The average molecular weight of the gaseous mixture is approximately 27 g/mol, which is not one of the provided options.

The average molecular weight (MW) of a mixture can be calculated as the sum of the weight percentages of each component multiplied by its respective molecular weight divided by 100. For the given mixture, the molecular weights of the components are:
CH4 = 16 g/mol
C2H4 = 28 g/mol
C2H2 = 26 g/mol
C2H2O = 42 g/mol.

We multiply the weight percentages with the molecular weights of each component and then sum them up:

Hence, the average molecular weight of the mixture is 27 g/mol. Thus, none of the options provided (a-d) is correct.

Answer:

a) 5,3176x10⁻⁴ moles

b) 6,85x10⁻⁴ moles

c) The appropriate formula to calculate is Henderson-Hasselbalch.

d) pH = 4,86. Acidic solution but slighty

Explanation:

a) moles of acetic acid:

9,20x10⁻³L × 57,8x10⁻³M = 5,3176x10⁻⁴ moles

b) moles of sodium acetate:

56,2x10⁻³g ÷ 82,0 g/mole = 6,85x10⁻⁴ moles

c) The appropriate formula to calculate is Henderson-Hasselbalch:

pH= pka + log₁₀ [tex]\frac{[A^-]}{[HA]}[/tex]

d) pH= 4,75 + log₁₀ [tex]\frac{[6,85x10_{-4}]}{[5,3176x10_{-4}]}[/tex]

pH = 4,86

3 < pH < 7→ Acidic solution but slighty

I hope it helps!

Answer:

Explanation:

The equilibrium relevant for this problem is:

H₂PO₄⁻ ↔ HPO₄⁻² + H⁺

The Henderson–Hasselbalch (H-H) equation is needed to solve this problem:

pH= pka + [tex]log\frac{[A^{-} ]}{[HA]}[/tex]

In this case, [A⁻] = [HPO₄⁻²], [HA] = [H₂PO₄⁻], pH = 7.4; from literature we know that pka=7.21.

We use the H-H equation to describe [HPO₄⁻²] in terms of  [H₂PO₄⁻]:

[tex]7.4=7.21+log\frac{[HPO4^{-2} ]}{[H2PO4^{-} ]} \\0.19=log\frac{[HPO4^{-2} ]}{[H2PO4^{-} ]} \\10^{0.19}= \frac{[HPO4^{-2} ]}{[H2PO4^{-} ]} \\1.549*[H2PO4^{-} ]=[HPO4^{-2} ][/tex]

The problem tells us that the concentration of phosphate is 1 mM, which means:

[HPO₄⁻²] + [H₂PO₄⁻] = 1 mM = 0.001 M

In this equation we can replace [HPO₄⁻²] with the term expressed in the H-H eq:

1.549 * [H₂PO₄⁻] + [H₂PO₄⁻] = 0.001 M

2.549 * [H₂PO₄⁻] = 0.001 M

[H₂PO₄⁻] = 3.923 * 10⁻⁴ M

With the value of [H₂PO₄⁻] we can calculate [HPO₄⁻²]:

[HPO₄⁻²] + 3.923 * 10⁻⁴ M = 0.001 M

[HPO₄⁻²] = 6.077 * 10⁻⁴ M

With the concentrations, the molecular weight, and the volume, we calculate the mass of each reagent:

Explanation:

The given data is as follows.

      Mass of antimony = 19.75 g

      Molar mass of Sb = 121.76 g/mol

Therefore, calculate number of moles of Sb as follows.

                    Moles of Sb = [tex]\frac{mass}{\text{molar mass}}[/tex]

                                         = [tex]\frac{19.75 g}{121.76 g/mol}[/tex]

                                         = 0.162 mol

Mass of oxygen given is 6.5 g and molar mass of oxygen is 16 g/mol. Hence, moles of oxygen will be calculated as follows.

           Moles of oxygen = [tex]\frac{mass}{\text{molar mass}}[/tex]

                                         = [tex]\frac{6.5 g}{16 g/mol}[/tex]

                                         = 0.406 mol

Hence, ratio of moles of Sb and O will be as follows

                          Sb : O

                      [tex]\frac{0.162}{0.162} : \frac{0.406}{0.162}[/tex]

                           1 : 2.5

We multiply both the ratio by 2 in order to get a whole number. Therefore, the ratio will be 2 : 5.

Thus, we can conclude that the empirical formula of the given oxide is [tex]Sb_{2}O_{5}[/tex].

Answer:

To know when a central atom in a lewis structure will have more than 8 electrons it is important to know where is the element at the periodic table and the orbital configuration of the atom.

Explanation:

The octet rule establishes that an atom could win, lose, or share electrons with other atoms till every atom have eight valence electrons. However exist exceptions to the octet rule. Some elements like Be, B and Al are stable with only six valence electrons because these three elements are small and with low electronegativity. On the other hand, some elements from the 3d orbital could expand their octet and still be stable, like S in SF6. This happens because elements from 3d orbital have enough space to suit more electrons.

Answer:

[Ca²⁺] = 0.068 M

Explanation:

The concentration of the calcium ion will be equal to the amount of calcium in CaCl₂, divided by the total volume:

C = n/V

When CaCl₂ dissociates in water, one mole of calcium ion is produced for every mole of CaCl₂, so the molar ratio of CaCl₂ to Ca²⁺ is 1:1. The moles of Ca²⁺ are calculated as follows:

(0.18 mol/L)(30.00 mL) = 5.4 mmol CaCl₂ = 5.4 mmol Ca²⁺

The total volume is (50.00 mL + 30.00 mL) = 80.00 mL

Thus, the concentration of Ca²⁺ is:

C = n/V = (5.4 mmol)/(80.00 mL) = 0.068 M

Answer:

5.65

Explanation:

Given that:

[tex]pK_{b}\ of\ CH_3NH_2=3.44[/tex]

[tex]K_{b}\ of\ CH_3NH_2=10^{-3.44}=3.6308\times 10^{-4}[/tex]

[tex]K_a\ of\ CH_3NH_3^+Cl^-=\frac {K_w}{K_b}=\frac {10^{-14}}{3.6308\times 10^{-4}}=2.7542\times 10^{-11}[/tex]

Concentration = 0.18 M

Consider the ICE take for the dissociation as:

                              [tex]CH_3NH_3^+[/tex]   ⇄     H⁺ +  [tex]CH_3NH_2[/tex]

At t=0                           0.18                 -                            -

At t =equilibrium        (0.18-x)                x                         x            

The expression for dissociation constant of acetic acid is:

[tex]K_{a}=\frac {\left [ H^{+} \right ]\left [CH_3NH_2 \right ]}{[CH_3NH_3^+]}[/tex]

[tex]2.7542\times 10^{-11}=\frac {x^2}{0.18-x}[/tex]

x is very small, so (0.18 - x) ≅ 0.18

Solving for x, we get:

x = 0.2227×10⁻⁵  M

pH = -log[H⁺] = -log(0.2227×10⁻⁵) = 5.65

Answer:

b. halogens

Explanation:

The elements of group 17 are called halogens. These are six elements Fluorine, Chlorine, Bromine, Iodine, Astatine. Halogens are very reactive these elements cannot be found free in nature. Their chemical properties are resemble greatly with each other. As we move down the group in periodic table size of halogens increases that's way fluorine is smaller in size as compared to other halogens elements. Their boiling points also increases down the group which changes their physical states.  

Answer:

Point source pollution:

 If pollution comes from a fix source then is called point source pollution.It have a specific location where pollution comes.

Ex: Air pollution ,water pollution.

Non point source pollution:

 If pollution comes from number of sources then is called point source pollution.This pollution does not have a specific point of source.

Ex: Spills ,leaks ,Sewage over flow etc.

Answer:

Defined as under.

Explanation:

Answer: The number of carbon and oxygen atoms in the given amount of carbon dioxide is [tex]4.72\times 10^{22}[/tex] and [tex]9.44\times 10^{22}[/tex] respectively

Explanation:

To calculate the number of moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]

Given mass of carbon dioxide gas = 3.45 g

Molar mass of carbon dioxide gas = 44 g/mol

Putting values in above equation, we get:

[tex]\text{Moles of carbon dioxide gas}=\frac{3.45g}{44g/mol}=0.0784mol[/tex]

1 mole of carbon dioxide gas contains 1 mole of carbon and 2 moles of oxygen atoms.

According to mole concept:

1 mole of a compound contains [tex]6.022\time 10^{23}[/tex] number of molecules

So, 0.0784 moles of carbon dioxide gas will contain [tex]1\times 0.0784\times 6.022\times 10^{23}=4.72\times 10^{22}[/tex] number of carbon atoms and [tex]2\times 0.0784\times 6.022\times 10^{23}=9.44\times 10^{22}[/tex] number of oxygen atoms

Hence, the number of carbon and oxygen atoms in the given amount of carbon dioxide is [tex]4.72\times 10^{22}[/tex] and [tex]9.44\times 10^{22}[/tex] respectively

Answer: [tex]4.4\times 10^{2}[/tex]

Explanation:

The chemical reaction follows the equation:

     [tex]2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)[/tex]

t = 0 [tex]5.000\times 10^{-3}[/tex] [tex]2.50\times 10^{-3}[/tex]    0

At eqm [tex](5.000\times 10^{-3}-2x)[/tex] [tex](2.50\times 10^{-3}-x)[/tex]   (2x)      

The expression for [tex]K_c[/tex] for the given reaction follows:

[tex]K_c=\frac{[SO_3]^2}{[SO_2]^2[O_2]}[/tex]

[tex]K_c=\frac{[2x]^2}{[5.000\times 10^{-3}-2x]^2[2.50\times 10^{-3}-x]}[/tex]

Given : [tex][SO_2]_{eqm}=2.80\times 10^{-3}[/tex]

[tex]5.000\times 10^{-3}-2x=2.80\times 10^{-3}[/tex]

[tex]x=1.1\times 10^{-3}[/tex]

Putting the values we get:

[tex]K_c=\frac{[2\times 1.1\times 10^{-3}]^2}{[5.000\times 10^{-3}-2\times 1.1\times 10^{-3}]^2[2.50\times 10^{-3}-1.1\times 10^{-3}]}[/tex]

[tex]K_c=4.4\times 10^2[/tex]

Therefore, the equilibrium concentration [tex]4.4\times 10^{2}[/tex]

Answer:

time = Molecules/Rate => 0.0079 segs

Explanation:

Rate = 7.64 * 10^19 molecules/segs

Molecules = 6.02 * 10^17 molecules

time = #?

time = Molecules/Rate => 0.0079 segs

The dimensional analysis calculates the variable from the given data. A chemical reaction with a reaction rate of 7.64 X 10¹⁹ will take 0.0079 seconds to consume 6.02 x 10¹⁷ molecules of reactant.

The reaction rate has been defined by the speed or the time taken for the product to get produced by the reactant undergoing the chemical reaction. The rate of reaction depends on the concentration of the reactants.

Given,

Rate of reaction = 7.64 x 10¹⁹ molecules per second

Molecules = 6.02 × 10¹⁷ molecules

Time is calculated by the dimensional analysis as,

Time = Molecules ÷ Rate

= 6.02 × 10¹⁷ molecules ÷ 7.64 x 10¹⁹ molecules per second

= 0.0079 seconds

Therefore, it will take 0.0079 seconds for 6.02 x 10¹⁷ molecules of reactant to yield the product.

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Answer: The correct answer is Option C.

Explanation:

The chemical formula for trinitrotoluene is [tex]C_7H_5N_3O_6[/tex]

In 1 mole of TNT, 7 moles of carbon atom, 5 moles of hydrogen atom, 3 moles of nitrogen atom and 6 moles of oxygen atom are present.

We know that:

Mass of trinitrotoluene = 227.1 g/mol

Mass of carbon = 12.01 g/mol

We are given:

Mass of TNT = 57.6 grams

To calculate the mass of carbon in given amount of TNT, we apply unitary method:

In 227.1 grams of TNT, amount of carbon present is = [tex](7\times 12.01)=84.07g[/tex]

So, in 57.6 grams of TNT, the amount of carbon present is = [tex]\frac{84.07g}{227.1g}\times 57.6g=21.3g[/tex]

Hence, the correct answer is Option C.

Answer: Freezing point of a solution will be [tex]-1.16^0C[/tex]

Explanation:

Depression in freezing point is given by:

[tex]\Delta T_f=i\times K_f\times m[/tex]

[tex]\Delta T_f=T_f^0-T_f=(5.50-T_f)^0C[/tex] = Depression in freezing point

i= vant hoff factor = 1 (for non electrolyte)

[tex]K_f[/tex] = freezing point constant = [tex]5.12^0C/m[/tex]

m= molality

[tex]\Delta T_f=i\times K_f\times \frac{\text{mass of solute}}{\text{molar mass of solute}\times \text{weight of solvent in kg}}[/tex]

Weight of solvent (benzene)= 1480 g =1.48 kg

Molar mass of solute (octane) = 114.0 g/mol

Mass of solute (octane) = 220 g

[tex](5.50-T_f)^0C=1\times 5.12\times \frac{220g}{114.0 g/mol\times 1.48kg}[/tex]

[tex](5.50-T_f)^0C=6.68[/tex]

[tex]T_f=-1.16^0C[/tex]

Thus the freezing point of a solution will be [tex]-1.16^0C[/tex]

Answer:

[tex]V=\dfrac{2}{9\ \mu}R^2g(\rho_d-\rho_f)[/tex]

Explanation:

Given that

Radius =R

[tex]Density\ of\ droplet=\rho_d[/tex]

[tex]Density\ of\ fluid=\rho_f[/tex]

When drop let will move downward then so

[tex]F_{net}=F_{weight}-F_{b}-F_d[/tex]

Fb = Bouncy force

Fd = Drag force

We know that

[tex]F_b=\dfrac{4\pi }{3}R^3\ \times \rho_f\times g[/tex]

[tex]F_{weight}=\dfrac{4\pi }{3}R^3\ \times \rho_d\times g[/tex]

[tex]F_{d}=6\pi \mu\ R\ V[/tex]

μ=Dynamic viscosity of fluid

V= Terminal velocity

So at the equilibrium condition

[tex]F_{net}=F_{weight}-F_{b}-F_d[/tex]

[tex]0=F_{weight}-F_{b}-F_d[/tex]

[tex]F_{weight}=F_{b}+F_d[/tex]

[tex]\dfrac{4\pi }{3}R^3\ \times \rho_d\times g=\dfrac{4\pi }{3}R^3\ \times \rho_f\times g+6\pi \mu\ R\ V[/tex]

So

[tex]V=\dfrac{2}{9\ \mu}R^2g(\rho_d-\rho_f)[/tex]

This is the terminal velocity of droplet.

Answer:

a) Reaction is not at equilibrium

b) Reaction will move towards backward direction

Explanation:

[tex]PCl_5(g) \rightarrow PCl_3(g) + Cl_2(g)[/tex]

Equilibrium constant = 26

[tex]Reaction\ quotient (Q) = \frac{[p_{PCl_3}]\times [p_{Cl_2}]}{[p_{PCl_5}]}[/tex]

[tex][p_{PCl_5}] = 0.012 atm[/tex]

[tex][p_{PCl_3}]= 0.90 atm[/tex]

[tex][p_{Cl_2}]= 0.45 atm[/tex]

[tex]Reaction\ quotient (Q) = \frac{[p_{PCl_3}]\times [p_{Cl_2}]}{[p_{PCl_5}]}[/tex]

[tex]Reaction quotient (Q) =\frac{0.90\times 0.45} {0.012} = 33.75[/tex]

As reaction quotient (Q) is more than equilibrium constant, so reaction is not at equilibrium and reaction will move towards backward direction.

Explanation:

Acid spills

These types of spills should be neutralized with base like sodium bicarbonate and then must be cleaned up by using paper towel or  sponge. Strong base like sodium hydroxide must not be used to neutralize. Best base to use is sodium bicarbonate which has much less chance of the injury.

Mercury spills

Mercury is found commonly in  the thermometers. If one have mercury spill, it must be cleaned up immediately with  either commercial product like Hg Aborb ™ or by using elemental sulfur. Mercury sponges  can also be purchased that form amalgam with liquid mercury and thus trapping it on surface of sponge.

Answer: NaCl (s) → NaCl (aq)

Explanation:

Entropy is often associated with the disorder or randomness of a system. Therefore, in each reaction, it is necessary to evaluate if the disorder increases or decreases to understand what happens to the entropy:

1) KCl (aq) + AgNO₃ (aq) → KNO₃ (aq) + AgCl (s) - In this reaction, we have only aqueous reactants in the beginning and in the product we have a precipitate. The solid state is more organised than the liquid, consequently, the entropy decreases.

2) NaCl (s) → NaCl (aq) - In this case, oposite to the first one, we go from a solid state to an aqueous state. The solvation of the ions Na⁺ and Cl⁻ is random while the solid state is very organised. Therefore, in this reaction the entropy increases.

3) 2NaOH (aq) + CO₂ (g) → Na₂CO₃ (aq) + H₂O (l) - In this reaction, the reactants have higher entropy because of the gas CO₂. Therefore, the entropy decreases.

4) C₂H₅OH (g) → C₂H₅OH (l) -  In this reaction, the reactant is a gas and the product a liquid. Therefore, the entropy decreases.