For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2(g) + 3H2(g) -----> 2NH(g).the standard change in Gibbs free energy is ΔG° = -32.8 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are. Pn2= 0.1 atm, Ph2=.1 atm and P (NH3)=.6 atm. delta g=?

Answer:

The answer to your question is P = 17.73 atm

Explanation:

V = 250 ml = 0.25 liters (L)

mass = 3.4 g

Temperature = 45°C = 45 + 273 = 318°K

Pressure = ?

R = 0.082 atm L / mol°K

Atomic mass Ne = 20.18 g

Process

1.- Calcule moles of Neon

                           20.18 g of Ne ------------------ 1 mol

                              3.4 g of Ne -------------------  x

                                            x = (3.4 x 1)/20.18

                                            x = 0.17 moles of Neon

2.- Find pressure

Ideal gases formula             PV = nRT

                                            [tex]P = \frac{nRT}{V}[/tex]

                                            [tex]P = \frac{(0.17)(0.082)(318)}{0.25}[/tex]

                                            [tex]P = \frac{4.433}{0.25}[/tex]        

                                                  P = 17.73 atm                                                                          

To calculate the pressure of the neon gas inside the flask, you can use the ideal gas law equation PV = nRT.

To calculate the pressure of the neon gas, we can use the ideal gas law equation: PV = nRT. The given volume is 250 mL, which needs to be converted to liters (1 L = 1000 mL), so the volume is 0.25 L. The given temperature is 45°C, which needs to be converted to Kelvin by adding 273, so the temperature is 45 + 273 = 318 K. The given mass is 3.4 g, and we can use the molar mass of neon (20.18 g/mol) to convert grams to moles: 3.4 g / 20.18 g/mol = 0.1682 mol.

Now we can substitute the values into the ideal gas law equation:

P(0.25 L) = (0.1682 mol)(0.0821 L·atm/mol·K)(318 K)

Solving for P gives:

P = (0.1682 mol)(0.0821 L·atm/mol·K)(318 K) / 0.25 L = 7.22 atm

Therefore, the pressure of the neon gas inside the flask is 7.22 atm.

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Answer:

Personal Referral.

Explanation:

This technique of finding employees is called Personal Referral. In personal referral the existing employee of the company uses hi/her own connections to find employees for the company. He/she may ask his/her asks current customers for names of friends, customers and other businesses that might be interested in job provided by the company.

Final answer:

Mary is employing a 'Word of Mouth' marketing strategy by asking current customers for referrals, tapping into the informal network to reach potential customers with the trust built through personal recommendations.

Explanation:

Mary, a sales representative, is utilizing a marketing strategy known as Word of Mouth. By asking current customers for referrals, she is tapping into her business's informal network to identify potential customers who might be interested in the cleaning services her company provides.

This approach takes advantage of the trust and reliability found within personal networks, as individuals are more likely to believe and try services recommended by people they know and trust. Additionally, Mary's strategy could involve engaging with information hubs or influencers within her network who are more likely to share information about the cleaning services with a broader audience.

In the context of increasing sales, connecting with customers on a more personal level and leveraging their networks can be an effective method to gain new leads. This is particularly effective as it has been shown that a vast majority of jobs, similar to customer opportunities, are found through social networks, highlighting the power of personal contacts and referrals. Mary's approach can be seen as a grassroots method to increase customer outreach and foster organic growth for the business.

Answer:

2Mg  +  O2 →  2MgO

Explanation:

In all conbustion you should know, that reactans are an specific compound and O2, so the products must be CO2 and H2O, or in this case, the corresponding oxide.

The balanced equation for the combustion of Magnesium is 2Mg + O2 -> 2MgO. It's a redox reaction where Magnesium is oxidised and Oxygen is reduced.

The combustion of Magnesium in Oxygen is a well-known reaction in Chemistry. The balanced equation for this reaction is 2Mg + O2 -> 2MgO. In this reaction, two moles of Magnesium react with one mole of Oxygen gas to produce two moles of Magnesium Oxide. This is a redox reaction where Magnesium gets oxidised and Oxygen gets reduced.

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Answer:

Molarity = 1.53 M

Explanation:

At STP,  

Pressure = 1 atm  

Temperature = 273.15 K

Given, Volume = 27.0 L

Using ideal gas equation as:

[tex]PV=nRT[/tex]

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

1 atm × 27.0 L = n × 0.0821 L.atm/K.mol × 273.15 K  

⇒n = 1.20 moles

Given that volume = 785 mL

Also,  

[tex]1\ mL=10^{-3}\ L[/tex]

So, Volume = 785 / 1000 L = 0.785 L

Considering:

[tex]Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}[/tex]

[tex]Molarity=\frac{1.20}{0.785}[/tex]

Molarity = 1.53 M

Answer:

d. n H2(g) = 0.034 mol

Explanation:

                              2 - Na - 2

                              4 - H - 4

                               2 - O - 2

∴ n Na(s) = 0.068 mol

⇒ n H2(g) = ( 0.068 mol Na(s) )( mol H2(g) / 2 mol Na(s) )

⇒ n H2(g) = 0.034 mol

Based on the stoichiometric relationship between sodium and hydrogen in the given balanced chemical equation, 0.068 mol of sodium would yield 0.034 mol of hydrogen gas.

The correct answer is (b) 0.034 mol H2. The balanced chemical equation given states that 2 moles of sodium metal (Na) react with 2 moles of water molecules (H2O) to produce 2 moles of sodium hydroxide (NaOH) and 1 mole of hydrogen gas (H2). This implies a stoichiometric ratio of 2:1 between sodium and hydrogen. Therefore, if we have 0.068 moles of sodium, we would obtain half of this number in moles of hydrogen because of this stoichiometric relationship. 0.068 mol ÷ 2 = 0.034 mol H2.

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Common cations that can form insoluble sulfate salts that can form insoluble salts with the anion include calcium, barium, strontium, and lead.

A precipitate forms only when [tex]Na_2SO_4[/tex] is added to the solution of the unknown soluble ionic compound. This indicates that the anions in [tex]Na_2SO_4 (SO_4^2-)[/tex] react with certain cations in the unknown compound to form an insoluble compound.

To form an insoluble compound with sulfate ions [tex](SO_4^2-)[/tex], the cations need to form an insoluble sulfate salt. Common cations that can form insoluble sulfate salts include [tex]Ca^{2+}, Ba^{2+}, Sr^{2+}, Pb^{2+}[/tex].

A precipitate forms when [tex]Na_2SO_4[/tex] is added to the unknown solution, it suggests that the unknown compound could contain one or more of these cations. Other cations that do not form insoluble sulfate salts would not result in a precipitate with [tex]Na_2SO_4[/tex].

For the determination of the cation present in the compound, a confirmatory test is almost necessary.

Therefore, the common cations that can form insoluble sulfate salts that can form insoluble salts with the anion include calcium, barium, strontium and lead.

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The cation that can be present in the unknown soluble ionic compound can be Ba2+ since Barium sulfate(BaSO4) is known to be an insoluble sulfate salt which forms a precipitate.

The unknown soluble ionic compound can have cations such as Ba2+ (barium). Here, the solubility is determined based on the interaction of ions in the solution. When a precipitate forms only with the addition of Na2SO4, it suggests that the sulfates form an insoluble compound with the cation present in the unknown solution. However, not with KCl or NaOH. According to solubility guidelines, sulfate salts (SO42-) are typically soluble, with exceptions for salts containing Pb2+, Sr2+, Ca2+, and Ba2+. So, one possible cation in the unknown soluble ionic compound is Ba2+.

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Answer: [tex]156.4^0C[/tex]

Explanation:

[tex]2C_6H_6(l)+15O_2(g)\rightarrow 12CO_2(g)+6H_2O(l)+6542kJ[/tex] [tex]\Delta H=-6542kJ[/tex]

To calculate the moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{7.700g}{78.11g/mol}=0.9858moles[/tex]

According to stoichiometry :

2 moles of [tex]C_6H_6[/tex] releases = 6542 kJ of heat

0.9858 moles of [tex]C_6H_6[/tex]  release =[tex]\frac{6542}{2}\times 0.9858=3224kJ[/tex] of heat

Thus heat given off by burning 7.700 g of [tex]C_6H_6[/tex]  will be absorbed by water.

[tex]Q=m\times c\times \Delta T[/tex]

Q = Heat absorbed= 3224kJ = 3224000J   (1kJ=1000J)

m= mass of water = 5691 g

c = specific heat capacity = [tex]4.184J/g^0C[/tex]

Initial temperature of the water = [tex]T_i[/tex] = 21.0°C

Final temperature of the water = [tex]T_f[/tex]  = ?

Putting in the values, we get:

[tex]3224000J =5691g\times 4.184J/g^0C\times (T_f-21)[/tex]

[tex]T_f=156.4^0C[/tex]

The final temperature of the water is [tex]156.4^0C[/tex]

Answer:

(C) substance B is not involved in the rate-determining step of the mechanism but is involved in subsequent steps.

Explanation:

A. Is incorrect because if the order of the reaction with respect B was one then the rate would increase by the same multiple that B is increased by.

B. If B is reactant then it must be involved in the mechanism of the reaction and in the formation of the product

D. If B was a catalyst then increasing it's amount would affect the rate

E. That is just factually untrue. Effect of reactants on rates can only be found experimentally, not stoichiometrically.

The most probable explanation for this observation is (C) substance B is not involved in the rate-determining step of the mechanism but is involved in subsequent steps.

Answer:

1 billion molecules O₂

Explanation:

From my research, a human red blood cell contains approximately 270 million hemoglobin molecules.    

A hemoglobin molecule contains four heme groups, each of which has an iron ion forming a coordination complex that carries every dioxygen molecule. Therefore for each hemoglobin molecule, we will have 4 dioxygen molecules. The heme groups are responsible for the transport of every dioxygen and other diatomic gases.                    

Hence, the number of O₂ molecules in a red blood cell saturated with 100% will be:                

[tex] \frac{270 \cdot10^{6} hemoglobine molecules}{1 red blood cell} \cdot \frac{4 heme group}{1 hemoglobine molecule} \cdot \frac{1 O_{2} molecules}{1 heme group} = 1 \cdot 10^{9} O_{2} \frac{molecules}{red blood cell} [/tex]

So, the correct answer is 1 billion of O₂ molecules.  

Have a nice day!

Answer: 181 kJ

Explanation:

The balanced chemical reaction is;

[tex]C_2H_5OH(l)+3O_2(g)\rightarrow 2CO_2(g)+3H_2Ol)[/tex] [tex]\Delta H=-555jJ[/tex]

To calculate the moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{15.0g}{46.0g/mol}=0.326moles[/tex]

According to stoichiometry:

1 mole of [tex]C_2H_5OH[/tex] on complete combustion give= 555 kJ

Thus 0.326 moles of [tex]C_2H_5OH[/tex] on complete combustion give=[tex]\frac{555}{1}\times 0.326=181kJ[/tex]

Thus the enthalpy change for combustion of 15.0 g of ethanol is 181 kJ

Answer:answers are in the explanation

Explanation:

(a). pH less than 7 between 1 - 3.5 are strong acid, and between 4.5-6.9 weak acid.

pH greater than 7; between 10-14 is a strong base, and between 7.1 - 9, it is weakly basic.

(b). Equation of reaction;

HBr + KOH ---------> KBr + H2O

One mole of HBr reacts with one mole of KOH to give one Mole of KBr and one mole of H2O

Calculating the mmol, we have;

mmol KOH = 28.0 ml × 0.50 M

mmol KOH= 14 mmol

mmol of HBr= 56 ml × 0.25M

mmol of HBr= 14 mmol

Both HBr and KOH are used up in the reaction, which leaves only the product,KBr and H2O.

The pH here is greater than 7

(C). [NH4^+] = 0.20 mol L^-1 × 50 ml. L^-1 ÷ 50 mL + 50mL

= 0.10 M

Ka=Kw/kb

10^-14/ 1.8× 10^-5

Ka= 5.56 ×10^-10

Therefore, ka= x^2 / 0.20

5.56e-10 = x^2/0.20

x= (0.20 × 5.56e-10)^2

x= 1.05 × 10^-5

pH = -log [H+]

pH= - log[1.05 × 10^-5]

pH = 4.98

Acidic(less than 7)

(c). 0.5 × 20/40

= 0.25 M

Ka= Kw/kb

kb= 10^-14/1.8× 10^-5

Kb = 5.56×10^-10

x= (5.56×10^-10 × 0.5)^2

x= 1.667×10^-5 M

pH will be basic

Final answer:

In titrations, the pH at the equivalence point depends on the type of titration. For part b, the pH after adding 28.0 mL of KOH can be calculated by determining the moles of HBr and KOH and using the stoichiometry of the reaction. Similarly, for part c and part d, we can calculate the pH by determining the moles of the reactants and using stoichiometry.

Explanation:

For the first part of the question, the pH at the equivalence point depends on the type of titration. In a titration between a weak acid and a strong base, the pH at the equivalence point will be greater than 7. In a titration between a strong acid and a strong base, the pH at the equivalence point will be equal to 7. In a titration between a weak base and a strong acid, the pH at the equivalence point will be less than 7.

For part b, we have a titration between a strong acid (HBr) and a strong base (KOH). The initial volume of HBr is 56.0 mL and the volume of KOH added is 28.0 mL. To calculate the pH after the addition of 28.0 mL of KOH, we need to determine the moles of HBr and KOH and use the stoichiometry of the reaction to find the concentration of the resulting solution, which will give us the pH.

For part c, we have a titration between a weak base (NH3) and a strong acid (HNO3). The initial volume of NH3 is 50.0 mL and the volume of HNO3 added is 50.0 mL. Similarly to part b, we need to determine the moles of NH3 and HNO3 and use the stoichiometry of the reaction to find the concentration of the resulting solution, which will give us the pH.

For part d, we have a titration between a weak acid (CH3COOH) and a strong base (NaOH). The initial volume of CH3COOH is 30.0 mL and the volume of NaOH added is also 30.0 mL. Again, we need to determine the moles of CH3COOH and NaOH and use the stoichiometry of the reaction to find the concentration of the resulting solution, which will give us the pH at this point.

Answer:

61.76%

Explanation:

Percent yield = Actual yield/Theoeetical yield × 100%

We need to calculate the theoretical yield for this reaction.

Firstly, we need to know the number of moles of hydrogen reacted = mass of hydrogen ÷ molar mass = 450 ÷ 2 = 225 moles

From the reaction, we can see that 3 moles of hydrogen yielded 2 moles of ammonia. Hence 225 moles of hydrogen will yield:

(225 × 2) ÷ 3 = 150 moles

The actual mass of ammonia yielded = number of moles × molar mass = 150 × 17 = 2550g

Actual yield = 1575g

Theoretical yield = 2550g

Percentage yield = 1575/2550 × 100% = 61.76%

The correct option is (c). The percent yield of this reaction is 62.1%

To calculate the percent yield of the reaction, we need to compare the actual yield to the theoretical yield. The balanced chemical equation for the production of ammonia is:

[tex]\[ N_2 + 3H_2 \rightarrow 2NH_3 \][/tex]

 From the equation, we see that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia. The molar masses of[tex]\( N_2 \), \( H_2 \), and \( NH_3 \)[/tex] are approximately 28.02 g/mol, 2.016 g/mol, and 17.031 g/mol, respectively.

 First, we calculate the number of moles of hydrogen gas that reacted:

[tex]\[ \text{moles of } H_2 = \frac{\text{mass of } H_2}{\text{molar mass of } H_2} = \frac{450 \text{ g}}{2.016 \text{ g/mol}} \approx 223.2 \text{ moles} \][/tex]

Since the stoichiometric ratio of[tex]\( H_2 \) to \( NH_3 \)[/tex] is 3:2, we can find the theoretical yield of ammonia:

[tex]\[ \text{moles of } NH_3 \text{ produced theoretically} = \frac{2}{3} \times 223.2 \text{ moles} \approx 148.8 \text{ moles} \][/tex]

 Now, we calculate the theoretical mass of ammonia that could be produced:

[tex]\[ \text{mass of } NH_3 \text{ theoretically} \approx 148.8 \text{ moles} \times 17.031 \text{ g/mol} \approx 2533.5 \text{ g} \][/tex]

The actual yield is given as 1575 g of ammonia. The percent yield is calculated by:

 [tex]\[ \text{Percent Yield} = \left( \frac{\text{actual yield}}{\text{theoretical yield}} \right) \times 100\% \][/tex]

[tex]\[ \text{Percent Yield} = \left( \frac{1575 \text{ g}}{2533.5 \text{ g}} \right) \times 100\% \approx 62.1\% \][/tex]

 Therefore, the percent yield of this reaction is 62.1%.

Answer:

Activation energy is the amount of energy required to convert the reactants into the activated complex (option B)

Explanation:

The activation energy is the minimum needed energy to make a reaction occurs. When the reaction occurs, the molecules of reactants joins together in a determined position, so when they bond all the molecules reactants, they make the activated complex. That's why we say, that the energy needed to make the molecules of reactants form the activated complex is finally the activation energy.

When the activated complex is formed, there is a few moment with all the molecules from reactants bonding together. By the end, they are separated so the products are been formed.

Activation energy is the amount of energy required to convert the reactants into the activated complex.

Activated complex is the specie which is obtain in the transition state of the chemical reaction, and in this complex partial bond of reactants as well as partial bond of products are present.

So, the minimum amount of energy required by the reactant molecules to reach the threshold point where this activated complex is formed, known as the activation energy. After that state complex will finally convert in the product.

Hence, option (B) is correct.

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Answer:

In the given chemical reaction:

Species Oxidized: I⁻

Species Reduced: Fe³⁺

Oxidizing agent: Fe³⁺

Reducing agent: I⁻

As the reaction proceeds, electrons are transferred from I⁻ to Fe³⁺

Explanation:

Redox reaction is a chemical reaction involving the simultaneous movement of electrons thereby causing oxidation of one species and reduction of the other species.

The chemical species that gets reduced by gaining electrons is called an oxidizing agent. Whereas, the chemical species that gets oxidized by losing electrons is called a reducing agent.

Given redox reaction: 2Fe³⁺ + 2I⁻ → 2Fe²⁺ + I₂

Oxidation half-reaction: 2 I⁻ +  → I₂ + 2 e⁻                 ....(1)

Reduction half-reaction: [ Fe³⁺ + 1 e⁻ → Fe²⁺ ] × 2

                                   ⇒  2 Fe³⁺ + 2 e⁻ → 2 Fe²⁺       ....(2)

In the given redox reaction, Fe³⁺ (oxidation state +3) accepts electrons and gets reduced to Fe²⁺ (oxidation state +2) and I⁻ (oxidation state -1) loses electrons and gets oxidized to I₂ (oxidation state 0).

Therefore, Fe³⁺ is the oxidizing agent and I⁻ is the reducing agent and the electrons are transferred from I⁻ to Fe³⁺.

In this electron transfer reaction, iodide ions (I-) are oxidized to iodine (I2) and act as the reducing agent, while iron(III) ions (Fe3+) are reduced to iron(II) ions (Fe2+) and act as the oxidizing agent.

In the provided electron transfer reaction, a notable chemical transformation unfolds where the iodide ion (I-) undergoes oxidation to form iodine (I2), while concurrently, the iron(III) ion (Fe3+) experiences reduction to yield iron(II) ion (Fe2+). In terms of the key participants, it is crucial to discern the roles of reducing and oxidizing agents. The reducing agent is the entity that itself undergoes oxidation, and in this specific scenario, the iodide ion (I-) fulfills this role by ceding electrons during the reaction.

Conversely, the oxidizing agent is the species that undergoes reduction in the course of the reaction, and here, it's the iron(III) ion (Fe3+). As the reaction unfolds, electrons are effectively transferred from iodide ions to iron(III) ions, signifying a fundamental aspect of electron transfer reactions. This intricate interplay between the reducing and oxidizing agents, with the exchange of electrons, characterizes the essence of redox reactions in chemistry.

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Answer:

outer electron moved to a higher energy state

Explanation:

To know this, let's write again the electron arrangements:

[A] = 1s² 2s² 2p^6 3s^1

[B] = 1s² 2s² 2p^6 5s^1

Now, let's discart the options.

First option cannot be, because if you count the inner electrons, which are the numbers uppering (besides the s and p), in both cases, you have the same number of electrons, which is 11 in both cases.

Second option cannot be either, because electron configuration, always go from lower to higher state. In the case, that one electron move to a lower state, it should move fro 3s to the 2p level. In this case, it was not, mainly because the lower level of 2, has already maxed out it's capacity to hold electrons.

Therefore, option 3 it's the more accurate option, you can see that from 2p6, it jump to the energy level 5, skipping 3 and 4th level. Therefore this is the correct option.

Answer:

The outer electron of atom B has moved to a higher energy state.

Explanation: (Graded correct)

Answer:

The halogens located in group 17

Explanation:

The change in energy of a neutral atom when an electron is added is known as electron affinity. Fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At) are known as halogens and conform the group 17 of the periodic table, the group that presents higher electron affinity. This characteristic happens because of their atomic structures, it is easier for them to gain electrons because they are closer to form octets.

Here I present you halogens' electron affinities values:

The use of negative signs is to indicate the RELEASE of energy.

I hope you find this information useful and interesting! Good luck!

Answer:

The answer to your question is letter A, Argon

Explanation:

Isotope               Atomic mass                      Percent (%)

    1                       35.9675                              0.337

    2                      37.9627                              0.063

    3                      39.9624                            99.6

Average atomic mass = (Mass isotope 1)(percent 1) + (Mass isotope 2)(percent  

                                        2) + (Mass isotope 3)(percent 3)

Average atomic mass = (35.9675)(0.00337) + (37.9627)(0.00063) +

                                       (39.9624)(0.996)

Average atomic mass = 0.1212 + 0.0239 + 39.8025

Average atomic mass = 39.9476

                   Theoretical  Atomic mass

a) Ar                         39.95

b) K                          39.10

c) Cl                         35.45

d) Ca                       40.08

Answer:

mass water = 32.4 g

Explanation:

specific heat iron = 0.450 J/g°C

specific heat water = 4.18 J/g°C

32.8 x 0.450 ( 59.1 - 22.4) + mass water x 4.18 ( 59.1- 63.1)=0

541.7 - mass water x 16.7 = 0

mass water = 32.4 g

Answer:C

Explanation:

A process is called spontaneous if the process takes place on its own without the intervention of external factors.

The spontaneous processes are generally quick with observable rates of reaction.But processes can be spontaneous even with negligible rates of reaction.

Spontaneity of reactions depend on temperature.

This is because spontaneity is measured by gibbs energy or enthalpy.

Both of these measures are dependent on temperature.

So,temperature affects spontaneity.

Answer: a. Synthesis

Explanation:

a. Synthesis reaction is a chemical reaction in which two reactants are combining to form one product.

Example: [tex]Mg+O_2\rightarrow 2MgO[/tex]  

Thus magnesium in its elemental form is combining with oxygen to form magnesium oxide.

b. Double displacement reaction is one in which exchange of ions take place.  

Example: [tex]2NaOH(aq)+(NH_4)_2SO_4(aq)\rightarrow 2NH_4OH(aq)+Na_2SO_4(aq)[/tex]

c. Decomposition is a type of chemical reaction in which one reactant gives two or more than two products.

Example: [tex]Li_2CO_3\rightarrow Li_2O+CO_2[/tex]

Answer:

Final temperature is 71·31 °C

Explanation:

where

m is the mass of the substance

s is the heat capacity of the substance

ΔT is the temperature difference

where

m is the mass of the substance

L is the latent heat of the substance

Let the final temperature be T

As the density of the water is 1 g/ml

∴ The mass of 90ml water will be 90 g

Heat gained by the ice when it is attained at 0°C and converted to water is

(10×2·08×11) +  10×6 = 288·8

But the heat loss by the water when water attains 0°C will be 90×4·18×80 = 30,096

As the heat loss is more therefore there will be further rise in temperature

Now the heat gain = 288·88 + 10×4·18×T

heat loss = 90×4·18×(80-T)  

Here in the case of heat loss as we are already mentioning that the heat is lost so we are taking the magnitude of the heat change otherwise it would be 90×4·18×(T-80)

288·88 + 41·8×T = 9×41·8×(80-T)

41·8×9×80 - 288·8 = 10×41·8×T

∴T=71·31 °C

Final answer:

Nonmetals generally gain electrons to form anions in reactions with metals, creating ionic compounds, or they share electrons in reactions with each other to form molecular compounds.

Explanation:

When nonmetals react with other elements, they typically undergo a process where they gain electrons to form anions, or negative ions, as they combine with metals to produce ionic compounds. In reactions with each other, nonmetals often form molecular compounds with covalent bonding, where electrons are shared rather than transferred. The most reactive nonmetals, like fluorine, have a particularly high electron affinity and can take part in vigorous redox reactions, changing their oxidation states. Considering the diverse group of nonmetals, these elements can form a variety of different compounds, both ionic and covalent, depending on the elements they react with and the environmental conditions.

Answer:

Metalloids have properties of metals and non-metals.

Explanation:

A metalloid is a type of chemical element which has properties in between, or that are a mixture of, those of metals and nonmetals.

The six commonly recognized metalloids are boron, silicon, germanium, arsenic, antimony, and tellurium.

Metalloids have a metallic appearance, but they are brittle (nonmetal property) and only fair conductors of electricity. Chemically, they behave mostly as nonmetals. They can form alloys with metal.

Most of their other physical properties and chemical properties are intermediate in nature.

That means Metalloids  have properties of both metal and nonmetal.

Answer:

The answer is NO₂-NO₂, N₂O₄

Explanation:

If 23.0 g of this gas were found to occupy 5.6 L at STP we can apply the Ideal gas Law to determinate the quantity of mols of the oxide.

As I have the mass, I can find out the molar weight.

STP are 1 atm and 273, 1 K so:

P . V = n . R . T

1 atm .  5.6L = n . 0.082 L.atm/mol.K . 273.1K

(1 atm .  5.6L)/ 0.082 mol.K/L.atm . 273.1K = n

0.250 mol = n

Molar weight = mass/mols

23 g /0.250 mol = 92 g/m

The percentages are:  30.4% N and 69.6%O

100% ____ 92 g

30.4% _____ (30.4 .92)/100 = 28 g → 2 mols of N

100% _____ 92 g

69.6% ____ (69.6 . 92)/ 100 = 64 g → 4 mols of O

Molecular formula N₂O₄

Empirical formula: NO₂-NO₂

Answer:

-2312 kJ

Explanation:

By the Hess Law, when a reaction is formed by several steps, the enthalpy change (ΔH) of the global reaction can be calculated by the sum of the enthalpy changes of the steps reactions.

Besides that, when a reaction is multiplied by a constant, ΔH must be multiplied by the same constant, and when the reaction is inverted, the signal of ΔH must be inverted.

B₂O₃(s) + 3H₂O(g) → 3O₂(g) + B₂H₆(g) ΔH = +2035 kJ (multiply by 2 and inverted)

2B(s) + 3H₂(g) → B₂H₆(g) ΔH = +36 kJ (multiply by 2)

H₂(g) + 1/2O₂(g) → H₂O(l) ΔH = -285 kJ (multiply by 6 and inverted)

H₂O(l) → H₂O(g) ΔH = +4 kJ (multiply by 6 and inverted)

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6O₂(g) + 2B₂H₆(g) → 2B₂O₃(s) + 6H₂O(g) ΔH = -4070 kJ

4B(s) + 6H₂(g) → 2B₂H₆(g) ΔH = +72 kJ

6H₂O(l) → 6H₂(g) + 3O₂(g) ΔH = +1710 kJ

6H₂O(g) → 6H₂O(l) ΔH = -24 kJ

Summing the equation, simplifying the equal terms in both sides:

4B(s) + 3O₂(g) → 2B₂O₃(s)

ΔH = -4070 + 72 + 1710 - 24

ΔH = -2312 kJ

Answer:

B) A series of chemical reactions where enzymes work one at a time to convert a reactant into intermediates and the intermediates into a final product.

Explanation:

In our cells there are multiple chemical reactions happening all the time to convert the  elements we ingest (food, water, air) into the products the organism needs.

This processes can be very complex and offen involves various reactions (steps). Also, many of this reactions need to by catalized by enzymes in order to happen.

Answer: B

Explanation:

A metabolic pathway is series of chemical reactions that are well organized, well co-ordinated, and purposeful manner; all these reactions are collectively called as metabolism.

Metabolic Pathways this is a series of biochemical reaction where enzymes work one at a time to convert a reactant into intermediates and the intermediates into a final product. The product of reactions serve as an a reactants for the next enzymatic reaction.

The reactants, intermediates, products of an enzymatic reaction are known as metabolites.

Types of Metabolic pathway

1. Catabolic

2. Anabolic

3. Amphibolic

Answer:

Atomic radius of sodium = 227 pm

Atomic radius of potassium = 280 pm

Explanation:

Atomic radii trend along group:

As we move down the group atomic radii increased with increase of atomic number. The addition of electron in next level cause the atomic radii to increased. The hold of nucleus on valance shell become weaker because of shielding of electrons thus size of atom increased.

Consider the example of sodium and potassium.

Sodium is present above the potassium with in same group i.e, group one.

The atomic number of sodium is 11 and potassium 19.

So potassium will have larger atomic radius as compared to sodium.

Atomic radius of sodium = 227 pm

Atomic radius of potassium = 280 pm

Answer:

Anthracite

Explanation:

Anthracite variety of coal is the coal with the highest energy available per unit burned. Anthracite is hard, brittle, lustrous coal . They also often referred as hard coal. Anthracite has a high percentage of carbon and low percentage of volatile matter. Other varieties of coal  are peat, lignite and bituminous.  

Answer:

The correct answer is: Oxidation number

Explanation:

According to the IUPAC nomenclature for the inorganic compounds, roman numerals are used to denote the oxidation number of a positively charged ion, called cation.

This rule is only applicable to elements that can form more than one cation with different oxidation state or charge.

The oxidation state or charge of each cation of such an element is denoted or represented by a Roman numeral in the parentheses followed by the name of the element.

Therefore, the oxidation number of a cation is denoted by a roman numeral which is written after the name of the element.