Question

Use the following information to find ΔH°f of gaseous HCl: N2(g) + 3H2(g) → 2NH3(g)                     ΔH°rxn...

Use the following information to find ΔH°f of gaseous HCl:

N2(g) + 3H2(g) → 2NH3(g)                     ΔH°rxn = - 91.8 kJ

N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(s)   ΔH°rxn = - 628.8 kJ

NH3(g) + HCl(g) → NH4Cl(s)               ΔH°rxn = - 176.2 kJ

Homework Answers

Answer #1

N2(g) + 3H2(g) → 2NH3(g) ΔH°rxn = - 91.8 kJ 1equation

N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(s) ΔH°rxn = - 628.8 kJ 2 equation

NH3(g) + HCl(g) → NH4Cl(s) ΔH°rxn = - 176.2 kJ 3 equation

Multiply the third equation by -2. The (-) will reverse the direction of the reaction.
Multiply the first reaction by -1.
Sum the modified first and third and add the second. You will be left with
H2(g) + Cl2(g) ---> 2HCl(g).

Now perform the same operations on the ΔH. e.g., third value times -2, first value times -1. Add them now and add the second value. That's it.

(-2)*(-176.2) + (-1)*(-91.8) + 1*(-628.8) = -184.6/2 =so, ∆HRx = −92.3 kJ mol−1 of HCl

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
N2 (g) + 3H2 (g) → 2NH3(g) ΔH = -92.2 kJ What mass of ammonia is...
N2 (g) + 3H2 (g) → 2NH3(g) ΔH = -92.2 kJ What mass of ammonia is theoretically produced if the above reaction released 183 kJ of heat? Please show work
Applying Hess’s Law, from the enthalpies of reactions, N2(g) + 3H2(g) → 2 NH3(g) ΔH =...
Applying Hess’s Law, from the enthalpies of reactions, N2(g) + 3H2(g) → 2 NH3(g) ΔH = − 91.8 kJ O2(g) + 2H2(g) → 2H2O (g) ΔH = − 483.7 kJ N2(g) + O2(g) → 2NO(g) ΔH = 180.6 kJ Calculate the enthalpy change (ΔHrxn) for the reaction: 4NH3(g) + 5O2(g) → 4 NO (g) + 6H2O(g)
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF: ΔH°f (kJ/mol) IF7(g) +...
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF: ΔH°f (kJ/mol) IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ IF7(g) -941 IF5(g) -840
Determine the equilibrium constant Kp at 25°C for the reaction: N2(g) + 3H2(g) ⇆ 2NH3(g) (G°f...
Determine the equilibrium constant Kp at 25°C for the reaction: N2(g) + 3H2(g) ⇆ 2NH3(g) (G°f (NH3(g)) = -16.6 kJ/mol)
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF: ΔH°f (kJ/mol) IF7(g) +...
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF: ΔH°f (kJ/mol) IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ IF7(g) -941 IF5(g) -840 Answers: (a) -190 KJ/mol (b) 101 KJ/mol (c) 24 KJ/mol (d) -95 KJ/mol (e) -146 KJ/mol
NO2(g) + 7⁄2H2(g) ---> 2H2O(ℓ) + NH3(g) ΔH° = ??? kJ Using the following two equations:...
NO2(g) + 7⁄2H2(g) ---> 2H2O(ℓ) + NH3(g) ΔH° = ??? kJ Using the following two equations: 2NH3(g) ---> N2(g) + 3H2(g) ΔH° = +92 kJ 1⁄2N2(g) + 2H2O(ℓ) ---> NO2(g) + 2H2(g) ΔH° = +170 kJ
Please solve step by step for Part D Consider the Haber synthesis of gaseous NH3 (ΔH∘f=−46.1kJ/mol...
Please solve step by step for Part D Consider the Haber synthesis of gaseous NH3 (ΔH∘f=−46.1kJ/mol ;ΔG∘f=−16.5kJ/mol) : N2(g)+3H2(g)→2NH3(g) Part A Use only these data to calculate ΔH∘ and ΔS∘ for the reaction at 25 ∘C. Express your answers using three significant figures separated by a comma. ΔH∘, ΔS∘ = -92.2,-199   kJ, J/K   Part D. What are the equilibrium constants Kp and Kc for the reaction at 370 K ? Assume that ΔH∘ and ΔS∘ are independent of temperature.​ Express...
calculate the standard free energy change delta G for reaction N2 (g) +3H2(g)—>2NH3 N2 delta H=0.00kj...
calculate the standard free energy change delta G for reaction N2 (g) +3H2(g)—>2NH3 N2 delta H=0.00kj mol^-1s=+191.5J mol^-1K^-1 H2 delta H=0.00kj mol^-1,s = +130.6j mol^-1 k-1 NH3 delta H=-46.0kj mol^-1,s =192.5 J mol^-1 k-1 A. +112.3 kJ B.-87.6kJ C.-7.4kJ D.-32.9 kJ E.-151.1kJ
Ammonia is formed by the Haber process according to the following reaction: N2(g) + 3H2(g) ⇌...
Ammonia is formed by the Haber process according to the following reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) Use the following data table to answer the questions below: Substance: ΔHf (kJ/mol) So (J/(mol*K) N2(g) 0    187.4 H2(g) 0 127.1 NH3(g) -47.3 197.6 Part 1: Using the table in the introduction, calculate the value of ΔH in units of kJ/mol. After, calculate the value of ΔS in units of J/(mol*K). Finally, cCalculate the value of ΔG in units of kJ/mol for...
consider the following reaction: 2NH3 (g) <=> N2 (g) + 3H2 (g) if 7.92 x 10-4...
consider the following reaction: 2NH3 (g) <=> N2 (g) + 3H2 (g) if 7.92 x 10-4 moles of NH3, 0.336 moles of N2 and 0.287 moles of H2 are at equilibrium in a 10.2 L container at 884 K, the value of the equilibrium, Kp, is _