4. For the reaction 2A(g) + B(g) → 4C + 3D, AG is 456.2 kJ/mol at 25.0°C. a. Write the Q expression for this reaction. b. Calculate the Q when the concentration of [A] = 0.432 M, (B] = 1.234 M, [C] = 0.3367 M and [D] = 0.250 M. c. Calculate the nonstandard Free Gibbs Value in kl/mol at 25.0°C d. What should be done to the concentrations of C and D to make the reaction go from being nonspontaneous to spontaneous? (Increase or decrease) Explain your answer. (Assume the concentration of A and B remain at 0.432 M and 1.234 M)

4. For the reaction 2A(g) + B(g) → 4C + 3D, AG is 456.2 kJ/mol at 25.0°C. a. Write the Q expression for this reaction. b. Calculate the Q when the concentration of [A] = 0.432 M, (B] = 1.234 M, [C] = 0.3367 M and [D] = 0.250 M. c. Calculate the nonstandard Free Gibbs Value in kl/mol at 25.0°C d. What should be done to the concentrations of C and D to make the reaction go from being nonspontaneous to spontaneous? (Increase or decrease) Explain your answer. (Assume the concentration of A and B remain at 0.432 M and 1.234 M)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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#8 Round each of your answers to the nearest kJ - as it states in the directions.
Calcium carbonate decomposes according to the following reaction. ????3(?)⟺???(?)+??2(?)CaCO3(s)⟺Cao(s)+CO2(g) The tabulated data below was determined at 25 °C. CaCO3(s) CaO(s) CO2(g) Δ?∘?ΔHf∘ Δ?∘?ΔHf∘, kJ/mol -1206.9 -635.1 -393.5 ?∘S∘ ?∘S∘, kJ/(mol K) 0.0929 0.0382 0.2137 Δ?∘?ΔGf∘ Δ?∘?ΔGf∘, kJ/mol -1128.8 -603.5 -394.4 What is ΔG° at 25 °C for this reaction? Is the reaction spontaneous at 25 °C? What is ΔG° at 1000 °C for this reaction? Is the reaction spontaneous at 1000 °C? Calculate KP for this reaction at 25 °C and 1000 °C.
Nitrogen tetroxide breaks down according to the equation: N204 (g) +2NO2 (g) AH = 54KJ / mol %3D Pure N204 (g) was added to a 3.00 L container at 127 ° C under a pressure of 5.00 kPa. After the system reached its equilibrium state, the total pressure in the container was found to have risen to 8.43 kPa. Question 1: Calculate the value of KP at 127 oC for this reaction Question 2: The volume of the container is suddenly compressed to 1.00 L at 127 ° OC, tripling the pressure of all components in the container from equilibrium in (a). In what direction would the equilibrium of the reaction shift? Calculate the new partial pressures of N204 and NO2, as well as the total pressure in the container, once equilibrium is re- established
The standard reaction free energy AGO = –194. kJ for this reaction: SnO₂(s) + 2 CO(g) → Sn(s) + 2 CO₂(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction 2 Sn (s) + 4CO₂ (g) 2SnO, (s) + 4CO(g) 3SnO₂(s) + 6CO(g) - 3Sn(s) + 6CO₂ (g) 2 Sn (s) + 2CO₂(g) → SnO₂ (s) + 2CO(g) 2 AG KJ KJ ☐ kJ x10 X S
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5. Consider the combustion reaction of octane (C8H18, mol. wt. = 114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. 2 C8H18 + 25 O2 ---> 16 CO2 + 18 H2O b. Calculate the standard free energy (in kJ/mol) released in this reaction. ∆Hfo (kJ/mol) Sfo (J/K mol) Octane(l) ─208.4 463.7 H2O(g) ─242 189 02 0 205 CO2(g) ─393.5 214 c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts)
Chp 19 #28 & # 30
Determine the temperature of a reaction if K = 1.20 x 106 when AG° = +22.70 kJ/mol.
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