4) Use Hess's law to calculate AG°rxn using the following information. 2 NO(g) + O(g) → NO2(g) AG°rxn=? %3D reverse -489.6KJ 8 2 O3(g) → 3 02(g) 02(g) → 2 0(g) NO(g) + O3(g)→ NO2(g) + O2(g) AG°rxn = +489.6 kJ AG°rxn = +463.4 kJ -463,4 KJ +어9.5K3 AG°rxn = - 199.5 kJ -> A) +753.5 kJ B) +277.0 kJ C-676.0 kJ D) -1152.5 kJ E) -225.7 kJ

4) Use Hess's law to calculate AG°rxn using the following information. 2 NO(g) + O(g) → NO2(g) AG°rxn=? %3D reverse -489.6KJ 8 2 O3(g) → 3 02(g) 02(g) → 2 0(g) NO(g) + O3(g)→ NO2(g) + O2(g) AG°rxn = +489.6 kJ AG°rxn = +463.4 kJ -463,4 KJ +어9.5K3 AG°rxn = - 199.5 kJ -> A) +753.5 kJ B) +277.0 kJ C-676.0 kJ D) -1152.5 kJ E) -225.7 kJ

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...

See similar textbooks

Similar questions

Please help very urgent
9.) Use Hess's law to calculate AG°rxn using the following information. NO(g) + 0(g) 2 03(g) → 3 02(g) → 2 0(g) NO2(g) AG°rxn=? AG°rxn=+489.6 kJ AG°rxn=+463.4 kJ 02(g) NO(g) + 03(g) → NO2(g)+ 02(g) AG°rxn=- 199.5 kJ
Determine the standard enthalpy of formation (in kJ/mol) of calcium carbonate (AH°) from the thermochemical equations given below. Ca(OH)2(s) → CaO(s) + H20(1) AH° = 65.2 kJ/mol-rxn Ca(OH)2(s) + CO2(g) → CaCO3(s) + H2O(1) AH° = -113.8 kJ/mol-rxn C(s) + O2(g) –CO2(g) AH° = -393.5 kJ/mol-rxn 2 Ca(s) + O2(g) → 2 CaO(s) AH° = -1270.2 kJ/mol-rxn
gopal
Determine the amount of heat (in kJ) associated with the production of 3.26 ×104 g of ammonia according to the following equation.N2(g) + 3H2(g) 2NH3 ΔH°rxn = −92.6 kJ Assume that the reaction takes place under standard-state conditions at 25 °C. Enter your answer in scientific notation. × 10 kJ
Determine the standard enthalpy of formation of Fe2O3(s) given the thermochemical equations below. Fe(s) + 3 H2O(l) → Fe(OH)3(s) + 3/2 H2(g) ΔrH° = +160.9 kJ H2(g) + 1/2 O2(g) → H2O(l) ΔrH° = –285.8 kJ Fe2O3(s) + 3 H2O(l) → 2 Fe(OH)3(s) ΔrH° = +288.6 kJ
Calcium carbide, CaC2, is manufactured by reducing lime with carbon at high temperature. (The carbide is used in turn to make acetylene, an industrially important organic chemical.) CaO(s)+3C(s)→CaC2(s)+CO(g) ΔH=464.8kJ Calculate the quantity of energy, in MJ, transferred when 34.8 mol CO(g) is formed by this reaction.
A hot lump of 47.547.5 g of iron at an initial temperature of 51.5 °C51.5 °C is placed in 50.0 mL H2OH2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g·°C)?0.449 J/(g·°C)? Assume no heat is lost to surroundings.
Give the ΔHΔH value for the formation of binary compounds as shown in the reaction H2(s)+Br2(g)→2HBr(s)+36.3kJH2(s)+Br2(g)→2HBr(s)+36.3kJ. Express your answer using three significant figures. If the value is positive, do not include the + sign in your answer.
The following reaction enthalpies can be measured: C2H4(g)+3O2(g)→2CO2(g)+2H2O(l) ΔH∘=−1411.83 kJ C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l) ΔH∘=−1367.68 kJ Find the enthalpy change when 9.55 kg of ethylene, C2H4(g), react with an excess of H2O(l)H2O(l) to produce ethanol, C2H5OH(l).
Define specific heat capacity. the quantity of heat required to raise the temperature of 1 mole of a substance by 1°C the quantity of heat required to change a system's temperature by 1°C the quantity of heat required to raise the temperature of 1 gram of a substance by 1°C the quantity of heat required to raise the temperature of 1 gram of a substance by 1°F the quantity of heat required to raise the temperature of 1 liter of a substance by 1°C
1. What is the standard enthalpy of formation (AH°) of HI given the following chemical equation? X 2HI(g) → H₂(g) + 1₂(s) AH°rxn=-53.0 kJ +53.0 kJ/mol b. -53.0 kJ/mol C. d. c + 26.5 kJ/mol - 26.5 kJ/mol