THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) – A2R4 (g) + 2XAR (g) AH = -80.6 kJ AX (g) + ¼R2 (g) – XAR (9) AH = -153.4 kJ Q (s) + R2 (9) → QR2 (s) AH = -501.1 kJ (Round off the final answer to ONE decimal place. Do not include the unit)

THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) – A2R4 (g) + 2XAR (g) AH = -80.6 kJ AX (g) + ¼R2 (g) – XAR (9) AH = -153.4 kJ Q (s) + R2 (9) → QR2 (s) AH = -501.1 kJ (Round off the final answer to ONE decimal place. Do not include the unit)

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

4. Hess's Law Calculate AH for the reaction: 2 C(s) + H2(g) → C:H2(g), given the following chemical equations and their respective enthalpy changes: C2H2(g)+02(g)→2CO2(g)+H20(1) AH, = -1299.6 kJ (1) %3D C(s)+02(g)→CO2(g) AH, = -393.5 kJ (2) H2(g)+502(g)→H20(1) AH3 = -285.8 kJ (3)
Determine the enthalpy of the reaction: 3Fe,O; (s) + CO (g) → CO, (g) + 2Fe;O4 (s), given the following reactions. 38. Fe,O3 (s) + 3CO (g) → 2Fe (s) + 3CO, (g) AH= -28.0 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe;O4 (s) AH =+12.5 kJ A) 40.5 +109 -59.0 -109
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (9) + 3J2X (1) AH = -1,017.3 kJ 4QJ3 (g) + 3X2 (g) → 202 (9) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (l) ΔH = -1,004 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (l) ΔH = -1,520.1 kJ Calculate the value of ΔH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g)
4) Given the data N2(8) + O2(8) 2 NO(8) AH = +180.7 kJ 2 NO(8) + O2(8) · 2 NO,(8) 2 N,0(8) – 2 N2(8) + O2(8) AH = -163.2 kJ AH = -113.1 kJ | use Hess's law to calculate AH for the reaction N20(8) + NO2(8) –→ 3 NO(8)
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (g) + 3J2X (1) AH = -1,096.4 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit,.)
THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (9) + Q (s) → A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (9) + 2XAR (g) ΔΗ = -88.4 kJ AX (g) + ½R2 (g) → XAR (g) AH = -164.8 kJ Q (s) + R2 (g) –→ QR2 (s) AH = -520.4 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)
Study the following thermochemical data very carefully: Clelg) lag) ICI(g) Ia(s) 2C(g) 21(g) I(g) + CI(g) la(g) AH = 242.3 kJ AH = 151.0 kJ AH = 211.3 kJ AH = 62.8 kJ I2(s) reacts with Clag) to produce ICI(g). Write the chemical equation to produce ONLY one mole of ICI(g)
2. Calculating enthalpy: AH = -206 kJ mol¹¹, 3 Fe(s) + 2 O₂(g) → Fe3O4 (S) AH = -136 kJ mol-¹, a) Given 2Fe(s) + 1.5 O₂(g) → Fe₂O3 (S) determine AH, for the following reaction: 4Fe₂O3(s) + Fe(s) → 3Fe3O4 (s) Is this reaction exothermic or endothermic? Is this enough information to inform whether this reaction occurs or not? O b) Given AH vap of water at 373 K = 40.7 kJ mol¹¹, C₂(l)=75.2 J mol¹¹K²¹ and ₂(g)=33.6 J mol¹¹K²¹, calculate AHvap of water at 298 K.
Rearrange the thermochemical equations given to determine the AH value for the equation of interest. Determine: 2 Fe203(s) + 3 C(s) → 3 CO2(g) + 4 Fe(s) Given Enthalpy (K/mol) 3 -833.8 O2(g) Fe203(s) 2 1. 2 Fe(s) + ch 2. C(s) + - O2(8) → CO(g) -110.4 1 O2(g) → CO2(g) -264.8 3. CO(g) + K/mol
THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s)→ A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AH = -87.2 kJ AX (g) + ½R2 (g) → XAR (g) AH = -157.3 kJ Q (s) + R2 (g) – QR2 (s) AH = -510.2 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)
to calculate the true enthalpies of these reactions by the Hess’ law, as: ΔH°(rxn) = Σ[ν × ΔHf°(product)] – Σ[ν × ΔHf°(reactant)] for: Mg(s) + ½O2(g) → MgO(s)