THERMODYNAMICS: Given the following hypothetical thermochemical equations:20J3 (g) + 302x (g) – 402 (g) + 3J2X ()AH = -1,017.3 kJ4QJ3 (e) + 3X2 (@) – 202 (g) + 6J2X (1)AH = -1,548.8 kJCalculate the value of AH (in kJ) for the reaction: a2 (g) + % X2 (a) - Q2X (g)(Round off the final answer to ONE decimal place. Do not include unit.)

2QJ3 (g) + 3Q2X (g) --> 4Q2 (g) + 3J2X (l) ∆H = - 1017.3 kJ 4QJ3 (g) + 3X2 (g) --> 2Q2…

THERMODYNAMICS: Given the following hypothetical thermochemical equations: 20J3 (0) + 302X (e) - 402 (9) + 3J2X (1) AH = -1.017.3 kJ 40J3 (e) + 3X2 (0) – 202 (a) + OJ2X () AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (0) + % X2 (a) – Q2X (@) (Round off the final answer to ONE decimal place. Do not include unit.)

THERMODYNAMICS: Given the following hypothetical thermochemical equations: 20J3 (0) + 302X (e) - 402 (9) + 3J2X (1) AH = -1.017.3 kJ 40J3 (e) + 3X2 (0) – 202 (a) + OJ2X () AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (0) + % X2 (a) – Q2X (@) (Round off the final answer to ONE decimal place. Do not include 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

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.)
A chemist measures the enthalpy change AH during the following reaction: C,H,0,(s)-3 CH,(o) + 3CO,(g) AH=-132. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH 9CH, (0) + 9Co, (a) - 30H,0,0) 3CH, (6) + 300, (a) - C,H,0,0) GH,0,) - CH, 6) + co,()
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)
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.)
4) Consider the thermochemical equation below. What mass of HgO must decompose to consume 400.0 kJ of heat? 2 HgO (s) → 2 Hg (1)+ O2(g) AH°rxn =+ 181.4 kJ (1) 5) Write the standard formation reaction for KAI(SO4)2(s). (1) 3 CO2 (g). (1) -393.5 kJ/mol 2 Cr (s) + 3 CO (ag) -110.5 kJ/mol Cr2O3 (s) 6) Consider the reaction 0.0 kJ/mol AH°f = -1139.7 kJ/mol Calculate AH°rxn.
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.
21. The enthalpy changes of these reactions can be measured: AH° = -1411.1 kJ C,H,(g) +30,(g) C,H,OH(C) + 3 0,(g) 2 CO,(g) +2 H,O(€) 2 CO,(g) + 3 H,0(e) 1) AH° =-1367.5 kJ - Use these values and Hess's law to determine the enthalpy change for the reaction CH,(g) + H,0(() CH,OH(€)
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.)
Substance SiO,(s) SICLO H,O) HCIE) AH°, (kJ/mol) -910.7 -687.0 -285.83 -92.307 Calculate the standard enthalpy change for the following reaction: SICI4(1) + 2H20(1) → SIO2 (s) + 4HCI (g)
17. Given the following set of reaction data, AH = -285.83 kJ mol- H2 (g)+}02(8) 2B(s) +3H, (8) 2B(s) +O2(8) –→ B,O3(s) → H2O(1) → B,H, (8) AH = 36.4 kJ mol- AH = –1273.5 kJ mol determine the heat of reaction (in kJ mol') for the following reaction. – B2O3 (s) +3H,0(1) w bns maldorg B,H, (8) + 30, (g) - AH = ? kJ mol-1 lo teari done roi noltaupa 189T) of 9je s beau mo A: –2167