THERMODYNAMICS Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) 402 (g) + 3J2X () AH = -1,034 kJ 4QJ3 (g) + 3X2 (g) 202 (g) + 6J2X () AH = -1.577.7 kJ Calculate the value of AH (in kJ) for the reaction: 02 (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) 402 (g) + 3J2X () AH = -1,034 kJ 4QJ3 (g) + 3X2 (g) 202 (g) + 6J2X () AH = -1.577.7 kJ Calculate the value of AH (in kJ) for the reaction: 02 (g) % X2 (g) – Q2X (g) (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...

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The oxidation of glucose, C6H12O6(s), is described by the following thermochemical equation:C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -2772 kJHow much heat, in kilojoules, can be produced by the oxidation of 3.56 g of fuel C6H12O6?Molar mass of C6H12O6 = 180.156 g/mol
What is the change in enthalpy for the reaction: 2B (s) + 3H2(g) → B2H6 (g) given these thermochemical equations? B2H6 (g) + 302 (g) →B2O3 (s) + 3 H₂O (g) AH = -2032 kJ 2B (s) + 3/2 O2 (g) → B2O3 (s) AH = -1272 kJ H2(g) + 1/2 O2 (g) → H2O (g) AH -241.8 kJ -4029 kJ +518.2 kJ +34.6 kJ -3546 kJ
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (g) + 3J2X (1) AH = -1,070 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X (1) AH = -1,580.2 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 (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)
Find the ΔH of the following reaction:
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.)
Given the following thermochemical equations: C2H29) + 5 02(9) 2C02(g) + H201) AH° = -1229.5 kJ AH° = -393.5 kJ C(6) + 02(g) → C02(g) 1 H2(9) +5 02(9) → H20) AH° = -285.5 kJ 2 Calculate the enthalpy (in kJ) for this reaction: 206) + H2(g) → C,H2(9)
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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.)
Consider the reaction of ammonia gas with O2(g) according to the thermochemical equation given below: 4NH3(g) + 7O2(g) 4NO2(g) + 6H2O(1) AH° = -1132 kJ/mole (c) Write the thermochemical equation representing the combustion of 1 mole of ammonia. (d) Write the thermochemical equation representing the reaction of 1 mole NO2(g) with Hz0