THERMODYNAMICS: Given the following hypothetical thermochemical equations: 20J3 (9) + 302X (g) – 4Q2 (9) + 3J2X (1) AH = -1,032 kJ 4QJ3 (g) + 3X2 (g) – 202 (g) + 6J2X (1) AH = -1,595.6 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (9) + % X2 (g) – Q2X (9) (Round off the final answer to ONE decimal place. Do not include unit.)

THERMODYNAMICS: Given the following hypothetical thermochemical equations: 20J3 (9) + 302X (g) – 4Q2 (9) + 3J2X (1) AH = -1,032 kJ 4QJ3 (g) + 3X2 (g) – 202 (g) + 6J2X (1) AH = -1,595.6 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (9) + % X2 (g) – Q2X (9) (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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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)
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)
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: Given the following hypothetical thermochemical equations: 20J3 (g) + 302x (g) – 402 (g) + 3J2X () AH = -1,017.3 kJ 4QJ3 (e) + 3X2 (@) – 202 (g) + 6J2X (1) AH = -1,548.8 kJ Calculate 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.)
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.)
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?
Calculate the internal energy change (ΔE) for a system undergoing an exothermic process in which 24.9 kJ of heat flows out of the system and where 13.6 kJ of work is done on the system. Show all work and units in your answer, Ex: (-12.4) + (-3.0) = -15.4 kJ.
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 = -89.3 kJ AX (g) + ½R2 (g) → XAR (g) AH = -152.2 kJ Q (s) + R2 (g) –→ QR2 (s) AH = -533.9 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)