When 1.50 mol of CH4(g) reacts with excess Çl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of AH for this reaction, as written. 2 CH4(g) + 3 Cl2(g) → 2 CHC13(1) + 3 H2(g) ΔΗ- A) -1420 kJ B) -708 kJ C) +708 kJ D) +1420 kJ Answer: A 1.50mal CHy 10GR KJ,|| 3mol Clz 15mol CHy -796.5KJ Rmol CHy

When 1.50 mol of CH4(g) reacts with excess Çl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of AH for this reaction, as written. 2 CH4(g) + 3 Cl2(g) → 2 CHC13(1) + 3 H2(g) ΔΗ- A) -1420 kJ B) -708 kJ C) +708 kJ D) +1420 kJ Answer: A 1.50mal CHy 10GR KJ,|| 3mol Clz 15mol CHy -796.5KJ Rmol CHy

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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