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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: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 72QAP: On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm...
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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) AH = ? A) -1420 kJ B) -708 kJ C) +708 kJ D) +1420 kJ Answer: A 1.50 mal CHy MOGR KJT4 2mol CHy 15mol CHy 3mol Clz -796.51J
Transcribed Image Text: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) AH = ? A) -1420 kJ B) -708 kJ C) +708 kJ D) +1420 kJ Answer: A 1.50 mal CHy MOGR KJT4 2mol CHy 15mol CHy 3mol Clz -796.51J
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