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When 150 Mol of CH4(g)reacts with Excess Cl2(g)at Constant Pressure According

Question 29

Multiple Choice

When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below,1062 kJ of heat are released.Calculate the value of ΔH for this reaction,as written.
2 CH4(g) + 3 Cl2(g) → 2 CHCl3(l) + 3 H2(g)

When 1.50 mol of CH<sub>4</sub>(g) reacts with excess Cl<sub>2</sub>(g) at constant pressure according to the chemical equation shown below,1062 kJ of heat are released.Calculate the value of ΔH for this reaction,as written. 2 CH<sub>4</sub>(g) + 3 Cl<sub>2</sub>(g) → 2 CHCl<sub>3</sub>(l) + 3 H<sub>2</sub>(g) H° = ? A) -1420 kJ mol<sup>-1</sup> B) -708 kJ mol<sup>-1</sup> C) +708 kJ mol<sup>-1</sup> D) +1420 kJ mol<sup>-1</sup> H° = ?


A) -1420 kJ mol-1
B) -708 kJ mol-1
C) +708 kJ mol-1
D) +1420 kJ mol-1

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