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. 2CH₄(g)+ 3Cl₂(g)→ 2CHCl₃(l)+ 3H₂(g)Δ_rH° = ?

Question

Quizplus · Accepted Answer

The reaction releases 1062 kJ for 1.50 mol of CH4. Since the balanced equation involves 2 mol of CH4, the ΔH for the reaction as written is (1062 kJ / 1.50 mol) * 2 mol = -1420 kJ.

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

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