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)ΔH = ?

Question

Quizplus · Accepted Answer

The reaction releases 1062 kJ for 1.50 mol of CH₄. The balanced equation involves 2 mol of CH₄, so the heat released 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