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 ?H for this reaction,as written. 2CH₄(g)+ 3Cl₂(g)? 2CHCl₃(l)+ 3H₂(g) $\Delta _ { \mathrm { r } }$ H° = ?

Question

Quizplus · Accepted Answer

The reaction releases 1062 kJ of heat for 1.50 mol of CH4. Since the balanced equation involves 2 mol of CH4, the enthalpy change for the reaction as written is (1062 kJ / 1.50 mol) * 2 mol = -1416 kJ, which is closest to -1420 kJ/mol.

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