When 2.500 mol of CH₄(g)reacts with excess Cl₂(g)at constant pressure according to the chemical equation shown below,1770.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 = ? A)-1416 kJ B)-708.0 kJ C)+708.0 kJ D)+1416 kJ

Question

Quizplus · Accepted Answer

The given reaction releases 1770 kJ of heat for 2.500 mol of CH4, so the ΔH for the reaction as written (which involves 2 moles of CH4) is calculated by (1770 kJ / 2.500 mol) * 2 = 1416 kJ. Since heat is released, ΔH is negative, making it -1416 kJ.

When 2500 Mol of CH4(g)reacts with Excess Cl2(g)at Constant Pressure According

When 2500 Mol of CH₄(g)reacts with Excess Cl₂(g)at Constant Pressure According