When 0.500 mol of CH₄(g)reacts with excess Cl₂(g)at constant pressure according to the chemical equation shown below,354 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 354 kJ of heat when 0.500 mol of CH4 reacts. Since the equation shows 2 moles of CH4 reacting, we need to double the heat released for 1 mole to find the ΔH for the reaction as written. Therefore, 354 kJ * 2 = 708 kJ released for 2 moles of CH4. Since heat is released, ΔH is negative, making it -708 kJ for 0.500 mol. For the entire reaction (which involves 2 moles of CH4), we double this amount to get -1416 kJ.

When 0500 Mol of CH4(g)reacts with Excess Cl2(g)at Constant Pressure According

When 0500 Mol of CH₄(g)reacts with Excess Cl₂(g)at Constant Pressure According