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) -1420 kJ B) -708 kJ C) +708 kJ D) +1420 kJ E) -710 kJ

Question

Quizplus · Accepted Answer

The given reaction releases 354 kJ of heat for 0.500 mol of CH4, which corresponds to 1/2 of the stoichiometric coefficient in the balanced equation. Therefore, for the full reaction (2 moles of CH4), it would release 2 * 354 kJ = 708 kJ. Since ΔH is expressed per mole of reaction as written, and the reaction as written involves 2 moles of CH4, the total heat released for the reaction as written is 708 kJ * 2 = 1420 kJ. The negative sign indicates that heat is released, making ΔH = -1420 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