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) H° = ? A)-1420 kJ mol^-1 B)-708 kJ mol^-1 C)+708 kJ mol^-1 D)+1420 kJ mol^-1

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The Answer of 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) H° = ? A)-1420 kJ mol^-1 B)-708 kJ mol^-1 C)+708 kJ mol^-1 D)+1420 kJ mol^-1

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