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Title: When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical ... Post by: wheels123 on Jun 23, 2021 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) ΔrH° = ? ▸ -1420 kJ mol-1 ▸ -708 kJ mol-1 ▸ +708 kJ mol-1 ▸ +1420 kJ mol-1 Title: When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical ... Post by: oscar520000 on Jun 23, 2021 Content hidden
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