When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy...

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When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy...

When excess Cl₂ at constant pressure reacts with 0.300 mol of CH₄(g) 295 kJ of energy evolves. Calculate the value of ΔH for this reaction, as written.

CH₄(g) + Cl₂(g) → CHCl₃(l) + H₂(g) ΔH = ?

a) -1970 kJ

b) -1770 kJ

c) +1970 kJ

d) -983 kJ

e) +1770 kJ

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When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy...

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When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy...

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