When 150 Mol of CH₄(g) Reacts with Excess Cl₂(g) at Constant

question 40

Multiple Choice

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.
2CH₄(g) + 3Cl₂(g) → 2CHCl₃(l) + 3H₂(g) H° = ?

• A) -1420 kJ
• B) -708 kJ
• C) +708 kJ
• D) +1420 kJ

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A principle in corporate finance that asserts the market value of a firm is unaffected by the capital structure, assuming no taxes and perfect markets.

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