Question

calculate the amount of heat absorbed when 0.540 moles of chlorine are used in the reaction. be sure your answer has the correct number of significant figures.\
\
\boxed{\space} kj

Explanation:

Step1: Identify Reaction Heat

Assume the reaction involving chlorine has a known molar enthalpy change (ΔH) per mole of Cl₂. For example, if a reaction like \( \text{Cl}_2(g)
ightarrow 2\text{Cl}(g) \) has \( \Delta H = +242\ \text{kJ/mol} \) (standard bond dissociation energy for Cl - Cl), we use this.

Step2: Calculate Heat Absorbed

Use the formula \( q = n \times \Delta H \), where \( n = 0.540\ \text{mol} \) and \( \Delta H = 242\ \text{kJ/mol} \).
\( q = 0.540\ \text{mol} \times 242\ \text{kJ/mol} = 130.68\ \text{kJ} \).
Round to 3 significant figures: \( 131\ \text{kJ} \) (or adjust based on actual ΔH value).

Answer:

\( 131 \) (or value based on specific reaction's ΔH, e.g., if ΔH = 242 kJ/mol, the answer is \( 131\ \text{kJ} \))