OnlineCBT
Chemistry · THERMODYNAMICS
हिन्दीDuring the complete combustion of butane, \( \text{C}_4\text{H}_{10}(g) + \frac{13}{2}\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 5\text{H}_2\text{O}(l) \), \( 2658.0\text{ kJ} \) of heat is released per mole. How much heat is released when \( 14.5\text{ g} \) of butane gas (molar mass = \( 58\text{ g mol}^{-1} \)) is burned completely at standard conditions?
Correct answer · Option 1
\( 664.5\text{ kJ} \)
Explanation
Number of moles of butane = \( \frac{14.5}{58} = 0.25\text{ mol} \). Heat released = \( 0.25 \times 2658.0\text{ kJ} = 664.5\text{ kJ} \).
