Answer :
Final answer:
2154.97 kilojoules of heat are released when 38.8 g of CH4(g) reacts completely with O2(g) at constant pressure, based on the combustion of 1 mol of CH4 releasing 890.4 kJ.
Explanation:
The question asks how many kilojoules of heat are released when 38.8 g of CH4(g) reacts completely with O2(g) to form CH3OH(g) at constant pressure. From the provided data, we know that the combustion of 1 mol of CH4 releases 890.4 kJ of heat energy. To find the heat released by 38.8 g of CH4, we first need to convert grams to moles, using the molar mass of CH4 (16.04 g/mol). After the conversion, we can use the proportionality of the enthalpy change to determine the heat released.
Calculating the moles of CH4:
38.8 g CH4 imes (1 mol CH4 / 16.04 g CH4) = 2.42 moles of CH4
Calculating the heat released:
2.42 moles CH4 imes (890.4 kJ / 1 mol CH4) = 2154.97 kJ
Therefore, 2154.97 kilojoules of heat are released when 38.8 g of CH4 is combusted.
