2CH3OH(g) yields 2CH4(g) + 02(g) deltaH = +252.8kJ A) Calculate the amount of he

Question

2CH3OH(g) yields 2CH4(g) + 02(g) deltaH = +252.8kJ A) Calculate the amount of heat transferred when 27.0g of CH3OH(g) is decomposed by this reaction at constant pressure. B) For a given sample of CH3OH, the enthalpy change during the reaction is 82.2kJ . How many grams of methane gas are produced? C)How many kilojoules of heat are released when 38.2g of CH4 (g) reacts completely with O2}(g) to form CH3OH (g) at constant pressure?

Explanation / Answer

part B) Change the g of CH3OH to moles. -> 21.0g(mol/32g) = 0.65625 mol CH3OH Then divide the enthalpy (252.8 kJ) by 2 because that is the coefficient of CH3OH in the equation. -> 252.8/2=126.4 Then multiply the number of mols (0.65625) by 126.4 kJ c. 82.1kJ(2 mol CH3OH/252.8 kJ)(2 mol CH4/2 mol CH3OH)(16.042 g CH4/1 mol CH4)=10.4 g CH4 (g) i dont know to solve part A

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