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The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of...

The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of methane is burned, 890.4 kj are give off to the surroundings. This means that the products have less energy stored in the bonds than the reactants. Thus, for the reaction: CH4(G) + 2 O (g) -> CO2 (g) + 2 H2O (I) deltaH= -890.4kj/mol. A) what is the enthalpy change when 2.00 mol of CH4 are burned? B)what is the enthalpy change when 22.4g of CH4 are burned C) if you were to attempt to make 45.0g of methane form CO2 and H20 (with O2 also being produced), What is the enthalpy change for the reaction?

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Answer #1

CH4(G) + 2 O (g) -> CO2 (g) + 2 H2O (I) deltaH= -890.4kj/mol.

A) what is the enthalpy change when 2.00 mol of CH4 are burned?

dH = Hrxn*n = -890.4*2 = -1780.8 kJ

B)what is the enthalpy change when 22.4g of CH4 are burned

mol = mass/MW = 22.4/16 = 1.4 mol

dH = Hrxn*n = -890.4*1.4 = -1246.56kJ

C) if you were to attempt to make 45.0g of methane form CO2 and H20 (with O2 also being produced), What is the enthalpy change for the reaction?

mol = mass/MW = 45/16 = 2.81

dH = Hrxn*n = -890.4*2.81 = -2502.024 kJ

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