At constant pressure, the combustion of 5.00 g of c2h6 (g) releases 259 kj of heat. what is δh for the reaction given below? 2 c2h6 (g) + 7 o2 (g) → 4 co2 (g) + 6 h2o (l).

Question

Adelyn

Chemistry

18 September, 01:06

At constant pressure, the combustion of 5.00 g of c2h6 (g) releases 259 kj of heat. what is δh for the reaction given below? 2 c2h6 (g) + 7 o2 (g) → 4 co2 (g) + 6 h2o (l).

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Lainey Ochoa · Answer 1

First let us calculate the number of moles of 5 grams of a sample given molar mass of 30.07 g/mol

moles = 5 g / (30.07 g/mol)

moles = 0.166 mol

From the equation, there are 2 moles for the reaction therefore the heat of reaction is:

δhrxn = (259 kJ / 0.166 mol) * (2 / 2)

δhrxn = 3,120.48 kJ / 2 mol