Below is a thermochemical equation for the combustion of propane (C3H8). Use thi

ID: 905010 • Letter: B

Question

Below is a thermochemical equation for the combustion of propane (C3H8). Use this equation to answer the following questions.

C3H8(g) + 5O2(g) ------> 3CO2(g) + 4H2O delta rH = -2220 kJ/mol*rxn

a.) how much heat energy (delta H) will be produced from the combustion of 3 moles of propane with excess O2?

b.) How much heat energy will be produced from the combustion of 100.0 g propane and excess O2?

c.) how much heat energy will be needed to synthesize propane from 500 g CO2 and excess H2O?

Given

Given reaction

C3H8(g) + 5O2(g) ------> 3CO2(g) + 4H2O delta rH = -2220 kJ/mol

a).

Heat produced from 3 mol.

In equation we know heat produced from 1 mol propane = 2220 kJ

We calculate heat produced from 3 mol

= 3 mol propane x -2220 kJ/mol

= -6660 kJ

Heat produced from 3 mol propane = - 6660 kJ

b).

Given mass of propane = 100.0 g

Moles of propane = 100.0 g / molar mass of propane

= 100.0 g /44.1 g per mol

= 2.27 mol propane

Heta produced = 2.27 mol propane x – 2220 kJ/mol

=-5034.0 kJ

c).

Mass of CO2 = 500 g

Calculation of moles of CO2 = 500 g / molar mass of CO2

= 500 g / 44.01g per mol = 11.34 mol

Equivalent heat for 3 mol CO2 is -2220 kJ

Heat produced when 11.34 CO2 are formed

= 11.34 mol CO2 x -2220 kJ/ 3 mol CO2

= -84089.19 kJ

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