Tim is grilling burgers for dinner. He uses 15.0g of propane. Given that the combustion of propane releases 2,220 kJ/mol and that the molecular weight of propane is 44.097 g/mol, calculate the enthalpy of the propane used for dinner.

A) 755 kJ

B) 1,390 kJ

C) 2,130 kJ

D) 6,530 kJ

Question

Chemistry

Franco

8 April, 20:22

Tim is grilling burgers for dinner. He uses 15.0g of propane. Given that the combustion of propane releases 2,220 kJ/mol and that the molecular weight of propane is 44.097 g/mol, calculate the enthalpy of the propane used for dinner.

A) 755 kJ

B) 1,390 kJ

C) 2,130 kJ

D) 6,530 kJ

+3

Answers (2)

Know the Answer?

Derek · Answer 1

A.

Hopefully it works

Paul Leonard · Answer 2

Heat Enthalpy used = 755 Kilojoules

Explanation:

15 grams propane = (15g/44.097g·mol⁻¹) = 0.3402mol propane

Heat Enthalpy used = 0.3402mol X 2,220Kj/mol = 755 Kilojoules

Tim is grilling burgers for dinner. He uses 15.0g of propane. Given that the combustion of propane releases 2,220 kJ/mol and that the molecular weight of propane is 44.097 g/mol, calculate the enthalpy of the propane used for dinner.A) 755 kJB) 1,390 kJC) 2,130 kJD) 6,530 kJ

Tim is grilling burgers for dinner. He uses 15.0g of propane. Given that the combustion of propane releases 2,220 kJ/mol and that the molecular weight of propane is 44.097 g/mol, calculate the enthalpy of the propane used for dinner.

A) 755 kJ

B) 1,390 kJ

C) 2,130 kJ

D) 6,530 kJ