A. You get 2219 kJ for a mol (44 g) propane; therefore,
2219 x (10/44) = ? kJ.
B. You get 2219 kJ for 4 mol H2O (4*18 = 72g). Therefore,
2219 kJ x (10/72) = ? kJ.
Given the following equation,
C3H8 (g) + 5O2 (g) -> 3CO2 (g) + 4H2O (g); H comb = -2219 kJ/mole
A) how much heat will be released when 10 g of propane is burned?
B) how much heat will be released when 10 g of water (H2O) is formed?
Please show all work.
2 answers
volume of oxygen in liters at .91 ml of oxygen
3 answers