Question

Propane gas, C3H8, reacts with oxygen to produce water and carbon dioxide.
C3H8(g)+5O2(g)→3CO2(g)+4H2O(l)

Part A

How many moles of CO2 form when 3.70 mol of C3H8 completely reacts?

Part B

How many grams of CO2 are produced from 17.4 g of propane gas?

Part C

How many grams of CO2 can be produced when 43.4 g of C3H8 reacts?

Answer 1

a) According to the stoichiometry 1 mole of propane gives 3 mol of CO₂
   so 3.70 mol of propane will give = 3*3.70 mol = 11.1 mol of CO₂

b) mol of propane gas = 17.4 gm / 44.1 gm/mol = 0.3945 mol
0.3945 mol of propane will give = 3*0.3945 = 1.1836 mol of CO₂
   grams of CO₂ produced are = 1.1836 mol * 44.01 g/mol = 52.0934 gms
[ CO₂ molar mass is 44.01 gm/mol ; propane molar mass = 44.1 gm/mol]

c) mol of propane = 43.4 gm / 44.1 gm/mol = 0.9841 mol
0.9841 mol of propane will give = 0.9841*3 = 2.9525 mol of CO₂
   grams of CO₂ produced = 2.9525 mol * 44.01 gm/mol = 129.9342 gms