Answer:
1. Here molar mass of C3H8 = 44.1 g/mol
Moles of C3H8 = 1000/44.1 = 22.67 moles
So, one mole of C3H8 will produce three moles of CO2.
Hence, the number of moles of CO2 forms = 68.02 moles
Now the molar mass of CO2 = 44.01 g/mol
Amount of CO2 formed = 2.994 Kg
2. As there are only two reactants available in this combustion process. The limiting reactant is C3H8.
3. The % yield of CO2 formed = (Actual/Theoretical) x 100 = (2.45/2.994) x 100 = 81.83 %
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4. Bob was cooking and used up 1.00 kg of CH. during the process. How many klog were produced? Show your work, roun...
Bob was cooking and used up 1.00 kg of C3Hs during the process. How many kilograms of CO were produced? Show your work, round your answer to three significant figures, and include 4 units (10 points)? CaHs+ 5023CO2+4H20 If Bob was doing the cooking outside where there was plenty of 02 gas available, what was the limiting reactant? If during this cooking, he produced 2.45 kg of CO2, what was his percent yield?