URGENT!
You just worked a volume-volume stoichiometry problem to find that 90 L of carbon dioxide gas (CO2) are produced when 30 litres of propane gas (C3H8) react with excess oxygen at STP according to the following chemical equation:
C3H8 (g) + 502(g) —> 4H2O(g) + 3CO2(g)
Does this final answer seem correct? Does it “make sense”?
The final answer does not seem correct. According to the balanced chemical equation, 1 mole of propane (C3H8) reacts with 5 moles of oxygen (O2) to produce 3 moles of carbon dioxide (CO2). Therefore, the stoichiometry calculation should yield a smaller volume of carbon dioxide gas than the initial volume of propane gas. It's important to double-check the stoichiometry calculation and ensure that the units are consistent throughout the calculation.
