Question

For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant.

C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)

Part B:
4.3 molC3H8
Express your answer using two significant figures.
V=. molH20

Part C:
4.3 molO2
Express your answer using three significant figures.
V=. molH20

Part D:
0.0528 molO2
Express your answer using two significant figures.
V=. molH20

Answer 1

For 4.3 mol of C3H8, 17.2 moles of H2O are formed. We cannot accurately determine the H2O formed from 4.3 mol of O2 without knowing the amount of C3H8. For 0.0528 mol of O2, 0.0422 moles of H2O are formed.

Step-by-step explanation:

To calculate the moles of product formed from a given amount of reactants, we'll use the balanced chemical equation C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g). The stoichiometric ratios tell us that for every mole of C3H8, we produce 4 moles of H2O.

Part B: Given 4.3 mol C3H8, the moles of H2O produced would be:

Moles of H2O = 4.3 mol C3H8 × (4 moles H2O / 1 mole C3H8) = 17.2 moles H2O

Part C: We can't directly give an answer for 4.3 mol O2 because we do not have the C3H8 to O2 ratio for this specific instance, but if we assume that C3H8 is in excess, the same calculation method would apply, and we would need 5 moles of O2 to react with 1 mole of C3H8. We cannot determine the exact moles of H2O without the corresponding amount of C3H8

Part D: For 0.0528 mol O2, the reaction is limited by O2 since it is not in excess, therefore, we calculate moles of H2O based on O2 available:

Moles of H2O = 0.0528 mol O2 × (4 moles H2O / 5 moles O2) = 0.0422 moles H2O