Given the reaction: C3H6 + 5O2 → 3CO2 + 4H2O At STP , how many litres of O2 are needed to completely burn 5.0 litres of C3H6?
Correct answer: E. 25
- A. 5
- B. 10
- C. 10.5
- D. 15
- E. 25
Explanation
Consider that no. of moles of reactants = volume of the reactants. As the molar ratio between C3H6 and O2 is 1:5, the volume ratio is also the same. For 1L of C3H6 we need 5L of O2. Since the volume of C3H6 is 5L now, to burn this, we require 25L of O2. All other options are incorrect because they do not follow the exact mole-volume relationship required in this case.
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Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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