On complete combustion 44 gram of a sample of a compound gives 88 gram CO2 and 36 gram of H2O the molecular formula of the compound may be
Correct answer: C. C2H4
- A. C4H6
- B. C6H6O
- C. C2H4
- D. C3H6O
Explanation
X + O2 --> CO2 + H2OMoles of Co2= 88/44= 2Moles of H2O= 36/18= 2So the compound X has 2 moles of C and 4 moles of H(its H2 in H2O, so 2x2=4)Answer is C2H4
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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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