Question

The equation shows one mole of ethanol fuel being burned in oxygen. Convert the energy released into its equivalent mass. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O (l) ΔH = -1418 kJ/mol

Answer 1

Answer:

$\boxed{\text{46.07 g}}$

Explanation:

M_r:      46.07

         C₂H₅OH(ℓ) + 3O₂(g) ⟶ 2CO₂(g) + 3H₂O(ℓ); ΔH = -1418 kJ·mol⁻¹

$\text{Mass} = \text{1418 kJ} \times \dfrac{\text{1 mol}}{\text{1418 kJ}} \times \dfrac{\text{46.07 g}}{\text{1mol}}= \textbf{46.07 g}\\\\\text{1418 kJ are equivalent to \boxed{\textbf{46.07 g}} of ethanol}$