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

`\boxed{\text{46.07 g}}`

Step-by-step explanation:

M_r: 46.07

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

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