Question

Given the reaction,

\[\ce{CH2O_{(g)} + O2_{(g)} -> CO2_{(g)} + H2O_{(g)}}\] ΔH = −527 kJ

How much heat will be evolved in the formation of 60 g of CO₂?

पर्याय

• 358.44 kJ

• 1433.44 kJ

• 716.72 kJ

• 400 kJ

Answer 1

716.72 kJ

Explanation:

According to the reaction, 527 kJ of heat is evolved per mole of CO₂ formed.

Number of moles of CO₂ = `("mass of CO"_2)/("molar mass of CO"_2)`

= `(60 "(g)")/(44 ("g"//"mol"))`

= 1.36 mol

Hence, the heat evolved in the formation of 1.36 mol of CO₂ = +527 kJ mol⁻¹ × 1.36 mol

= +716.72 kJ