When 1 g of anhydrous oxalic acid is burnt at 25° C, the amount of heat liberated is 2.835 kJ . Δ H combustion is (oxalic acid: .C 2 H 2 O 4)

Question

When 1 g of anhydrous oxalic acid is burnt at 25° C, the amount of heat liberated is 2.835 kJ . Δ H combustion is (oxalic acid: .C 2 H 2 O 4) (A) -255.15 kJ (B) -445.65 kJ (C) -295.24 kJ (D) -155.16 kJ

Tardigrade Admin · Accepted Answer

underset text(oxalic acid)H2C2O4(s) + (1/2) O2(g) → 2CO2 (g) + H2O(l) We know, Δ H text combusion = Amount of heat liberated when 1 mole of substance reacts with oxygen. Mol. wt. of oxalic acid =90 g mol -1 1 g oxalic acid liberates 2.835 kJ ∴ 90 g (1 mole) oxalic acid liberates 2.835 × 90 kJ mol -1=255.15 kJ ∴ Heat involved =-255.15 kJ

Q. When 1g of anhydrous oxalic acid is burnt at 25∘C, the amount of heat liberated is 2.835kJ.ΔH combustion is (oxalic acid : C2​H2​O4​)

-255.15 kJ

-445.65 kJ

-295.24 kJ

-155.16 kJ

Q. When $1 g$ of anhydrous oxalic acid is burnt at $2 5^{\circ} C$ , the amount of heat liberated is $2.835 k J .Δ H$ combustion is (oxalic acid : $C_{2} H_{2} O_{4})$