For the reaction H2(g) + I2(g) leftharpoons 2HI(g) Kc = 66.9 at 350°C and Kc = 50.0 at 448°C. The reaction has

Question

For the reaction H2(g) + I2(g) leftharpoons 2HI(g) Kc = 66.9 at 350°C and Kc = 50.0 at 448°C. The reaction has (A) Δ H = + ve (B) Δ H =-v e (C) Δ H = zero (D) Δ H = Not found the signs

Tardigrade Admin · Accepted Answer

K decreases as increase in temp. Hence exothermic Δ H < 0

Q. For the reaction $H_{2} (g) + I_{2} (g) ⇌ 2 H I (g) Kc = 66.9$ at $350° C$ and $K_{c} = 50.0$ at $448° C$ . The reaction has

$Δ H = +$ ve

$Δ H =$ -v e

$Δ H =$ zero

$Δ H =$ Not found the signs

$K$ decreases as increase in temp. Hence exothermic $Δ H < 0$

Q. For the reaction H2​(g)+I2​(g)⇌2HI(g)Kc=66.9 at 350°C and Kc​=50.0 at 448°C. The reaction has

ΔH=+ ve

ΔH=-v e

ΔH= zero

ΔH= Not found the signs