Heat of formation of KOHs using the following equations - Ks- H2Ol-aq - KOHaq-1-2H2g- - H- -48-0 kcal H2 g - 1-2O2g - H2Ol- - H- -68-4 kcal KOHs- aq - KOHaq- - H- -14-0 kcal

The correct option is A 102.4 kcal Given that, K(s)+ H_2O(l)+ (Aq.) ⟶ KOH(aq) + 1/2H_2(g); Δ H= 48.0 kcal ...( i) H_2( g ) + 1/2O_2(g) ⟶ H_2O ...

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Heat of Formation

Heat of forma...

Question

Heat of formation of KOH(s) using the following equations :

$K (s) + H_{2} O (l) + (a q) ⟶ K O H (a q) + \frac{1}{2} H_{2} (g); Δ H = - 48.0 k c a l$

$H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); Δ H = - 68.4 k c a l$

$K O H (s) + (a q) ⟶ K O H (a q); Δ H = - 14.0 k c a l$

- 102.4 k c a l

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- 152.5 k c a l

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- 112.6 k c a l

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None of these

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K O H

K_{(s)} + H_{2} O + a q \to {K O H}_{(a q)} + \frac{1}{2} H_{2}; Δ H = - 48.4 K . C a l

H_{2 (g)} + \frac{1}{2} O_{2 (g)} \to H_{2} O_{(l)}; Δ H = - 68.44 K . C a l

{K O H}_{(s)} + a q \to {K O H}_{(a q)}; Δ H = - 14.0 K . C a l

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 68.09 k c a l

K + H_{2} O + w a t e r \to K O H (a q .) + \frac{1}{2} H_{2}; Δ H = - 48.0 k c a l

K O H + w a t e r \to K O H (a q); Δ H = - 14.0 k c a l

K O H

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 68.39 K c a l

K + H_{2} O + w a t e r \to K O H (a q) + \frac{1}{2} H_{2}

Δ H = - 48.0 K c a l

K O H + w a t e r \to K O H (a q) Δ H = - 14.0 K c a l

K O H

H_{2} + 1 / 2 O_{2} ⟶ H_{2} O; Δ H^{⊖} = - 68 K c a l

K + H_{2} O + a q ⟶ K O H (a q) + 1 / 2 H_{2}; Δ H^{⊖} = - 48 K c a l

K O H + a q ⟶ K O H (a q); Δ H^{⊖} = - 14 K c a l

K O H i n K c a l

H^{+} (a q) + O H^{-} (a q) = H_{2} O (l); Δ H = - X_{1} k J . m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) = H_{2} O (l); Δ H = - X_{2} k J . m o l^{- 1}

C O_{2} (g) + H_{2} (g) = C O (g) + H_{2} O (l); Δ H = + X_{3} k J . m o l^{- 1}

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) = 2 C O (g) + H_{2} O (l); Δ H = + X_{4} k J . m o l^{- 1}

H_{2} O (l)

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