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The value of K(c) for the reaction: H(2)...

The value of `K_(c)` for the reaction: `H_(2)(g)+I_(2)(g) hArr 2HI (g)` is 48 at 773 K. If one mole of `H_(2)`, one mole of `I_(2)` and three moles of HI are taken in a 1L falsk, find the concentrations of `I_(2)` and HI at equilibrium at 773 K.

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To solve the problem, we need to find the concentrations of \( I_2 \) and \( HI \) at equilibrium for the reaction: \[ H_2(g) + I_2(g) \rightleftharpoons 2HI(g) \] Given: - \( K_c = 48 \) at \( 773 \, K \) - Initial moles: \( H_2 = 1 \, \text{mol}, I_2 = 1 \, \text{mol}, HI = 3 \, \text{mol} \) - Volume of the flask = 1 L ...
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