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Sodium bicarbonate decomposes at high temperatures according to the following equation: $2 N a H C O_{3} (s) ⇌ N a_{2} C O_{3} (s) + H_{2} O (g) + C O_{2} (g)$ . At a certain temperature, 50.0 g of $N a H C O_{3}$ is allowed to react in a 6.0 L evacuated vessel. At equilibrium, the total pressure is 4 atm, with some of both solids still present. If 50.0 g of $N a H C O_{3}$ is allowed to react in a 3.0 L evacuated vessel at the same temperature, what will the pressure (in mmHg) of $C O_{2} (g)$ be at equilibrium?

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answer is 1520.

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Detailed Solution

$2 N a H C O_{3} (s) ⇌ N a_{2} C O_{3} (s) + H_{2} O (g) + C O_{2} (g)$
$K_{p} = p_{H_{2} O} \times p_{C O_{2} = 2 \times 2 = 4}$
$K_{p}$ is constant at constant $T \Rightarrow p_{H_{2} O} = p_{C O_{2}} = 2 a t m$

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