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Consider the reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.19-L flask at 500 K contains 9.02...

Consider the reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.19-L flask at 500 K contains 9.02 g of CO and 0.57 g of H2. At equilibrium, the flask contains 2.35 g of CH3OH. Calculate the equilibrium constant at this temperature.

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Answer #1

The molar masses of CO, H2 and methanol are 28 g/mol, 2 g/mol and 32 g/mol respectively.

Initially 9.02 g of CO and 0.57 g of H2 are present in 5.19 L flask. The mass is divided with molar mass to get the number of moles. The number of moles are divided with volume in L to get molar concentration.

Hence, the initial concentrations are

The equilibrium concentration is

0.01415 M methanol is obtained from 0.01415 M CO and Hydrogen

Hence, the equilibrium concentrations are

The equilibrium constant is


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