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Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.64 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.64 L flask at a certain temperature initially contains 0.765 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.3 g HI. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. please round to two digits

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Expert Solution

Important points to remember:

1. Concentration = moles/total volume

2. Law of mole balance (not mass balance, be careful) applies according to the stoichiometry of the reaction.

3. Kc is defined for the concentration of the reactants and products in equilibrium. Only subsitute the equilibrium values of concentration.

4. MW of H2 = 2 g; MW of I2 = 253.8 g; MW of HI = 127.9

5. Amount of HI produced =1/2 x Amount of H2 or I2 consumed: You can see from the stoichiometry of the reaction.

milcah answered 2 years ago
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