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For this question, the HI and I2 are not really left over but have equilibrium concentrations that you need to solve for in order to get K. To get their equilibrium concentrations, you set up an ICE table. The 60% of H2 used up refers to the change in H2, "x", which you can get by multiplying 0.6 to the initial molarity of H2. Knowing what "x" is and subtracting/adding "x" from the initial concentrations will allow you to complete the ICE table and find the final concentrations of HI and I2.
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