Chemistry

Chemistry

Problem

At 500 K, the equilibrium constant for the reaction H2(g)+I2(g)⇌2 HI(g)\mathrm{H_2(g) + I_2(g) \rightleftharpoons 2\,HI(g)} is Kc=49K_c = 49. A mixture at this temperature initially contains [H2]=0.50 M,  [I2]=0.50 M,  [HI]=3.50 M[\mathrm{H_2}] = 0.50\,\text{M},\; [\mathrm{I_2}] = 0.50\,\text{M},\; [\mathrm{HI}] = 3.50\,\text{M} and is at equilibrium. If exactly 0.25 M0.25\,\text{M} of HI\mathrm{HI} is suddenly removed while temperature and volume remain constant, what is the value of the reaction quotient QcQ_c immediately after the removal, and what will be the direction of the net reaction as the system re-establishes equilibrium? a) Qc=49;  the reaction will remain at equilibrium (no net shift)Q_c = 49;\;\text{the reaction will remain at equilibrium (no net shift)} b) Qc=13;  the reaction will shift right to form more HIQ_c = 13;\;\text{the reaction will shift right to form more }\mathrm{HI} c) Qc=42;  the reaction will shift right to form more HIQ_c = 42;\;\text{the reaction will shift right to form more }\mathrm{HI} d) Qc=42;  the reaction will shift left to form more H2Q_c = 42;\;\text{the reaction will shift left to form more }\mathrm{H_2} and I2\mathrm{I_2}

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