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Class 11 Chemistry Practice Test: Equilibrium - Law of Chemical Equilibrium and Equilibrium Constant
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According to the "Law of Chemical Equilibrium," the equilibrium constant is the ratio of the product of the concentration of the products to the product of the concentration of the reactants. Each concentration term raises the stoichiometric coefficient in the balanced chemical equation.

Class 11 Chemistry Practice Test: Equilibrium - Law of Chemical Equilibrium and Equilibrium Constant
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10 Questions

1. for the reaction H2(g) + Br2(g) ↔ 2HBr(g) the equilibrium constant is given as 0.04 then what is the equilibrium constant for the reaction 2HBr(g) ↔ H2(g) + Br2(g)?
2. A reaction is given by aA + bB → cC + dD. How do you represent an equilibrium constant?
3. Given that at 800k the concentrations are as follows: N2=3.0 × 10–3M, O2 = 4.2 × 10–3M and NO = 2.8 × 10–3M, what is the equilibrium constant for the reaction N2(g) + O2(g) \(\rightleftharpoons \) 2NO(g)?
4. The value of equilibrium constant for different chemical reactions at a particular temperature is ____________
5. If we use activities in place of molar concentration in an equilibrium constant expression then what is the dimension of k?
6. If the chemical reaction is: aA + bB → cC + dD and K is the equilibrium constant. Then what is the equilibrium constant of the reaction naA + nbB → ncC + ndD?
7. What does it indicate having a higher equilibrium constant?
8. What is the equilibrium constant of the following reaction: 4NH3 + 5O2 → 4NO + 6H2O?
9. If the initial concentrations of reactants in a reaction increase then the equilibrium constant ____________
10. The equilibrium constant of a reaction is 20 units and the equilibrium constant of other reaction is 30 units when both the reactions are added up together then the equilibrium constant of the resultant reaction is given by _____________

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