Question

Consider the following reaction where K. = 154 at 298 K. 2NO(g) + Br2(g) 2 2NOBr(g) A reaction mixture was found to contain 5.19x10-2 moles of NO(g), 3.85x10 - moles of Br (9) and 9.56x102 moles of NOBr(g). in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Answer 1

To determine if the reaction is at equilibrium, compare the reaction quotient, Qc, with the equilibrium constant, K. If Qc = K, the reaction is at equilibrium. If Qc < K, the reaction must run in the forward direction. If Qc > K, the reaction must run in the reverse direction.

Step-by-step explanation:

To determine if the reaction is at equilibrium, we can compare the reaction quotient, Qc, with the equilibrium constant, K. Qc is calculated using the concentrations of the reactants and products at a particular point in time, while K represents the equilibrium concentrations. If Qc is equal to K, the reaction is at equilibrium. If Qc is less than K, the reaction must run in the forward direction to reach equilibrium. If Qc is greater than K, the reaction must run in the reverse direction to reach equilibrium.

In this case, the reaction quotient can be calculated using the given concentrations: [NO] = 5.19x10^(-2) M, [Br2] = 3.85x10^(-9) M, [NOBr] = 9.56x10^(-2) M. Compare the calculated Qc with K to determine the direction the reaction must run.

Answer 2

The correct option is A.

Step-by-step explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
`K_(eq)`

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

`2NO(g) + Br_2(g)\rightleftharpoons 2NOBr(g)`

The equilibrium constant of the reaction =
`K_c=154`

Concentration of NO gas =
`[NO]=(5.19* 10^(-2) mol)/(1L)=5.19* 10^(-2) M`

Concentration of bromine gas =
`[Br_2]=(3.85* 10^(-2) mol)/(1L)=3.85* 10^(-2) M`

Concentration of NOBr gas =
`[NOBr]=(9.56* 10^(-2) mol)/(1L)=9.56* 10^(-2) M`

`Q_c=([NOBr]^2)/([NO]^2[Br])`

`Q_c=((9.56* 10^(-2) M)^2)/((5.19* 10^(-2))^2* 3.85* 10^(-2) M)=88.13`

`K_c>Q_c`

No , the reaction is not at equilibrium. the reaction will move in forward direction to attain an equilibrium.