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timama [110]
3 years ago
10

N which direction will the net reaction proceed.

Chemistry
1 answer:
finlep [7]3 years ago
6 0

Answer:

1) The correct answer is option b.

2) The correct answer is option a.

Explanation:

1)

X+Y\rightleftharpoons Z

At 300 K, the value of the K_p=1.00

The K_c and K_p is related by :

K_p=K_c\times (RT)^{\Delta n}

where,

K_p = equilibrium constant at constant pressure

K_c = equilibrium concentration constant

R = gas constant = 0.0821 L⋅atm/(K⋅mol)

T = temperature = 300 K

\Delta n = change in the number of moles of gas = 1 - 2 = -1

Now put all the given values in the above relation, we get:

1.00=K_c\times (0.0821 L atm/(K mol)\times 300)^{-1}

K_c=24.63

The K_c of the reaction = 24.63

Given = [X] = [Y] = [Z] = 1.0 M

Value of reaction quotient = Q

Q=\frac{[Z]}{[X][Y]}=\frac{1.0 M}{1.0M\times 1.0 M}=1

Q, the equilibrium will move in forward direction that is in the right direction.

2)

X+Y\rightleftharpoons Z

At 300 K, the value of the K_p=1.00

Given = P_x = P_z = 1.0 atm, P_y = 0.50 atm

Value of reaction quotient in terms of partial pressure = Q_p

Q_p=\frac{P_z}{P_x\times P_y}=\frac{1.0 atm}{1.0 atm\times 0.50 atm}

Q_p=2

Q_p>K_pthe equilibrium will move in backword direction that is in the left direction.

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