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Equilibrium Processes Chemical Equilibrium Chemistry Class 11th

If 80g of copper sulphate CuSO₄ $\cdot$ 5H₂O is dissolved in deionized water to make 5L of solution. The concentration of the copper sulphate solution is x × 10^-3 mol L^-1. The value of x is________.

[Atomic masses Cu : 63.54u, S : 32u, O : 16u, H : 1u]

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alok kumar singh | Contributor-Level 10

3 months ago

Mass of CuSO₄. 5H₂O = 80 g

Volume of solution = 5L

Molar mass of CuSO₄.5H₂O = 249.54g/ml

$C o n c e n t r a t i o n = \frac{m o l e s}{v o l u m e o f s o l u t i o n}$

$\begin{array}{l} = \frac{0.32}{5} = 0.064 M \\ = 64 \times 1 0^{- 3} M \end{array}$

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Value of K_p for the equilibrium reaction N₂O_4(g) $\overset{}{?}$ 2NO_2(g) at 288 K is 47.9. The K_c for this reaction at same temperature is_________. (Nearest integer)

(R = 0.083 L bar K^-1 mol^-1)

alok kumar singh

K_p = 47.9 T = 288 K

K_C =? R = 0.083 L bar/K mol

$N_{2} O_{4} (g) ? 2 N O_{2} (g)$

Using

$K_{p} = K_{C} {(R T)}^{Δ n g}$

Here ;

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49.7 = K_C (0.083 × 288)¹

K_C = 2

When 5.1g of solid NH₄HS is introduced into a two litre evacuated flask at 27°C, 20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The K_p for the reaction at 27°C is x × 10^-2. The value of x is_______. (Integer answer)

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alok kumar singh

Moles of NH₄HS initially taken = $\frac{5.1}{51} = 0.1 m o l$

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t = $\infty$ 0 0.1 mol 0 0

t = $\infty$ 0.1 (1 - 0.2) 0.1 × 0.2 0.1 × 0.2

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The equilibrium constant K_c at 298 K for the reaction

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alok kumar singh

For equation A + B $? C + D$

$K_{C} = \frac{[C] [D]}{[A] [B]} = 100 a t 298 K$

Here; A + B $?$ C + D

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eq. (1-x) (1-x) (1-x) (1-x)

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If 80g of copper sulphate CuSO₄ $\cdot$ 5H₂O is dissolved in deionized water to make 5L of solution. The concentration of the copper sulphate solution is x × 10^-3 mol L^-1. The value of x is________.

[Atomic masses Cu : 63.54u, S : 32u, O : 16u, H : 1u]

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If 80g of copper sulphate CuSO4 ⋅ 5H2O is dissolved in deionized water to make 5L of solution. The concentration of the copper sulphate solution is x × 10-3 mol L-1. The value of x is________. [Atomic masses Cu : 63.54u, S : 32u, O : 16u, H : 1u]

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If 80g of copper sulphate CuSO₄ $\cdot$ 5H₂O is dissolved in deionized water to make 5L of solution. The concentration of the copper sulphate solution is x × 10^-3 mol L^-1. The value of x is________.

[Atomic masses Cu : 63.54u, S : 32u, O : 16u, H : 1u]