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Question
Equilibrium constant, Kc for the reaction
\[\ce{N2 (g) + 3H2 (g) ⇌ 2NH3 (g)}\] at 500 K is 0.061.
At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L–1 N2, 2.0 mol L–1 H2 and 0.5 mol L–1 NH3. Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?
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Solution
The given reaction is:
| N2(g) | + | 3H2(g) | ↔ | 2NH3(g) | |
| At a particular time | 3.0 mol L-1 | 2.0 mol L-1 | 0.5 mol L-1 |
Now, we know that,
`"Q"_"C" = ["NH"_3]^2/(["N"_2]["H"_2]^3)`
` =(0.5)^2/((3.0)(2.0)^3)`
= 0.0104
it is given that `"K"_"C"` = 0.061
Since `"Q"_"C" != "K"_"C"`, the reaction is not at equilibrium.
Since `"Q"_"C" < "K"_"C"`, the reaction will proceed in the forward direction to reach equilibrium.
RELATED QUESTIONS
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
\[\ce{CH3COOH (l) + C2H5OH (l) ⇌ CH3COOC2H5 (l) + H2O (l)}\]
Write the concentration ratio (reaction quotient), Qc, for this reaction (note: water is not in excess and is not a solvent in this reaction).
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
\[\ce{CH3COOH (l) + C2H5OH (l) ⇌ CH3COOC2H5 (l) + H2O (l)}\]
At 293 K, if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.
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Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after sometime. Has equilibrium been reached?
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\[\ce{\underset{(pink)}{[Co(H2O)6]^{3+}} (aq) + 4Cl- (qa) ⇌ \underset{(blue)}{[CoCl4]^{2-}} (aq) + 6H2O (l)}\]
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