1
JEE Main 2016 (Offline)
+4
-1
The equilibrium constant at 298 K for a reaction A + B $$\leftrightharpoons$$ C + D is 100. If the initial concentration of all the four species were 1M each, then equilibrium concentration of D (in mol L–1) will be:
A
0.818
B
1.818
C
1.182
D
0.182
2
JEE Main 2015 (Offline)
+4
-1
The standard Gibbs energy change at 300 K for the reaction 2A $$\leftrightharpoons$$ B + C is 2494.2 J. At a given time, the composition of the reaction mixture is [A] = 1/2, [B] = 2 and [C] = 1/2. The reaction proceeds in the: [R = 8.314 J/K/mol, e = 2.718]
A
reverse direction because Q > Kc
B
forward direction because Q < Kc
C
reverse direction because Q < Kc
D
forward direction because Q > Kc
3
JEE Main 2014 (Offline)
+4
-1
For the reaction SO2 (g) + $${1 \over 2} O_2(g) \leftrightharpoons$$ SO3(g).
if KP = KC(RT)x where the symbols have usual meaning then the value of x is: (assuming ideality)
A
-1
B
-1/2
C
1/2
D
1
4
AIEEE 2012
+4
-1
The equilibrium constant (KC) for the reaction N2(g) + O2(g) $$\to$$ 2NO(g) at temperature T is 4 $$\times$$ 10–4. The value of KC for the reaction, NO(g) $$\to$$ 1/2N2(g) + 1/2O2(g) at the same temperature is :
A
0.02
B
2.5 $$\times$$ 102
C
4 $$\times$$ 10-4
D
50.0
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