1
JEE Main 2019 (Online) 12th January Morning Slot
+4
-1
Two solids dissociate as follows –

The total pressure when both the solids dissociated simultaneously is -
A
(x + y) atm
B
$$\left( {\sqrt {x + y} } \right)$$ atm
C
2$$\left( {\sqrt {x + y} } \right)$$ atm
D
x2 + y2 atm
2
JEE Main 2019 (Online) 11th January Morning Slot
+4
-1
Consider the reaction
N2(g) + 3H2(g) $$\rightleftharpoons$$ 2NH3(g)

The equilibrium constant of the above reaction is Kp. If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that PNH3 << Ptotal at equilibrium)
A
$${{{3^{{3 \over 2}}}{K_P^{{1 \over 2}}}{P^2}} \over 4}$$
B
$${{K_P^{{1 \over 2}}{P^2}} \over 4}$$
C
$${{{3^{{3 \over 2}}}{K_P^{{1 \over 2}}}{P^2}} \over 16}$$
D
$${{K_P^{{1 \over 2}}{P^2}} \over 16}$$
3
JEE Main 2019 (Online) 10th January Evening Slot
+4
-1
5.1 g NH4SH is introduced in 3.0 L evacuated flask at 327ºC. 30% of the solid NH4SH decomposed to NH3 and H2S as gases . The Kp of the reaction at 327oC is (R = 0.082 L atm mol–1 K–1, Molar mass of S = 32 g mol–1 molar mass of N = 14 g mol–1)
A
0.242 $$\times$$ 10$$-$$4 atm2
B
1 $$\times$$ 10–4 atm2
C
4.9 $$\times$$ 10$$-$$3 atm2
D
0.242 atm2
4
JEE Main 2019 (Online) 10th January Morning Slot
+4
-1
The values of Kp/Kc for the following reactions at 300 K are, respectively : (At 300 K, RT = 24.62 dm3 atm mol–1)

N2(g) + O2(g)  $$\rightleftharpoons$$ 2 NO(g)

N2O4(g)  $$\rightleftharpoons$$   2 NO(g)

N2(g) + 3H2(g) $$\rightleftharpoons$$ 2 NH3(g)
A
24.62 dm3 atm mol–1, 606.0 dm6 atm2 mol–2 1.65 $$\times$$ 10–3 dm–6 atm–2 mol2
B
1,4.1 $$\times$$ 10–2 dm–3 atm–1 mol, 606 dm6 atm2 mol–2
C
1,24.62 dm3 atm mol–1 , 1.65 $$\times$$ 10–3 dm–6 atm –2 mol2
D
1, 24.62 dm3 atm mol–1, 606.0 dm6 atm2 mol–2
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