1
JEE Advanced 2016 Paper 2 Offline
+3
-0
Paragraph
Thermal decomposition of gaseous X2 to gaseous X at 298 K takes place according to the following equations:
X2 (g) $$\leftrightharpoons$$ 2X (g)
The standard reaction Gibbs energy, $$\Delta _rG^o$$, of this reaction is positive. At the start of the reaction, there is one mole of X2 and no X. As the reaction proceeds, the number of moles of X formed is given by $$\beta$$. Thus, $$\beta _{equilibrium}$$ is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given R = 0.083 L bar K-1 mol-1)
Question
The equilibrium constant Kp for this reaction at 298 K, in terms of $$\beta _{equilibrium}$$, is
A
$${{8\beta _{equilibrium}^2} \over {2 - {\beta _{equilibrium}}}}$$
B
$${{8\beta _{equilibrium}^2} \over {4 - {\beta _{equilibrium}^2}}}$$
C
$${{4\beta _{equilibrium}^2} \over {2 - {\beta _{equilibrium}}}}$$
D
$${{4\beta _{equilibrium}^2} \over {4 - {\beta _{equilibrium}^2}}}$$
2
JEE Advanced 2016 Paper 2 Offline
+3
-0
Paragraph
Thermal decomposition of gaseous X2 to gaseous X at 298 K takes place according to the following equations:
X2 (g) $$\leftrightharpoons$$ 2X (g)
The standard reaction Gibbs energy, $$\Delta _rG^o$$, of this reaction is positive. At the start of the reaction, there is one mole of X2 and no X. As the reaction proceeds, the number of moles of X formed is given by $$\beta$$. Thus, $$\beta _{equilibrium}$$ is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given R = 0.083 L bar K-1 mol-1)
Question
The INCORRECT statement among the following for this reaction, is
A
Decrease in the total pressure will result in formation of more moles of gaseous X
B
At the start of the reaction, dissociation of gaseous X2 takes place spontaneously
C
$${{\beta _{equilibrium}}}$$ = 0.7
D
Kc < 1
3
IIT-JEE 2008 Paper 2 Offline
+3
-1

Solubility product constants (K$$_{sp}$$) of salts of types MX, MX$$_2$$ and M$$_3$$X at temperature T are 4.0 $$\times$$ 10$$^{-8}$$, 3.2 $$\times$$ 10$$^{-14}$$ and 2.7 $$\times$$ 10$$^{-15}$$, respectively. Solubilities (mol dm$$^{-3}$$) of the salts at temperature 'T' are in the order:

A
MX > MX$$_2$$ > M$$_3$$X
B
M$$_3$$X > MX$$_2$$ > MX
C
MX$$_2$$ > M$$_3$$X > MX
D
MX > M$$_3$$X > MX$$_2$$
4
IIT-JEE 2008 Paper 1 Offline
+3
-1

2.5 mL of $$\frac{2}{5}$$M weak monoacidic base (K$$_b$$ = 1 $$\times$$ 10$$^{-12}$$ at 25$$^\circ$$C) is titrated with $$\frac{2}{15}$$M HCl in water at 25$$^\circ$$C. The concentration of H$$^+$$ at equivalence point is (K$$_w$$ = 1 $$\times$$ 10$$^{-14}$$ at 25$$^\circ$$C).

A
3.7 $$\times$$ 10$$^{-13}$$ M
B
3.2 $$\times$$ 10$$^{-7}$$ M
C
3.2 $$\times$$ 10$$^{-2}$$ M
D
2.7 $$\times$$ 10$$^{-2}$$ M
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