QBManager

Chemical Equilibrium

229156 The yield of the products in the reaction,
$A_{2} (g) + 2 B (g) ⇌ C (g) + Q (kJ)$
would be higher at

1 high temperature and high pressure

2 high temperature and low pressure

3 low temperature and high pressure

4 low temperature and low pressure

Explanation:

$A_{2} (g) + 2 B (g) ⇌ C (g) + QkJ$
The forward reaction is exothermic. Thus, according to Le-Chatelier's principal, the lower is temperature, greater would be the yield of ammonia. Also, the forward reaction occurs with decrease in number of gaseous molecules. Thus according to Le-Chatelier's principal an increase in pressure, will shift the equilibrium in a direction in which the number of gaseous molecules decreases. In other word high pressure will favour the formation of products.

[NEET-2018]

Chemical Equilibrium

229157 The supply of oxygen to tissues by blood, can be explained by

1 Le-Chatelier's principle

2 Boyle's law

3 Charis' law

4 Dalton's law

Explanation:

Le-Chatelier's principle drives the following reaction forward as blood passes through the alveoli
$H^{+} + {HCO}_{3} \to H_{2} {CO}_{3} \to {CO}_{2} + H_{2} O$
The carbon dioxide produced here continually diffuses into the alveoli and is exhaled, ensuring favorable kinetics for the reaction to proceed. Thus, correct answer is option (a).

Shift-II

Chemical Equilibrium

229158 ${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$ at constant temp, the pressure will increase if:

1 Vol. of container increase

2 Temperature increases

3 Concentration of

CaO

increases.

4 Concentration of

{CaCO}_{3}

increases.

Explanation:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$
$K_{p} = P_{{CO}_{2}}$
Pressure will increase only be increasing temperature as it will change $K_{p}$ value.

AIIMS-27.05.2018-(E)

Chemical Equilibrium

229160 In a reaction $A + B ⇌ C + D$ , Le Chatelier's principle asserts that an equilibrium between $A$ and $B$ producing $C$ and $D$ can be shifted towards $C$ and $D$ by
(i) increasing the concentration of $A$ or $B$
(ii) increasing the concentration of $C$ or $D$
(iii) decreasing the concentration of $A$ or $B$

1 (ii) only

2 Both (i) and (ii)

3 (iii) only

4 (i) only

Explanation:

$A + B ⇌ C + D$
Thus, in the given equilibria, if concentration of $A$ and $B$ is increased the reaction will move in forward direction to reduce the effect of increase in concentration of A and B. According to Le-Chatelier's principal, if a system in equilibrium is subjected to a change in any of the factors that determine the equilibrium conditions of a system then the equilibrium will shift in the direction so, as to reduce or to counteract the effects of the change

J and K CET-(2018)

Chemical Equilibrium

229161 A reaction has both $Δ H$ and $Δ S - v e$ . The rate of reaction

1 Increases with increases in temperature

2 Cannot be predicated for change in temperature

3 Increases with decreases in temperature

4 Remains unaffected by change in temperature

Explanation:

$Δ G = Δ H - T Δ S$
So, $Δ G = - ve$ then the $Δ S$ must be less than $Δ H$ i.e. $Δ H$ $> T Δ S$ .
Negative value of enthalpy change $Δ H$ corresponds to exothermic reaction with decrease in temperature, the rate of reaction increases, Hence the option (c) is correct.

Karnataka-CET-2017

Chemical Equilibrium

229156 The yield of the products in the reaction,
$A_{2} (g) + 2 B (g) ⇌ C (g) + Q (kJ)$
would be higher at

1 high temperature and high pressure

2 high temperature and low pressure

3 low temperature and high pressure

4 low temperature and low pressure

Explanation:

$A_{2} (g) + 2 B (g) ⇌ C (g) + QkJ$
The forward reaction is exothermic. Thus, according to Le-Chatelier's principal, the lower is temperature, greater would be the yield of ammonia. Also, the forward reaction occurs with decrease in number of gaseous molecules. Thus according to Le-Chatelier's principal an increase in pressure, will shift the equilibrium in a direction in which the number of gaseous molecules decreases. In other word high pressure will favour the formation of products.

[NEET-2018]

Chemical Equilibrium

229157 The supply of oxygen to tissues by blood, can be explained by

1 Le-Chatelier's principle

2 Boyle's law

3 Charis' law

4 Dalton's law

Explanation:

Le-Chatelier's principle drives the following reaction forward as blood passes through the alveoli
$H^{+} + {HCO}_{3} \to H_{2} {CO}_{3} \to {CO}_{2} + H_{2} O$
The carbon dioxide produced here continually diffuses into the alveoli and is exhaled, ensuring favorable kinetics for the reaction to proceed. Thus, correct answer is option (a).

Shift-II

Chemical Equilibrium

229158 ${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$ at constant temp, the pressure will increase if:

1 Vol. of container increase

2 Temperature increases

3 Concentration of

CaO

increases.

4 Concentration of

{CaCO}_{3}

increases.

Explanation:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$
$K_{p} = P_{{CO}_{2}}$
Pressure will increase only be increasing temperature as it will change $K_{p}$ value.

AIIMS-27.05.2018-(E)

Chemical Equilibrium

229160 In a reaction $A + B ⇌ C + D$ , Le Chatelier's principle asserts that an equilibrium between $A$ and $B$ producing $C$ and $D$ can be shifted towards $C$ and $D$ by
(i) increasing the concentration of $A$ or $B$
(ii) increasing the concentration of $C$ or $D$
(iii) decreasing the concentration of $A$ or $B$

1 (ii) only

2 Both (i) and (ii)

3 (iii) only

4 (i) only

Explanation:

$A + B ⇌ C + D$
Thus, in the given equilibria, if concentration of $A$ and $B$ is increased the reaction will move in forward direction to reduce the effect of increase in concentration of A and B. According to Le-Chatelier's principal, if a system in equilibrium is subjected to a change in any of the factors that determine the equilibrium conditions of a system then the equilibrium will shift in the direction so, as to reduce or to counteract the effects of the change

J and K CET-(2018)

Chemical Equilibrium

229161 A reaction has both $Δ H$ and $Δ S - v e$ . The rate of reaction

1 Increases with increases in temperature

2 Cannot be predicated for change in temperature

3 Increases with decreases in temperature

4 Remains unaffected by change in temperature

Explanation:

$Δ G = Δ H - T Δ S$
So, $Δ G = - ve$ then the $Δ S$ must be less than $Δ H$ i.e. $Δ H$ $> T Δ S$ .
Negative value of enthalpy change $Δ H$ corresponds to exothermic reaction with decrease in temperature, the rate of reaction increases, Hence the option (c) is correct.

Karnataka-CET-2017

Chemical Equilibrium

229156 The yield of the products in the reaction,
$A_{2} (g) + 2 B (g) ⇌ C (g) + Q (kJ)$
would be higher at

1 high temperature and high pressure

2 high temperature and low pressure

3 low temperature and high pressure

4 low temperature and low pressure

Explanation:

$A_{2} (g) + 2 B (g) ⇌ C (g) + QkJ$
The forward reaction is exothermic. Thus, according to Le-Chatelier's principal, the lower is temperature, greater would be the yield of ammonia. Also, the forward reaction occurs with decrease in number of gaseous molecules. Thus according to Le-Chatelier's principal an increase in pressure, will shift the equilibrium in a direction in which the number of gaseous molecules decreases. In other word high pressure will favour the formation of products.

[NEET-2018]

Chemical Equilibrium

229157 The supply of oxygen to tissues by blood, can be explained by

1 Le-Chatelier's principle

2 Boyle's law

3 Charis' law

4 Dalton's law

Explanation:

Le-Chatelier's principle drives the following reaction forward as blood passes through the alveoli
$H^{+} + {HCO}_{3} \to H_{2} {CO}_{3} \to {CO}_{2} + H_{2} O$
The carbon dioxide produced here continually diffuses into the alveoli and is exhaled, ensuring favorable kinetics for the reaction to proceed. Thus, correct answer is option (a).

Shift-II

Chemical Equilibrium

229158 ${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$ at constant temp, the pressure will increase if:

1 Vol. of container increase

2 Temperature increases

3 Concentration of

CaO

increases.

4 Concentration of

{CaCO}_{3}

increases.

Explanation:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$
$K_{p} = P_{{CO}_{2}}$
Pressure will increase only be increasing temperature as it will change $K_{p}$ value.

AIIMS-27.05.2018-(E)

Chemical Equilibrium

229160 In a reaction $A + B ⇌ C + D$ , Le Chatelier's principle asserts that an equilibrium between $A$ and $B$ producing $C$ and $D$ can be shifted towards $C$ and $D$ by
(i) increasing the concentration of $A$ or $B$
(ii) increasing the concentration of $C$ or $D$
(iii) decreasing the concentration of $A$ or $B$

1 (ii) only

2 Both (i) and (ii)

3 (iii) only

4 (i) only

Explanation:

$A + B ⇌ C + D$
Thus, in the given equilibria, if concentration of $A$ and $B$ is increased the reaction will move in forward direction to reduce the effect of increase in concentration of A and B. According to Le-Chatelier's principal, if a system in equilibrium is subjected to a change in any of the factors that determine the equilibrium conditions of a system then the equilibrium will shift in the direction so, as to reduce or to counteract the effects of the change

J and K CET-(2018)

Chemical Equilibrium

229161 A reaction has both $Δ H$ and $Δ S - v e$ . The rate of reaction

1 Increases with increases in temperature

2 Cannot be predicated for change in temperature

3 Increases with decreases in temperature

4 Remains unaffected by change in temperature

Explanation:

$Δ G = Δ H - T Δ S$
So, $Δ G = - ve$ then the $Δ S$ must be less than $Δ H$ i.e. $Δ H$ $> T Δ S$ .
Negative value of enthalpy change $Δ H$ corresponds to exothermic reaction with decrease in temperature, the rate of reaction increases, Hence the option (c) is correct.

Karnataka-CET-2017

Chemical Equilibrium

229156 The yield of the products in the reaction,
$A_{2} (g) + 2 B (g) ⇌ C (g) + Q (kJ)$
would be higher at

1 high temperature and high pressure

2 high temperature and low pressure

3 low temperature and high pressure

4 low temperature and low pressure

Explanation:

$A_{2} (g) + 2 B (g) ⇌ C (g) + QkJ$
The forward reaction is exothermic. Thus, according to Le-Chatelier's principal, the lower is temperature, greater would be the yield of ammonia. Also, the forward reaction occurs with decrease in number of gaseous molecules. Thus according to Le-Chatelier's principal an increase in pressure, will shift the equilibrium in a direction in which the number of gaseous molecules decreases. In other word high pressure will favour the formation of products.

[NEET-2018]

Chemical Equilibrium

229157 The supply of oxygen to tissues by blood, can be explained by

1 Le-Chatelier's principle

2 Boyle's law

3 Charis' law

4 Dalton's law

Explanation:

Le-Chatelier's principle drives the following reaction forward as blood passes through the alveoli
$H^{+} + {HCO}_{3} \to H_{2} {CO}_{3} \to {CO}_{2} + H_{2} O$
The carbon dioxide produced here continually diffuses into the alveoli and is exhaled, ensuring favorable kinetics for the reaction to proceed. Thus, correct answer is option (a).

Shift-II

Chemical Equilibrium

229158 ${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$ at constant temp, the pressure will increase if:

1 Vol. of container increase

2 Temperature increases

3 Concentration of

CaO

increases.

4 Concentration of

{CaCO}_{3}

increases.

Explanation:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$
$K_{p} = P_{{CO}_{2}}$
Pressure will increase only be increasing temperature as it will change $K_{p}$ value.

AIIMS-27.05.2018-(E)

Chemical Equilibrium

229160 In a reaction $A + B ⇌ C + D$ , Le Chatelier's principle asserts that an equilibrium between $A$ and $B$ producing $C$ and $D$ can be shifted towards $C$ and $D$ by
(i) increasing the concentration of $A$ or $B$
(ii) increasing the concentration of $C$ or $D$
(iii) decreasing the concentration of $A$ or $B$

1 (ii) only

2 Both (i) and (ii)

3 (iii) only

4 (i) only

Explanation:

$A + B ⇌ C + D$
Thus, in the given equilibria, if concentration of $A$ and $B$ is increased the reaction will move in forward direction to reduce the effect of increase in concentration of A and B. According to Le-Chatelier's principal, if a system in equilibrium is subjected to a change in any of the factors that determine the equilibrium conditions of a system then the equilibrium will shift in the direction so, as to reduce or to counteract the effects of the change

J and K CET-(2018)

Chemical Equilibrium

229161 A reaction has both $Δ H$ and $Δ S - v e$ . The rate of reaction

1 Increases with increases in temperature

2 Cannot be predicated for change in temperature

3 Increases with decreases in temperature

4 Remains unaffected by change in temperature

Explanation:

$Δ G = Δ H - T Δ S$
So, $Δ G = - ve$ then the $Δ S$ must be less than $Δ H$ i.e. $Δ H$ $> T Δ S$ .
Negative value of enthalpy change $Δ H$ corresponds to exothermic reaction with decrease in temperature, the rate of reaction increases, Hence the option (c) is correct.

Karnataka-CET-2017

Chemical Equilibrium

229156 The yield of the products in the reaction,
$A_{2} (g) + 2 B (g) ⇌ C (g) + Q (kJ)$
would be higher at

1 high temperature and high pressure

2 high temperature and low pressure

3 low temperature and high pressure

4 low temperature and low pressure

Explanation:

$A_{2} (g) + 2 B (g) ⇌ C (g) + QkJ$
The forward reaction is exothermic. Thus, according to Le-Chatelier's principal, the lower is temperature, greater would be the yield of ammonia. Also, the forward reaction occurs with decrease in number of gaseous molecules. Thus according to Le-Chatelier's principal an increase in pressure, will shift the equilibrium in a direction in which the number of gaseous molecules decreases. In other word high pressure will favour the formation of products.

[NEET-2018]

Chemical Equilibrium

229157 The supply of oxygen to tissues by blood, can be explained by

1 Le-Chatelier's principle

2 Boyle's law

3 Charis' law

4 Dalton's law

Explanation:

Le-Chatelier's principle drives the following reaction forward as blood passes through the alveoli
$H^{+} + {HCO}_{3} \to H_{2} {CO}_{3} \to {CO}_{2} + H_{2} O$
The carbon dioxide produced here continually diffuses into the alveoli and is exhaled, ensuring favorable kinetics for the reaction to proceed. Thus, correct answer is option (a).

Shift-II

Chemical Equilibrium

229158 ${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$ at constant temp, the pressure will increase if:

1 Vol. of container increase

2 Temperature increases

3 Concentration of

CaO

increases.

4 Concentration of

{CaCO}_{3}

increases.

Explanation:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$
$K_{p} = P_{{CO}_{2}}$
Pressure will increase only be increasing temperature as it will change $K_{p}$ value.

AIIMS-27.05.2018-(E)

Chemical Equilibrium

229160 In a reaction $A + B ⇌ C + D$ , Le Chatelier's principle asserts that an equilibrium between $A$ and $B$ producing $C$ and $D$ can be shifted towards $C$ and $D$ by
(i) increasing the concentration of $A$ or $B$
(ii) increasing the concentration of $C$ or $D$
(iii) decreasing the concentration of $A$ or $B$

1 (ii) only

2 Both (i) and (ii)

3 (iii) only

4 (i) only

Explanation:

$A + B ⇌ C + D$
Thus, in the given equilibria, if concentration of $A$ and $B$ is increased the reaction will move in forward direction to reduce the effect of increase in concentration of A and B. According to Le-Chatelier's principal, if a system in equilibrium is subjected to a change in any of the factors that determine the equilibrium conditions of a system then the equilibrium will shift in the direction so, as to reduce or to counteract the effects of the change

J and K CET-(2018)

Chemical Equilibrium

229161 A reaction has both $Δ H$ and $Δ S - v e$ . The rate of reaction

1 Increases with increases in temperature

2 Cannot be predicated for change in temperature

3 Increases with decreases in temperature

4 Remains unaffected by change in temperature

Explanation:

$Δ G = Δ H - T Δ S$
So, $Δ G = - ve$ then the $Δ S$ must be less than $Δ H$ i.e. $Δ H$ $> T Δ S$ .
Negative value of enthalpy change $Δ H$ corresponds to exothermic reaction with decrease in temperature, the rate of reaction increases, Hence the option (c) is correct.

Karnataka-CET-2017