229186
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ + heat. What is the effect of the increase of temperature on the equilibrium of the reaction?
1 Equilibrium is shifted to the left
2 Equilibrium is shifted to the right
3 Equilibrium is unaltered
4 Reaction rate does not change
Explanation:
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}+$ heat It is an exothermic reaction, so high temperature favours backward reaction. Hence, equilibrium is shifted towards the left.
KARNATAKA-CET
Chemical Equilibrium
229187
What happens to the yield on application of high pressure in the Haber's synthesis of ammonia?
1 Increases
2 decreases
3 unaffected
4 reaction stops
Explanation:
Haber's process of synthesis of ammonia $\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ High pressure favours the reaction that decrease the number of gas molecules. Since, the number of molecules of gaseous products are less than the number of molecules of gaseous reactants, thus according to Lechatelier's principal, high pressure favour the forward reaction. i.e more ammonia will be abtained.
J and K CET-(2008)
Chemical Equilibrium
229190
When hydrogen molecule decompose into it's atoms which consitions gives maximum yields of $\mathrm{H}$ atoms?
1 High temperature and low pressure
2 Low temperature and high pressure
3 High temperature and high pressure
4 Low temperature and low pressure
Explanation:
$\mathrm{H}_{2} \rightarrow 2 \mathrm{H}-\Delta \mathrm{H}$ The reaction is endothermic accompanied by increase in the number of moles. According to Le-chatelier's principal, to increase the rate of forward reaction. temperature should be increased and pressure should be decrease.
BITSAT-2007
Chemical Equilibrium
229191
Given the equilibrium system: $\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$ $(\Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol})$. What change will shift the equilibrium to the right?
1 Decreasing the temperature
2 Increasing the temperature
3 Dissolving $\mathrm{NaCl}$ crystals in the equilibrium mixture
4 Dissolving $\mathrm{NH}_{4} \mathrm{NO}_{3}$ crystals in the equilibrium mixture
Explanation:
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}), \Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol}$ Endothermic reactions are favoured at high temperature. Therefore, increasing the temperature will shift equilibrium to the right.
229186
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ + heat. What is the effect of the increase of temperature on the equilibrium of the reaction?
1 Equilibrium is shifted to the left
2 Equilibrium is shifted to the right
3 Equilibrium is unaltered
4 Reaction rate does not change
Explanation:
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}+$ heat It is an exothermic reaction, so high temperature favours backward reaction. Hence, equilibrium is shifted towards the left.
KARNATAKA-CET
Chemical Equilibrium
229187
What happens to the yield on application of high pressure in the Haber's synthesis of ammonia?
1 Increases
2 decreases
3 unaffected
4 reaction stops
Explanation:
Haber's process of synthesis of ammonia $\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ High pressure favours the reaction that decrease the number of gas molecules. Since, the number of molecules of gaseous products are less than the number of molecules of gaseous reactants, thus according to Lechatelier's principal, high pressure favour the forward reaction. i.e more ammonia will be abtained.
J and K CET-(2008)
Chemical Equilibrium
229190
When hydrogen molecule decompose into it's atoms which consitions gives maximum yields of $\mathrm{H}$ atoms?
1 High temperature and low pressure
2 Low temperature and high pressure
3 High temperature and high pressure
4 Low temperature and low pressure
Explanation:
$\mathrm{H}_{2} \rightarrow 2 \mathrm{H}-\Delta \mathrm{H}$ The reaction is endothermic accompanied by increase in the number of moles. According to Le-chatelier's principal, to increase the rate of forward reaction. temperature should be increased and pressure should be decrease.
BITSAT-2007
Chemical Equilibrium
229191
Given the equilibrium system: $\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$ $(\Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol})$. What change will shift the equilibrium to the right?
1 Decreasing the temperature
2 Increasing the temperature
3 Dissolving $\mathrm{NaCl}$ crystals in the equilibrium mixture
4 Dissolving $\mathrm{NH}_{4} \mathrm{NO}_{3}$ crystals in the equilibrium mixture
Explanation:
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}), \Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol}$ Endothermic reactions are favoured at high temperature. Therefore, increasing the temperature will shift equilibrium to the right.
229186
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ + heat. What is the effect of the increase of temperature on the equilibrium of the reaction?
1 Equilibrium is shifted to the left
2 Equilibrium is shifted to the right
3 Equilibrium is unaltered
4 Reaction rate does not change
Explanation:
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}+$ heat It is an exothermic reaction, so high temperature favours backward reaction. Hence, equilibrium is shifted towards the left.
KARNATAKA-CET
Chemical Equilibrium
229187
What happens to the yield on application of high pressure in the Haber's synthesis of ammonia?
1 Increases
2 decreases
3 unaffected
4 reaction stops
Explanation:
Haber's process of synthesis of ammonia $\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ High pressure favours the reaction that decrease the number of gas molecules. Since, the number of molecules of gaseous products are less than the number of molecules of gaseous reactants, thus according to Lechatelier's principal, high pressure favour the forward reaction. i.e more ammonia will be abtained.
J and K CET-(2008)
Chemical Equilibrium
229190
When hydrogen molecule decompose into it's atoms which consitions gives maximum yields of $\mathrm{H}$ atoms?
1 High temperature and low pressure
2 Low temperature and high pressure
3 High temperature and high pressure
4 Low temperature and low pressure
Explanation:
$\mathrm{H}_{2} \rightarrow 2 \mathrm{H}-\Delta \mathrm{H}$ The reaction is endothermic accompanied by increase in the number of moles. According to Le-chatelier's principal, to increase the rate of forward reaction. temperature should be increased and pressure should be decrease.
BITSAT-2007
Chemical Equilibrium
229191
Given the equilibrium system: $\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$ $(\Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol})$. What change will shift the equilibrium to the right?
1 Decreasing the temperature
2 Increasing the temperature
3 Dissolving $\mathrm{NaCl}$ crystals in the equilibrium mixture
4 Dissolving $\mathrm{NH}_{4} \mathrm{NO}_{3}$ crystals in the equilibrium mixture
Explanation:
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}), \Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol}$ Endothermic reactions are favoured at high temperature. Therefore, increasing the temperature will shift equilibrium to the right.
229186
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ + heat. What is the effect of the increase of temperature on the equilibrium of the reaction?
1 Equilibrium is shifted to the left
2 Equilibrium is shifted to the right
3 Equilibrium is unaltered
4 Reaction rate does not change
Explanation:
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}+$ heat It is an exothermic reaction, so high temperature favours backward reaction. Hence, equilibrium is shifted towards the left.
KARNATAKA-CET
Chemical Equilibrium
229187
What happens to the yield on application of high pressure in the Haber's synthesis of ammonia?
1 Increases
2 decreases
3 unaffected
4 reaction stops
Explanation:
Haber's process of synthesis of ammonia $\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ High pressure favours the reaction that decrease the number of gas molecules. Since, the number of molecules of gaseous products are less than the number of molecules of gaseous reactants, thus according to Lechatelier's principal, high pressure favour the forward reaction. i.e more ammonia will be abtained.
J and K CET-(2008)
Chemical Equilibrium
229190
When hydrogen molecule decompose into it's atoms which consitions gives maximum yields of $\mathrm{H}$ atoms?
1 High temperature and low pressure
2 Low temperature and high pressure
3 High temperature and high pressure
4 Low temperature and low pressure
Explanation:
$\mathrm{H}_{2} \rightarrow 2 \mathrm{H}-\Delta \mathrm{H}$ The reaction is endothermic accompanied by increase in the number of moles. According to Le-chatelier's principal, to increase the rate of forward reaction. temperature should be increased and pressure should be decrease.
BITSAT-2007
Chemical Equilibrium
229191
Given the equilibrium system: $\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$ $(\Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol})$. What change will shift the equilibrium to the right?
1 Decreasing the temperature
2 Increasing the temperature
3 Dissolving $\mathrm{NaCl}$ crystals in the equilibrium mixture
4 Dissolving $\mathrm{NH}_{4} \mathrm{NO}_{3}$ crystals in the equilibrium mixture
Explanation:
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightarrow \mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}), \Delta \mathrm{H}=+3.5 \mathrm{kcal} / \mathrm{mol}$ Endothermic reactions are favoured at high temperature. Therefore, increasing the temperature will shift equilibrium to the right.
