On a cool morning (12"C), a balloon is filled with 1.5 L of helium. By mid afternoon, the temperature has soared to 32°C. What i
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The given question is incomplete. The complete question is :
For the reaction at equilibrium, which statement correctly describes the effects of increasing pressure and adding
, respectively
a) Increasing pressure causes shift to reactants, adding causes shift to products.
b) Increasing pressure causes shift to products ,adding causes shift to reactants.
c) Increasing pressure causes shift to products, adding causes shift to products.
d) Increasing pressure causes shift to reactants,adding causes shift to reactants
Answer: Increasing pressure causes shift to reactants, adding causes shift to products.
Explanation:
Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.
This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.
For the given equation:
a) If the pressure is increased, the volume will decrease according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. As the number of moles of gas molecules is lesser at the reactant side. So, the equilibrium will shift in the left direction. i.e. towards reactants.
b) If is added, the equilibrium will shift in the direction where
is decreasing. So, the equilibrium will shift in the right direction. i.e. towards products.
Explanation :
In the given case different law related to gas is given. The attached figure shows the required solution.
Boyle's law states that the pressure is inversely proportional to the volume of the gas i.e.
k is a constant.
Charle's law states that the volume of directly proportional to the temperature of the gas.
Combined gas law is the combination of the pressure, volume and the temperature of the gas i.e.
Hence, this is the required solution.
