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1 answer:
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Answer:
Increasing temperature
Explanation:
Enthalpy of the reaction = -393.5 kJ/mol
Negative sign implies that reaction is exothermic.
Effect of change in reaction condition is explained by Le chateliers principle.
According to Le chateliers principle, if the reaction conditions of a reversible reaction in a state of dynamic equilibirum is changed, the reaction will move in a direction to counteract the change.
1. Increasing the temperature
Forward reaction is exothermic that means temperature increases in forward direction. Backward reaction will be endothermic and so there is decrease in temperature in backward direction or in left direction.
On increasing temperature, reaction will be move in direction to counteract the increased temperature, therefore reaction will move in left direction.
2. Adding O2
If O2 is added, then reaction will move in a direction in which its get consumed. So, reaction will move in forward direction or in right direction.
3. Removing C (s)
Le Chatelier's principle does not apply on solids, so removal of C(s) does not affect the equilibrium.
Answer: (a) The reaction mixture will proceed toward products.
Explanation:
Equilibrium constant is defined as the ratio of pressure of products to the pressure of reactants each raised to the power their stoichiometric ratios. It is expressed as
K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.
For the given chemical reaction:
The expression for is written as:
Thus as , the reaction will shift towards the right i.e. towards the product side.