Which statement is true about a catalyst?
1 answer:
Answer:
C. A catalyst lowers the activation energy of a reaction.
Explanation:
- Catalyst increases the rate of the reaction without affecting the equilibrium position.
- Catalyst increases the rate via lowering the activation energy of the reaction.
- This can occur via passing the reaction in alternative pathway (changing the mechanism).
- The activation energy is the difference in potential energies between the reactants and transition state (for the forward reaction) and it is the difference in potential energies between the products and transition state (for the reverse reaction).
- in the presence of a catalyst, the activation energy is lowered by lowering the energy of the transition state, which is the rate-determining step, catalysts reduce the required energy of activation to allow a reaction to proceed and, in the case of a reversible reaction, reach equilibrium more rapidly.
- Catalyst does not consumed during a chemical reaction.
Kindly, find the attached image.
- So, the right choice is:
<em>C. A catalyst lowers the activation energy of a reaction.</em>
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Solution us here,
let the rate of diffusion of H2(r1) be x and⁷ the rate of diffusion of gas(r2) be x+x/6=7x/6.
Molar mass of H2 (M1)=2 g
Molar mass of gas(M2)= ?
Now, from the Ghram's law of diffusion of gas,
here, it looks like I have done wrong.
But all of the answers in option are wrong.
Because, rate of diffusion of any gas is inversely proportional to the square root of its malor mass.
And in the question, gas has higher rate of diffusion than hrdrogen. So it should have molar mass less than hydrogen.