If the activation energy required for a chemical reaction were reduced, what would happen to the rate of the reaction?
2 answers:
Answer: The rate would increase.
Explanation:
Activation energy is the extra energy that must be supplied to reactants in order to cross the energy barrier and thus convert to products.
A chemical reaction which involves lower activation energy, means more molecules will gain sufficient energy to cross the energy barrier, thus effective collisions increase and more products will be formed and hence the rate of reaction would increase.
The effect of catalyst on activation energy is shown in the image below:
You might be interested in
Answer:
The correct answer would be- 1:1:1:1.
Explanation:
According to the question the cross between the two pea plants with the genotype RrYy and rryy where R for round seeds and r for recessive form that expressed wrinkled seed character. The other character of this dihybrid cross is the color of the seds Y for green and y for yellow seeds.
The cross is shown in the image attached that suggests that phenotypic ratio would be 1:1:1:1 as RrYy, Rryy, rrYy, and rryy.
Thus, the correct answer is : 1:1:1:1.
