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weeeeeb [17]
3 years ago
8

If a chemical reaction catalyzed by an enzyme is being carried out, and there is a sudden, drastic decrease in temperature, what

is most likely to happen next?. A. Enzyme activity will decrease, and the reaction will proceed very slowly, or possibly not at all.. B. Less heat will be lost to the environment, and the reaction will take place more efficiently.. C. The reaction will proceed more quickly since the activation energy is decreased.. D. The reaction rate will decrease and eventually return to normal as the enzyme adapts to the temperature change.
Chemistry
2 answers:
LenaWriter [7]3 years ago
5 0

If a chemical reaction catalyzed by an enzyme is being carried out, and there is a sudden, drastic decrease in temperature, the thing that will most likely to happen next is going to be the :

“enzyme activity will decrease, and the reaction will proceed very slowly, or possibly not at all.“

Explanation:

This compliance is required to how enzymes bind to other molecules and cause chemical reactions to occur on those molecules. Lowering the temperature reduces the motion of molecules and atoms, expecting this compliance is reduced or lost. As the temperature decreases, so do enzyme activity. While higher temperatures do increase the activity of enzymes and the rate of reactions,

insens350 [35]3 years ago
4 0

If a chemical reaction catalyzed by an enzyme is being carried out, and there is a sudden, drastic decrease in temperature, the thing that will most likely to happen next is going to be the “enzyme activity will decrease, and the reaction will proceed very slowly, or possibly not at all.“ The correct answer between all the choices given is the first choice or letter A. I am hoping that this answer has satisfied your query and it will be able to help you, and if you would like, feel free to ask another question.

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A 825 g iron block is heated to 352 degrees C and is placed in an insulated container (of negligible heat capacity) containing 4
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Answer : The final equilibrium temperature of the water and iron is, 537.12 K

Explanation :

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

q_1=-q_2

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c_1 = specific heat of iron =  560 J/(kg.K)

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m_2 = mass of water = 40 g

T_f = final temperature of water and iron = ?

T_1 = initial temperature of iron = 352^oC=273+352=625K

T_2 = initial temperature of water = 20^oC=273+20=293K

Now put all the given values in the above formula, we get:

(825\times 10^{-3}kg)\times 560J/(kg.K)\times (T_f-625K)=-(40\times 10^{-3}kg)\times 4186J/(kg.K)\times (T_f-293K)

T_f=537.12K

Therefore, the final equilibrium temperature of the water and iron is, 537.12 K

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