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katen-ka-za [31]
3 years ago
14

In an exothermic reaction, heat can be considered a __________.

Chemistry
2 answers:
GenaCL600 [577]3 years ago
7 0
Answer is: product of reaction.
<span>There are two types of reaction: endothermic reaction (chemical reaction that absorbs more energy than it releases) and exothermic reaction (chemical reaction that releases more energy than it absorbs). 
</span><span>According to Le Chatelier's principle when the reaction is exothermic heat is included as a product.</span>
OlgaM077 [116]3 years ago
4 0
In an exothermic reaction, heat can be considered a product while in an endothermic reaction heat can be considered a reactant.
Exothermic reaction is a chemical reaction that releases energy in form of light or heat to the surroundings. The total energy of the products is less than the total energy of the reactants, thus the change in enthalpy is negative. Endothermic reactions on the other hand are chemical reactions in which heat is absorbed from the surroundings. 
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Read 2 more answers
Given the initial rate data for the reaction being A + B + C --&gt; D determine the rate expression for the reaction and the (k)
Vesnalui [34]

Answer:

k = 100 mol⁻² L² s⁻¹, r= k[A][B]²

Explanation:

A + B + C --> D

[A] [B] [C] IRR

0.20 0.10 0.40 .20

0.40 0.20 0.20 1.60

0.20 0.10 0.20 .20

0.20 0.20 0.20 .80

Comparing the third and fourth reaction, the concentrations of A and C are constant. Doubling the concentration of B causes a change in the rate of the reaction by a factor of 4.

This means the rate of reaction is second order with respect to B.

Comparing reactions 2 and 3, the concentrations of B and C are constant. Halving the concentration of A causes a change in the rate of the reaction by a factor of 2.

This means the rate of reaction is first order with respect to A.

Comparing reactions 1 and 3, the concentrations of A and B are constant. Halving the concentration of A causes no change in the rate of the reaction.

This means the rate of reaction is zero order with respect to C.

The rate expression for this reaction is given as;

r = k [A]¹[B]²[C]⁰

r= k[A][B]²

In order to obtain the value of the rate constant, let's work with the first reaction.

r = 0.20

[A] = 0.20 [B] = 0.10

k = r / [A][B]²

k = 0.20 / (0.20)(0.10)²

k = 100 mol⁻² L² s⁻¹

8 0
3 years ago
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