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xxTIMURxx [149]
3 years ago
9

How does changing the temperature affect the chemical reaction?

Chemistry
1 answer:
Rufina [12.5K]3 years ago
4 0

Answer:

C

Explanation:

Temperature is directly related to kinetic energy (KE). As we raise temperature, we are raising KE, as well. Particles with more KE move more quickly and with more force.

This means that these particles are more likely to collide with each other and react to allow the chemical reaction to follow through. In turn, if the chemical reaction is more likely to go to completion, the reaction rate increases, eliminating A and B.

The concentration of the solute is not affected by the temperature; in other words, temperature will not increase or decrease the amount of solute in the solution, so eliminate D.

Thus the answer is C.

Hope this helps!

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2. if 0.20 m fe3 had been used instead of 0.020 m fe3 , how would the numerical value of the rate constant and the activation en
dezoksy [38]

the calculated value is Ea is 18.2 KJ and A is 12.27.

According to the exponential part in the Arrhenius equation, a reaction's rate constant rises exponentially as the activation energy falls. The rate also grows exponentially because the rate of a reaction is precisely proportional to its rate constant.

At 500K, K=0.02s−1

At 700K, k=0.07s −1

The Arrhenius equation can be used to calculate Ea and A.

RT=k=Ae Ea

lnk=lnA+(RT−Ea)

At 500 K,

ln0.02=lnA+500R−Ea

500R Ea (1) At 700K lnA=ln (0.02) + 500R

lnA = ln (0.07) + 700REa (2)

Adding (1) to (2)

700REa100R1[5Ea-7Ea] = 0.02) +500REa=0.07) +700REa.

=ln [0.02/0 .07]

Ea= 2/35×100×8.314×1.2528

Ea =18227.6J

Ea =18.2KJ

Changing the value of E an in (1),

lnA=0.02) + 500×8.314/18227.6

= (−3.9120) +4.3848

lnA=0.4728

logA=1.0889

A=antilog (1.0889)

A=12.27

Consequently, Ea is 18.2 KJ and A is 12.27.

Learn more about Arrhenius equation here-

brainly.com/question/12907018

#SPJ4

5 0
1 year ago
Cual es la diferencia entre capacidad termica calor especifico y calor latente
gayaneshka [121]

Answer:

?

Explanation:

5 0
2 years ago
In a sample of oxygen gas at room temperature, the average kinetic energy of all the balls stays constant. Which postulate of ki
ipn [44]

The kinetic energy of gas particles depends on temperature. Greater the temperature higher will be the average kinetic energy

Kinetic energy is related to the temperature as:

KE = 3/2 kT

where k = Boltzmann constant

T = temperature

In the given example, since the temperature of O2 gas is maintained at room temperature, the average KE will also remain constant.

The fifth postulate of the kinetic molecular theory which states that the temperature of the gas depends on the average KE of the particles of the gas explains the above observation.

6 0
3 years ago
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storchak [24]
I say the Correct answer is
 
B)  There will be a shift toward the products.
8 0
2 years ago
Plz answer and you will get 5+ points
serg [7]
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