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zysi [14]
3 years ago
13

Consider the following equilibrium: CO2(g) + C(graphite) 2CO(g); ΔH = 172.5 kJ The equilibrium constant for this reaction will

Chemistry
1 answer:
bezimeni [28]3 years ago
8 0

Answer: Option (B) is the correct answer.

Explanation:

As the given reaction is as follows.

               CO_{2}(g) + C(graphite) \rightarrow 2CO(g)

Equilibrium constant for this reaction will be as follows.

             K_{c} = \frac{[CO_{2}]}{[CO]^{2}}

According to Le Chatelier's principle, when we increase the temperature then the equilibrium will shift towards the right hand side.

As a result, concentration of carbon dioxide will decrease whereas concentration of carbon monoxide will increase.

Thus, we can conclude that in the given reaction equilibrium constant for this reaction will decrease with increasing temperature.

 

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3 years ago
Identify the unit cell that has a = B = y = 90°.
elixir [45]

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8 0
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What will the volume be of 50 moles of helium at 25°C and 2.5 atm?​
yulyashka [42]
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7 0
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8. Which type of bond results when one or more valence
Gekata [30.6K]

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B

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8 0
3 years ago
The volume of carbon gas at 5.0 ATM was measured to be 363 ml. What will the pressure be if the volume is change to .00020 ml?
aleksley [76]

Answer:

The answer to your question is P2 = 9075000 atm

Explanation:

Data

Pressure 1 = P1 = 5 atm

Volume 1 = V1 = 363 ml

Pressure 2 = P2 = ?

Volume 2 = 0.0002 ml

Process

To solve this problem use Boyle's law

                 P1V1 = P2V2

-Solve for P2

                 P2 = P1V1/V2

-Substitution

                  P2 = (5 x 363) / 0.0002

-Simplification

                  P2 = 1815 / 0.0002

-Result

                 P2 = 9075000 atm

5 0
3 years ago
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