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2 years ago

calculate pressure exerted by 1.255 mol of CI2 in a volume of 5.005 L at a temperature 273.5 k using ideal gas equation

Chemistry

1 answer:

balu736 [363]2 years ago

8 0

Answer:

The pressure is 5.62 atm.

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

P= ?
V= 5.005 L
n= 1.255 mol
R= 0.082 $\frac{atm*L}{mol*K}$
T= 273.5 K

Replacing:

P* 5.005 L= 1.255 mol* 0.082 $\frac{atm*L}{mol*K}$ *273.5 K

Solving:

$P=\frac{1.255 mol* 0.082 \frac{atm*L}{mol*K} *273.5 K}{5.005 L}$

P= 5.62 atm

<u><em>The pressure is 5.62 atm.</em></u>

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Answer:

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At a certain concentration of H2 and NH3, the initial rate of reaction is 0.120 M / s. What would the initial rate of the reacti

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The question is incomplete, here is the complete question:

The rate of certain reaction is given by the following rate law:

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As we are given that:

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Dividing 2 by 1, we get:

$\frac{R}{0.120}=\frac{k(\frac{[H_2]}{2})^2[NH_3]}{k[H_2]^2[NH_3]}$

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Answer:

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