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sertanlavr [38]
2 years ago
13

If I have an unknown quantity of gas at a pressure of 204.83 kPa, a volume of 27.88 liters, and a temperature of 8.76°C , how ma

ny moles of gas do I have?​
Chemistry
2 answers:
Amiraneli [1.4K]2 years ago
8 0
Um what this answer is but I think 1.26
weeeeeb [17]2 years ago
6 0

Answer:

700

Explanation:

<u>How to find</u>

Multiply the volume and pressure and divide the product by the temperature and the molar gas constant to calculate the moles of the hydrogen gas.

Solve: 204.83 × 27.88 / 8.76 = 651.901872146

Which is 651.90

In the nearest hundredths, the moles of gas is 700

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Explanation:

The equilibrium reaction is

                           2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)

initially conc.         p            p                  0

At eqm.                p-2x        p-x               2x

Given: p_{NOCl}= 2x= 115torr

x=57.5 torr

The expression for equilibrium constant is :

K_p=\frac{p_{NOCl}^2}{p_{NO}^2\times p_{Cl_2}}

p_{NOCl} = 2x =115 torr

p_{NO} = (p-2x) = p-115 torr

p_{Cl_2} = (p-x)= p-57.5 torr

Now put all the given values in this expression, we get

0.27=\frac{(115)^2}{(p-115)^2\times (p-57.5)}

p=139.4torr

Therefore, the initial partial pressures of NO and Cl_2 is 139.4 torr.

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