Question

the pressure inside each of two identical cylinders is equal to atmospheric pressure. one cylinder contains hydrogen, the other nitrogen. both gases are at the same temperature. the number of moles of hydrogen is greater than the number of moles of nitrogen. less than the number of moles of nitrogen. equal to the number of moles of nitrogen.

Answer 1

The number of moles of hydrogen is equal to the number of moles of nitrogen.

According to the ideal gas equation

PV = nRT

where

• P = the pressure of the gas
• V = the volume of gas
• n = the total amount of ideal gas (moles)
• R = the universal gas constant
• T = the temperature

In the problems there are two identical cylinders means, V₁ = V₂

The pressure inside each of two identical cylinders is equal to atmospheric pressure means, P₁ = P₂

Both gases are at the same temperature, means T₁ = T₂

$\frac{P_1 V_1}{P_2 V_2} \:=\: \frac{n_1 RT_1}{n_2 RT_2}$

$\frac{P_1 V_1}{P_2 V_2} \:=\: \frac{n_1 T_1}{n_2 T_2}$

n₁ = n₂

So the total amount of hydrogen gas is equal to total amount of ideal nitrogen gas.

Learn more about the ideal gas equation here: brainly.com/question/27870704

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