Question

The pressure of 1.35 moles of gas in a container was 580.0 torr. The total pressure of the container was 945 torrents. Is there another gas in the container? Why?

o Yes. This is the correct pressure for this molar amount of gas.
o Yes. This is not the correct pressure for this molar amount of gas.
o yes. There is less pressure recorded in the container than the total pressure.
o No. This is the correct pressure for this molar amount of gas.
oNo. This is not the correct pressure for this molar amount of gas.
o No. The values should not be

Answer 1

Answer:

o Yes. This is the correct pressure for this molar amount of gas.

Answer 2

Answer:

Yes, there is another gas present in the container because total pressure is not equal to individual pressure of the gas.

Concept:

Dalton's law of Partial Pressure: This law states that the total pressure exerted by a mixture of gases is equal to the sum of partial pressures exerted by individual gases.

$P_{total} = P_1 + P_2 + P_3 + --------$

where $P_{total}$ = Total pressure exerted by the mixture of gases.

$P_1, P_2, P_3 ----$ = Individual partial pressure of gases

Answer and explanation:

Given that,

Pressure of a gas in a container, P₁ = 580 torr

Total pressure, $P_{total}$ = 945 torr

Number of moles of first gas, n₁ = 1.35 moles

Now, according to Dalton's law of partial pressure,

$P_1 \ should \ be \ equal \ to\ P_{total}$ but they are not equal and this means that there is some another gas also present in the container.

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