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3 years ago

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Two steel containers of equal volume contain two different gases at the same temperature. the first container holds 1.3 moles of

n^2 gas and the second contains 1.3 moles of so^3 gas. compare the pressures of the two containers

1 answer:

ki77a [65]3 years ago

8 0

<span>Both of the containers have exactly the same pressure.</span>

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The diagram below shows a gas sample being measured with an open-end mercury (Hg) manometer. If a barometer reads 730. 1 torr, w

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The pressure of the gas in the flask (in atm) when Δh = 5.89 cm is 1.04 atm

<h3>Data obtained from the question</h3>

The following data were obtained from the question:

Atmospheric pressure (Pa) = 730.1 torr = 730.1 mmHg
Change in height (Δh) = 5.89 cm
Pressure due to Δh (PΔh) = 5.89 cmHg = 5.89 × 10 = 58.9 mmHg
Pressure of gas (P) =?

<h3>How to determine the pressure of the gas</h3>

The pressure of the gas can be obtained as illustrated below:

P = Pa + PΔh

P = 730.1 + 58.9

P = 789 mmHg

Divide by 760 to express in atm

P = 789 / 760

P = 1.04 atm

Thus, the pressure of the gas when Δh = 5.89 cm is 1.04 atm

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