A sample of nitrogen occupies 5.50 liters under a pressure of 900 torr at 25oC. At what temperature will it occupy 10.0 liters at the same pressure?

The temperature at which the gas will occupy 10 L is 268.8 °C

We'll begin by listing out what was given from the question. This includes:

Initial volume (V₁) = 5.5 L

Initial temperature (T₁) = 25 °C = 25 + 273 = 298 K

Final volume (V₂) = 10 L

Pressure = constant

Using the Charles' law equation, we can obtain the new temperature of the gas as illustrated below:

Cross multiply

5.5 × T₂ = 298 × 10

5.5 × T₂ = 2980

Divide both side by 5.5

T₂ = 541.8

Subtract 273 to express in degree celsius (°C)

T₂ = 541.8 – 273

Therefore, the temperature at which the gas will occupy 10 L is 268.8 °C

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At 268.82°C volume occupied by nitrogen is 10 liters at pressure of 900 torr.

Explanation:

Given:

Volume of a sample of nitrogen = 5.50 liters

Pressure = 900 torr

Temperature = 25°C

To find the temperature at which the nitrogen will occupy 10 liters volume at same pressure.

Solution:

Since the pressure is kept constant, so we can apply the temperature-volume law also called the Charles Law.

Charles Law states that the volume of a gas held at constant pressure is directly proportional to the temperature of the gas in Kelvin.

Thus, we have :

∝

where is a constant.

For two samples of gases, the law can be given as:

From the data given:

We need to find .

Plugging in values in the formula.

Multiplying both sides by .

Multiplying both sides by

Thus, at 268.82°C volume occupied by nitrogen is 10 liters at pressure of 900 torr.

change tension

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explanation:

this statement is false. after falling for 5 seconds, its speed will not be 100 m/s.