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2. A 2.5 mol SAMPLE OF OXYGEN GAS (O2) INCREASES TO 3.2 mol
FROM AN INITIAL PRESSURE OF 720 mmHg. THE VOLUME
CHANGES FROM 34 L TO 45 L, AND THE TEMPERATURE
INCREASES FROM 25°C TO 45°C, WHAT IS THE FINAL PRESSURE
OF THIS GAS?

Respuesta :

696.32 mmHg is the final pressure of the gas.

What is an ideal gas equation?

The ideal gas equation, pV = nRT, is an equation used to calculate either the pressure, volume, temperature or number of moles of a gas.

Given data:

[tex]P_1[/tex] = 720 mmHg              

[tex]P_2[/tex] = ?

[tex]n_1[/tex] = 2.5 mol                

[tex]n_2[/tex] = 3.2 mol

[tex]V_1[/tex] = 34 L            

[tex]V_2[/tex] = 45 L

Formula

Combined gas law

[tex]\frac{P_1 V_1}{n_1} = \frac{P_2 V_2}{n_2}[/tex]

[tex]P_2[/tex] = 696.32 mmHg

Hence, 696.32 mmHg is the final pressure of the gas.

Learn more about an ideal gas equation here:

https://brainly.com/question/19251972

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