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PLEASE ANSWER ITS URGENT 40 POINTS!!!

A gas exerts a pressure of 2.15 atm in a 0.0900 l container. What is the new pressure when the gas is transferred to a container with a volume of 4.75 L?
P = atm
Assume that the number of moles and the temperature remain constant

1 Answer

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Step-by-step explanation:

We can use the combined gas law to solve this problem, which states:

(P1 * V1) / T1 = (P2 * V2) / T2

Where:

P1 and V1 are the initial pressure and volume

T1 is the initial temperature

P2 and V2 are the final pressure and volume

T2 is the final temperature

In this case, we can assume that the temperature remains constant, so T1 = T2. We also know the initial pressure and volume (P1 = 2.15 atm and V1 = 0.0900 L), and we want to find the final pressure (P2) when the gas is transferred to a new container with a volume of 4.75 L (V2 = 4.75 L).

Plugging in these values, we get:

(2.15 atm * 0.0900 L) / T = (P2 * 4.75 L) / T

Simplifying this equation by canceling out the T's and solving for P2, we get:

P2 = (2.15 atm * 0.0900 L) / 4.75 L

P2 = 0.0406 atm

Therefore, the new pressure is 0.0406 atm when the gas is transferred to a container with a volume of 4.75 L. This makes sense because the pressure decreases as the volume increases, assuming the temperature remains constant.

User Stanley Stuart
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