A gas sample has an initial volume of 4.5 liters at a pressure of 731 mmHg. If the volume is increased to 8.9 liters, what is the pressure?
p1v1 = p2v2
What is the volume occupied by 12.3 g or argon gas at a pressure of 1.17 atm and a temperature of 455K?
Use PV = nRT.
n = grams/molar mass
That is the ideal gas law
Pv=nRT
Use the Given/the known and you will get the answer
Given:
known RPT 0.08206 atm x L/mol x K
To solve this problem, you can use Boyle's Law, which states that the pressure and volume of a given amount of gas are inversely proportional at constant temperature. Mathematically, Boyle's Law can be expressed as:
P1V1 = P2V2
Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
In this case, the initial volume (V1) is 4.5 liters, the initial pressure (P1) is 731 mmHg, and the final volume (V2) is 8.9 liters. We want to find the final pressure (P2).
Using the formula, we can rearrange it to solve for P2:
P2 = (P1 * V1) / V2
Let's substitute in the given values:
P2 = (731 mmHg * 4.5 liters) / 8.9 liters
Now, we can calculate the final pressure (P2) by dividing the product of the initial pressure and volume by the final volume:
P2 = 3260.5 mmHg / 8.9 liters
After performing the division, you will get the final pressure (P2) in units of mmHg.