To what temperature in K must a variable volume container of helium gas be cooled to obtain a final volume of 0.182 L? The initial volume and temperature are 2.34 L and 314 K, respectively. The pressure and number of moles are fixed.
You're supposed to us V1/T1=V2/T2, and I did that and got .001356, which isn't right. Can someone help please?
At a fixed temperature and number of moles of nitrogen gas, its volume and pressure are 368 mL and 668 torr, respectively. What is the final pressure in torr, if the final volume is 260 mL?
This is P1V1=P2V2. I got 1.244, which is also wrong. Why?
Thanks in advance!
Let's solve each problem step-by-step.
1. For the first problem, we can use the equation V1/T1 = V2/T2 to find the final temperature. We have the following values:
Initial volume, V1 = 2.34 L
Initial temperature, T1 = 314 K
Final volume, V2 = 0.182 L
Let's plug these values into the equation and solve for the final temperature, T2:
V1/T1 = V2/T2
2.34/314 = 0.182/T2
Now, we can cross multiply and solve for T2:
2.34 * T2 = 314 * 0.182
T2 = (314 * 0.182) / 2.34
Calculating this expression gives T2 = 24.425 K.
Therefore, the helium gas must be cooled to 24.425 K to obtain a final volume of 0.182 L.
2. For the second problem, we can use the equation P1V1 = P2V2 to find the final pressure. We have the following values:
Initial volume, V1 = 368 mL
Final volume, V2 = 260 mL
Initial pressure, P1 = 668 torr
Let's plug these values into the equation and solve for the final pressure, P2:
P1V1 = P2V2
668 * 368 = P2 * 260
Now, we can solve for P2:
P2 = (668 * 368) / 260
Calculating this expression gives P2 = 943.723 torr.
Therefore, the final pressure is approximately 943.723 torr when the final volume is 260 mL.
Please double-check your calculations to make sure you entered the values correctly and performed the calculations accurately. Let me know if you need further assistance!
To solve these problems, you are correct in using the ideal gas laws equations. However, it seems there may be some confusion in the calculations.
Let's start with the first problem:
The equation you should be using is:
V1/T1 = V2/T2
Given:
V1 = 2.34 L
T1 = 314 K
V2 = 0.182 L
We need to find T2, the final temperature in Kelvin.
Rearranging the equation, we get:
T2 = (V2 / V1) * T1
Substituting the given values, we have:
T2 = (0.182 L / 2.34 L) * 314 K
T2 = 24.2 K
Therefore, the helium gas must be cooled to approximately 24.2 K to obtain a final volume of 0.182 L.
Now let's move on to the second problem:
The equation to use here is:
P1 * V1 = P2 * V2
Given:
P1 = 668 torr
V1 = 368 mL
V2 = 260 mL
We need to find P2, the final pressure in torr.
Rearranging the equation, we get:
P2 = (P1 * V1) / V2
Substituting the given values, we have:
P2 = (668 torr * 368 mL) / 260 mL
P2 = 944 torr
Therefore, the final pressure in the container would be 944 torr if the final volume is 260 mL.
It's important to double-check your calculations and ensure that you are accurately substituting the values into the equations. Also, pay attention to unit conversions if needed. These steps should help you arrive at the correct answers to the problems.