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!
(V1/T1) = (V2/T2)
(0.182/T) = (2.34/314)
Solve for T. I found about 24.
I think I figures out what you're doing and it isn't the way to solve these problems. You're dividing 2.34/314 = 0.00745 then multiplying by 0.185 to obtain 0.00136. There's nothing wrong with 2.34/314 = 0.00745 so you rewrite the equation as (0.185/T) = 0.00745. From there, however, it is T = (0.185/0.00745) = about 24.
P1V1 = P2V2
668*368 = P2*260
P2 = about 945 torr
I expect you are not punching the right keys at the right time. You can go through it step by step if you wish and I can show you where you're going wrong.
To solve both of these problems, you correctly identified the appropriate equations to use. However, it seems like there might have been errors in the calculations or conversions. Let's go through each problem step by step and double-check the calculations.
1. Variable volume container of helium gas:
Given:
- Initial volume (V1) = 2.34 L
- Initial temperature (T1) = 314 K
- Final volume (V2) = 0.182 L
Using the equation V1/T1 = V2/T2, we can rearrange it to solve for T2:
T2 = (V2 * T1) / V1
Plugging in the values:
T2 = (0.182 L * 314 K) / 2.34 L
T2 ≈ 24.28 K
So, the helium gas must be cooled to approximately 24.28 K to obtain a final volume of 0.182 L.
2. Fixed volume and pressure of nitrogen gas:
Given:
- Initial volume (V1) = 368 mL = 0.368 L
- Initial pressure (P1) = 668 torr
- Final volume (V2) = 260 mL = 0.26 L
Using the equation P1V1 = P2V2, we can rearrange it to solve for P2:
P2 = (P1 * V1) / V2
Plugging in the values:
P2 = (668 torr * 0.368 L) / 0.26 L
P2 ≈ 943.38 torr
So, the final pressure of the nitrogen gas would be approximately 943.38 torr when the final volume is 260 mL.
I hope this helps! Let me know if you have any further questions.
To answer both of these questions, you need to use the ideal gas law equation, which states that the product of pressure (P) and volume (V) is directly proportional to the number of moles (n) and the temperature (T) of a gas, mathematically represented as PV = nRT. In these specific cases, the number of moles and the pressure are fixed, so we can re-write the equation as V/T = constant.
For the first question, where the initial volume and temperature are given as V1 = 2.34 L and T1 = 314 K, and the final volume is V2 = 0.182 L, we can substitute these values into the equation as follows:
(V1/T1) = (V2/T2)
(2.34/314) = (0.182/T2)
Cross multiplying gives: 2.34T2 = 0.182 * 314
Now you can solve for T2 by dividing both sides of the equation by 2.34: T2 = (0.182 * 314) / 2.34
Calculating this gives T2 ≈ 24.4 K.
For the second question, where the initial volume and pressure are given as V1 = 368 mL and P1 = 668 torr, and the final volume is V2 = 260 mL, we can use the same equation as before:
(P1V1) = (P2V2)
(668 * 368) = (P2 * 260)
Now you can solve for P2 by dividing both sides of the equation by 260: P2 = (668 * 368) / 260
Calculating this gives P2 ≈ 947.2 torr.
Make sure that you have correctly inputted the given values into the equations and followed the correct order of operations in your calculations.