Question

At 10°C, the gas in a cylinder has a volume of 0.250 L. The gas is allowed to expand to 0.285 L.

What must the final temperature be for the pressure to remain constant? (Hint °C + 273 = K.)


248 K


284 K


323 K


282 K

Answer 1

are you sure

Answer 2

To solve this problem, we can use the ideal gas law, which states:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature

Since the pressure is constant, we can simplify the equation to:

V1/T1 = V2/T2

Where:
V1 = initial volume
T1 = initial temperature
V2 = final volume
T2 = final temperature

Plugging in the given values:

V1 = 0.250 L
T1 = 10°C + 273 = 283 K
V2 = 0.285 L

Now we can solve for T2:

0.250/283 = 0.285/T2

Cross-multiplying, we get:

0.250T2 = 0.285 * 283

0.250T2 = 80.955

T2 = 80.955/0.250

T2 ≈ 323.82

Rounding to the nearest whole number, the final temperature must be approximately 323 K.

Therefore, the correct answer is 323 K.

Answer 3

Apologies for the confusion in my previous response. Let's solve the problem correctly.

By using the formula V1/T1 = V2/T2 and plugging in the given values:

V1 = 0.250 L
T1 = 10°C + 273 = 283 K
V2 = 0.285 L

We have:

0.250/283 = 0.285/T2

Cross-multiplying, we get:

0.250T2 = 0.285 * 283

0.250T2 = 80.655

Finally, solving for T2:

T2 = 80.655/0.250

T2 ≈ 322.62

Rounding to the nearest whole number, the final temperature must be approximately 323 K.

Therefore, the correct answer is 323 K.