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.
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
3 answers
are you sure
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.
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.
2 answers