If a sample of gas occupies 25.0 mL at -25°C and 650 mmHg, what is the volume at 25°C and 353 mmHg?
(Could you please show me step by step?)
This is (P1V1/T1) = (P2V2/T2)
The must be in kelvin. What else is there to show? Substitute the numbers form the problem and solve for the only unknown.
So (650)(25)/248=353(x)/298
65.5241=.8441/(x)
55.3=x
got it right thanks Dr.Bob
To solve this problem, we can use the combined gas law equation:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
We are given:
P1 = 650 mmHg (initial pressure)
V1 = 25.0 mL (initial volume)
T1 = -25°C (initial temperature)
We need to find:
V2 (final volume)
P2 = 353 mmHg (final pressure)
T2 = 25°C (final temperature)
Step 1: Convert temperatures to Kelvin
To convert from Celsius to Kelvin, we add 273.15 to the Celsius temperature.
T1 = -25°C + 273.15 = 248.15 K
T2 = 25°C + 273.15 = 298.15 K
Step 2: Plug in the values into the equation
(P1 * V1) / T1 = (P2 * V2) / T2
(650 mmHg * 25.0 mL) / 248.15 K = (353 mmHg * V2) / 298.15 K
Step 3: Solve for V2
Cross-multiply the equation to solve for V2:
(650 mmHg * 25.0 mL * 298.15 K) = (353 mmHg * V2 * 248.15 K)
V2 = (650 mmHg * 25.0 mL * 298.15 K) / (353 mmHg * 248.15 K)
Step 4: Calculate the final volume
V2 = (4914375) / (87431495) ≈ 0.056 mL
The final volume is approximately 0.056 mL.