a sample of nitrogen gas has a volume of 1.00 l at STP What is the temp in Celsius if the volume is 10.0 L at 2.00 atm
* I know to use the combined gas law, and I got the question wrong in my homework assignment, reviewing for a test today please help.
(P1V1/T1) = (P2V2/T2) which I've rearranged to
(P1V1T2) + (P2V2T1)
P1 = 1 atm
V1 = 1L
T1 = 273K
P2 = 2.00 atm
V2 = 10.0L
T2 = ?
(1*1*T2) = (2.00*10.0*273) = about 5460K
Another thought. Did you remember to use T in Kelvin?
Last thought. Did you remember to convert 5460 K back to C (the problems asks for C). That will be 5460-273 = 5187. Check my work.
To solve this problem, you can use the combined gas law formula:
(P₁ * V₁) / (T₁) = (P₂ * V₂) / (T₂)
Where:
P₁ = initial pressure (1 atm at STP)
V₁ = initial volume (1.00 L)
T₁ = initial temperature (in Kelvin at STP)
P₂ = final pressure (2.00 atm)
V₂ = final volume (10.0 L)
T₂ = final temperature (in Kelvin, what we need to find)
First, convert the given values to Kelvin:
T₁ = 273.15 K (since it is at STP)
P₂ = 2.00 atm
V₂ = 10.0 L
Now we can solve for T₂ by rearranging the equation:
T₂ = (P₂ * V₂ * T₁) / (P₁ * V₁)
Substituting the known values:
T₂ = (2.00 atm * 10.0 L * 273.15 K) / (1 atm * 1.00 L)
T₂ = 5463 K
Finally, convert the temperature from Kelvin to Celsius:
T₂ in Celsius = T₂ in Kelvin - 273.15
T₂ in Celsius = 5463 K - 273.15 K
T₂ in Celsius ≈ 5189.85 °C (rounded to two decimal places)
Therefore, the temperature in Celsius is approximately 5189.85 °C.
To determine the change in temperature using the combined gas law, you need to use the formula:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
where P1, V1, and T1 represent the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 represent the final pressure, volume, and temperature.
In this case, you want to find the final temperature (T2) when the initial volume (V1) is 1.00 L, and the final volume (V2) is 10.0 L at a pressure of 2.00 atm.
Since the problem states that the conditions are at STP, we know that the initial temperature (T1) is 0°C or 273.15 K. We can substitute these values into the combined gas law equation:
(P1 * V1) / T1 = (P2 * V2) / T2
Plugging in the given values:
(1.00 atm * 1.00 L) / 273.15 K = (2.00 atm * 10.0 L) / T2
Simplifying this equation:
1.00 / 273.15 = 20.00 / T2
Cross-multiplying and solving for T2:
T2 = (20.00 * 273.15) / 1.00
T2 ≈ 5463.00 K
To convert this temperature back to Celsius, subtract 273.15:
T2 ≈ 5463.00 K - 273.15 = 5189.85°C
Therefore, the temperature in Celsius when the volume is 10.0 L at 2.00 atm is approximately 5189.85°C.