Answer:
165°C
Explanation:
We can use here the combined gas law, relating the temperature, pressure, and volume of a gas with a constant quantity:
P₁V₁
T₁
P2V2
T2
If you're using the ideal-gas equation, which we're NOT using here, you would have to convert each measurement into the appropriate units (L, K, atm, and mol). The only measurement that needs conversion here is temperature, from °C to K. (You will always convert temperature to Kelvin (absolute temperature) when using gas equations).
The Kelvin temperature is
K= 20°C + 273 = 293K
Let's rearrange the combined gas law to solve for the final temperature, T2:
T2
P2V2T1
P₁V₁
Plugging in known values, we can find the final temperature:
T2
(56.7kPa) (8.00L) (293K) (86.7kPa) (3.50L) 438K
Lastly, we'll convert back from K to °C:
438K 273 = 165°C
