A gas at 61°C occupies a volume of 0.67 L. At what Celsius temperature will the volume increase to 1.12 L?
whats the answer didn't understand
Use Charles' Law:
(V1/T1) = (V2/T2)
Make sure to convert your temperatures from Celsius to Kelvin. (°C + 273)
(.67/61 +273) = (1.12/T2) Then go back from Kelvin to Celsius for your final answer.
To find the Celsius temperature at which the volume of the gas increases to 1.12 L, we can use the combined gas law, which relates the initial and final conditions of temperature, volume, and pressure.
The combined gas law equation is:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 and P2 are the initial and final pressures, which we can assume to be constant.
V1 and V2 are the initial and final volumes.
T1 and T2 are the initial and final temperatures.
We are given:
T1 = 61°C
V1 = 0.67 L
V2 = 1.12 L
To find T2, we need to rearrange the combined gas law equation to solve for T2:
T2 = (P2 * V2 * T1) / (P1 * V1)
Since the problem does not provide pressure values and it is assumed to be constant, we can cancel out the pressure terms from the equation. This leaves us with:
T2 = (V2 * T1) / (V1)
Substituting the given values:
T2 = (1.12 L * 61°C) / (0.67 L)
Now, we can calculate the value of T2:
T2 = 101.492°F
Therefore, at a Celsius temperature of approximately 101.492, the volume of the gas will increase to 1.12 L.