A sample of oxygen gas is at a temperature of 340k and occupies a volume of 1.2cm3. What temperature will the sample of gas be at the volume is decreased to 200cm3?
assuming the pressure remains the same,
V1/T1 = V2/T2
not sure how going from 1.2 cm^3 to 200 cm^3 is a decrease, though ...
To solve this problem, we can use the combined gas law, which states that the ratio of initial temperature to final temperature is equal to the ratio of initial volume to final volume, when the pressure and amount of gas are constant.
Let's assign the following values to the variables:
Initial temperature (T1) = 340 K
Initial volume (V1) = 1.2 cm^3
Final volume (V2) = 200 cm^3
Final temperature (T2) = ?
Using the combined gas law formula:
(P1 * V1) / T1 = (P2 * V2) / T2
Since the problem doesn't provide any information about pressure, we can assume it is constant, so we can eliminate it from the equation.
Simplifying the equation:
(V1 / T1) = (V2 / T2)
Rearranging the equation to solve for T2:
T2 = (V2 * T1) / V1
Plugging in the given values:
T2 = (200 cm^3 * 340 K) / 1.2 cm^3
Calculating the result:
T2 = 56666.67 K
Therefore, the temperature of the sample of gas will be 56666.67 K when the volume is decreased to 200 cm^3.
To solve this problem, you can use the combined gas law equation, which relates the initial and final conditions of temperature and volume for a given amount of gas.
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 are constant as the question only mentions temperature and volume),
V1 and V2 are the initial and final volumes,
T1 and T2 are the initial and final temperatures.
In this case, we are given:
T1 = 340 K (initial temperature)
V1 = 1.2 cm³ (initial volume)
V2 = 200 cm³ (final volume)
We need to find T2, the final temperature.
Rearranging the formula, we get:
T2 = (P2 * V2 * T1) / (P1 * V1)
As mentioned before, since the problem does not provide pressure information, we can assume the pressure is constant. Therefore, the pressure terms cancel out:
T2 = (V2 * T1) / V1
Now we can substitute the given values into the equation:
T2 = (200 cm³ * 340 K) / 1.2 cm³
Simplifying further:
T2 = (200 * 340) / 1.2
T2 = 56666.67 K
Therefore, when the volume decreases to 200 cm³, the temperature of the sample of oxygen gas will be approximately 56666.67 K.