Question

If a 2.01 L sample of hydrogen gas has a pressure of 4081 torr at a temperature of 37°C, what would be its new volume if the temperature increased to 168°C and the pressure increased to 57304 torr?

a. 0.47 L
b. 1.29 L
c. 2.83 L
d. 5.21 L

Answer 1

By applying the combined gas law to the given conditions and solving for the new volume, we find that the new volume of the 2.01 L hydrogen gas sample, when the temperature is increased to 168°C and the pressure to 57304 torr, is approximately 0.47 L.

Step-by-step explanation:

If a 2.01 L sample of hydrogen gas has a pressure of 4081 torr at a temperature of 37°C, you're asking to find its new volume if the temperature increased to 168°C and the pressure increased to 57304 torr. To solve this, we need to use the combined gas law, which is expressed as (P1 * V1) / T1 = (P2 * V2) / T2, where P stands for pressure, V stands for volume, and T stands for temperature in Kelvin. Converting temperatures to Kelvin, we have 310.15 K (37°C) and 441.15 K (168°C). Now, we can rearrange the formula to solve for the new volume (V2).

First, convert the pressures to atmospheres so they cancel out with the units (1 atm = 760 torr). We then plug in the known values: (4081 torr / 760 torr/atm) * 2.01 L / 310.15 K = (57304 torr / 760 torr/atm) * V2 / 441.15 K.
After converting, simplifying, and solving for V2, we find that the new volume is approximately 0.47 L.