Question

A sample of gas in a flexible container starts at a temp of 30 degrees c l, 1.5atm and 2.0ml. If the temp decreases to 25 degrees c and the pressure increases to 2.0 atm, what will the new volume be?

Answer 1

1.475ml

Step-by-step explanation:

We add 273 to °C to convert it to kelvin

Answer 2

To solve this problem, we can use the combined gas law, which states:

(P1 * V1) / (T1) = (P2 * V2) / (T2)

Where:
P1 and P2 are the initial and final pressures,
V1 and V2 are the initial and final volumes,
T1 and T2 are the initial and final temperatures.

Given:
P1 = 1.5 atm
V1 = 2.0 mL
T1 = 30 °C = 273.15 + 30 = 303.15 K
T2 = 25 °C = 273.15 + 25 = 298.15 K
P2 = 2.0 atm

Let's substitute these values into the combined gas law equation and solve for V2:

(1.5 * 2.0) / 303.15 = (2.0 * V2) / 298.15

3.0 / 303.15 = (2.0 * V2) / 298.15

0.0099 = (2.0 * V2) / 298.15

Cross-multiplying:

2.0 * V2 = 0.0099 * 298.15

2.0 * V2 = 2.948485

V2 = 2.948485 / 2.0

V2 = 1.4742425 mL

Therefore, the new volume will be approximately 1.47 mL when the temperature decreases to 25 degrees Celsius and the pressure increases to 2.0 atm.