A sample of argon gas occupies a volume of 950 mL at 25.0C. What volume will the gas occupy at 50.0C if the pressure remains constant?

V1/T1 = V2/T2. Don't forget to convert celsius to Kelvin.

To find the volume of the argon gas at 50.0C if the pressure remains constant, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature when pressure is constant.

The formula for Charles's Law is:

V1 / T1 = V2 / T2

Where:
V1 = initial volume
V2 = final volume
T1 = initial temperature
T2 = final temperature

Given:
V1 = 950 mL (convert to liters by dividing by 1000: 0.950 L)
T1 = 25.0C (convert to Kelvin by adding 273.15: 298.15 K)
T2 = 50.0C (convert to Kelvin: 323.15 K)

Using the formula:

V1 / T1 = V2 / T2

(0.950 L) / (298.15 K) = V2 / (323.15 K)

Solving for V2:

V2 = (0.950 L) * (323.15 K) / (298.15 K)

V2 ≈ 1.03 L

Therefore, the volume of the argon gas at 50.0C, if the pressure remains constant, will be approximately 1.03 L.

To solve this question, we can use the combined gas law equation, which is derived from Boyle's law, Charles's law, and Gay-Lussac's law. The equation is as follows:

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

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

In this case, we are given:
V1 = 950 mL
T1 = 25.0°C = 25.0 + 273.15 K = 298.15 K
T2 = 50.0°C = 50.0 + 273.15 K = 323.15 K
P1 and P2 remain constant.

Let's plug in the values into the equation:

(P1 * 950 mL) / (298.15 K) = (P2 * V2) / (323.15 K)

Since the pressure remains constant, we can simplify further:

950 mL / 298.15 K = V2 / 323.15 K

To find V2, we can cross multiply and solve for V2:

V2 = (950 mL * 323.15 K) / 298.15 K

V2 ≈ 1031.65 mL

Therefore, the volume of the argon gas at 50.0°C will be approximately 1031.65 mL if the pressure remains constant.