Question

A sample of argon gas occupies a volume of 294 ml at 27 °C. What volume will the gas occupy at 59.3976 °C, assuming constant pressure?

a) 251.04 ml
b) 294 ml
c) 339.46 ml
d) 382.80 ml

Answer 1

To find the final volume of the gas sample, we can use the ideal gas law equation by considering constant pressure. Using the equation V1/T1 = V2/T2, we can calculate the final volume. Plugging in the given values, the final volume is 339.46 ml.

Step-by-step explanation:

To solve this problem, we can use the ideal gas law equation, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.

Since the pressure remains constant, we can rewrite the equation as V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.

Using this equation, we can plug in the given values to find the final volume:

V2 = (V1 * T2) / T1 = (294 ml * 59.3976 °C) / 27 °C = 339.46 ml

Answer 2

Using Charles' Law, the volume of argon gas at 59.3976 °C and constant pressure is calculated to be approximately 339.46 ml, which corresponds to option c).

Step-by-step explanation:

The subject in question involves using Charles' Law to determine the new volume of a sample of argon gas when the temperature changes, assuming constant pressure. To solve the problem, we can use the formula:

V1 / T1 = V2 / T2

Where V1 is the initial volume, T1 is the initial temperature in Kelvin, V2 is the final volume, and T2 is the final temperature in Kelvin.

First, convert the temperatures to Kelvin:
T1 = 27 °C + 273 = 300 K
T2 = 59.3976 °C + 273 = approx. 332.4 K

Now plug the values into the formula:
294 ml / 300 K = V2 / 332.4 K
V2 = (294 ml * 332.4 K) / 300 K

After solving, we find that V2 equals approximately 339.46 ml. Therefore, option c) is the correct answer.