Question

1.77 moles of Neon has a pressure of 936.0 mmHg at 57.0 C. What is the volume of the Neon gas? (only use numbers, and round to the hundredths place)

Answer 1

To find the volume of 1.77 moles of Neon gas at 936.0 mmHg and 57.0 ℃, the ideal gas law is used, converting units to atmospheres and Kelvin, resulting in a volume of 39.46 L.

Step-by-step explanation:

To calculate the volume of 1.77 moles of Neon gas at a pressure of 936.0 mmHg and a temperature of 57.0 ℃, we will use the Ideal Gas Law, which is represented by the formula PV = nRT. Here, P represents the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles of gas, R is the Ideal Gas Constant (0.0821 L·atm/(mol·K)), and T is the absolute temperature in Kelvin (K).

First, convert the temperature to Kelvin: T = 57.0 ℃ + 273.15 = 330.15 K

Next, convert the pressure to atmospheres: P = 936.0 mmHg * (1 atm / 760 mmHg) = 1.2316 atm

Now, we can solve for V:

V = (nRT) / P = (1.77 mol * 0.0821 L·atm/(mol·K) * 330.15 K) / 1.2316 atm

V = 39.46 L

Therefore, the volume of the Neon gas is 39.46 L, when rounded to the hundredths place.