Question

11) If I have 2.75 moles of gas at a

temperature of 175 K and a pressure of 177.3
mmHg, what is the volume of the gas?

Answer 1

The volume of the gas is approximately 19.4 liters.

Step-by-step explanation:

We can use the Ideal Gas Law to solve for the volume of the gas:

`PV = nRT`

Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

First, we need to convert the temperature to Kelvin by adding 273.15:

`175 K + 273.15 = 448.15 K`

Next, we can plug in the values and solve for V:

`V = (nRT) / P`

`V = (2.75 mol * 0.0821 Latm/molK * 448.15 K) / (177.3 mmHg / 760 mmHg/atm)`

V ≈ 19.4 L

Answer 2

We can use the Ideal Gas Law to solve for the volume of the gas:

PV = nRT

where:
P = pressure = 177.3 mmHg
V = volume (unknown)
n = moles = 2.75 mol
R = gas constant = 0.08206 L·atm/mol·K
T = temperature = 175 K

Substituting the values:

V = nRT/P
V = (2.75 mol)(0.08206 L·atm/mol·K)(175 K)/(177.3 mmHg)
V = 5.33 L (rounded to two decimal places)

Therefore, the volume of the gas is approximately 5.33 L.