What is the volume occupied by 20.2g NH3(g) at -25 degrees celsius and 752 mmHg?
This is Ideal Gas Law.
To find the volume occupied by a gas, we can use the Ideal Gas Law, which is represented by the equation:
PV = nRT
Where:
P = pressure of the gas
V = volume occupied by the gas
n = number of moles of the gas
R = ideal gas constant
T = temperature of the gas in Kelvin
Let's break down the given information:
- Pressure (P) = 752 mmHg
- Temperature (T) = -25 degrees Celsius
To use the Ideal Gas Law, we need to convert the temperature to Kelvin. We can do this by adding 273.15 to the Celsius temperature:
T(K) = T(°C) + 273.15
So, T(K) = -25 + 273.15 = 248.15 K
Now, we need to calculate the number of moles (n) of NH3(g). We can use the molar mass of NH3 to convert the given mass to moles:
Molar mass of NH3(g) = 17.03 g/mol
n = mass / molar mass
n = 20.2 g / 17.03 g/mol ≈ 1.186 mol
Now that we have all the variables, we can rearrange the Ideal Gas Law equation to solve for volume (V):
V = (nRT) / P
Let's substitute the values into the equation:
V = (1.186 mol * 0.0821 L/mol·K * 248.15 K) / 752 mmHg
Note: The ideal gas constant, R, has a value of 0.0821 L/mol·K.
Now we can calculate the volume. To do this, we need to convert mmHg to atmospheres (atm) because the units for R are in atm·L/mol·K:
1 atm = 760 mmHg
V = (1.186 mol * 0.0821 L/mol·K * 248.15 K) / (752 mmHg / 760 mmHg/atm)
V ≈ 0.091 L or 91 mL
Therefore, the volume occupied by 20.2 g of NH3(g) at -25 degrees Celsius and 752 mmHg is approximately 0.091 L or 91 mL.