Question

An unknown quantity of NH, has a pressure of 102.4 ka, a volume of 45 L, and temperature of 87 °C. How many grams of gas are there?

Answer 1

To find the number of grams of NH3 gas, we first need to calculate the number of moles of gas using the ideal gas law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in L)
n = moles of gas
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)

First, we need to convert the given pressure to atm:
102.4 kPa * (1 atm / 101.3 kPa) = 1.01 atm

Next, we need to convert the given temperature to Kelvin:
87 °C + 273 = 360 K

Now, we can plug in the values into the ideal gas law equation:
(1.01 atm) * (45 L) = n * (0.0821 L.atm/mol.K) * (360 K)

45.45 = 29.242n
n = 1.5562 mol

Now, we can calculate the molar mass of NH3:
N: 1 * 14 g/mol = 14 g/mol
H: 3 * 1 g/mol = 3 g/mol

Molar mass of NH3 = 14 g/mol + 3 g/mol = 17 g/mol

Finally, we can calculate the mass of NH3 gas using the number of moles and molar mass:
mass = moles * molar mass
mass = 1.5562 mol * 17 g/mol = 26.46 g

Therefore, there are approximately 26.46 grams of NH3 gas present.