Question

ammonia gas has a molar mass approximately 17 g per mile at 290 K and 1.2 atm a sample of ammonia has a volume of 3.7 L in 3 to 5 sentences explain how you can find the mass of the ammonia then given R equals 0.0821 L times atmosphere divided by moles times Kelvin calculate the mass

Answer 1

To find the mass of ammonia gas in the given sample, you can first use the Ideal Gas Law, which is formulated as PV = nRT. Rearranging this equation allows you to solve for the number of moles (n):

\[ n = \frac{PV}{RT}. \]

Using the provided values (P = 1.2 atm, V = 3.7 L, R = 0.0821 L·atm/(mol·K), and T = 290 K), you can calculate the number of moles of ammonia. Once you have the number of moles, multiply it by the molar mass of ammonia (approximately 17 g/mol) to find the mass.

Now, let's calculate the number of moles:

\[
n = \frac{(1.2 \, \text{atm}) \times (3.7 \, \text{L})}{(0.0821 \, \text{L·atm/(mol·K)}) \times (290 \, \text{K})}
\]

Calculating the denominator:

\[
0.0821 \times 290 \approx 23.877.
\]

Now, substituting back into the equation for n:

\[
n \approx \frac{(1.2 \times 3.7)}{23.877} \approx \frac{4.44}{23.877} \approx 0.186.
\]

Now, to find the mass:

\[
\text{mass} = n \times \text{molar mass} = 0.186 \, \text{mol} \times 17 \, g/mol \approx 3.162 \, g.
\]

Thus, the mass of the ammonia gas sample is approximately 3.16 g.