Question

At 0°C and 0.500 atm, 4.48 LNH₃(g) contains ________.

1) 0.20 mol NH₃
2) 3.40 g
3) 6.02×1022 molecules
4) 0.40 mol NH₃

Answer 1

To find the volume of a sample of ammonia at 0 °C and 1.00 atm, we can use the ideal gas law equation PV = nRT. Given the initial volume, temperature, and pressure, we can rearrange the equation to solve for the final volume. By substituting the given values into the equation, we find that the final volume is 0.188 L.

Step-by-step explanation:

To find the volume of a sample of ammonia at 0 °C and 1.00 atm, we can use the ideal gas law equation: PV = nRT. R represents the ideal gas constant, which is 0.0821 L·atm/(mol·K). We are given the initial volume (V1 = 0.250 L), temperature (T1 = 27 °C = 300 K), and pressure (P1 = 0.850 atm).

We want to find the final volume (V2) at 0 °C and 1.00 atm, so the final temperature (T2 = 0 °C = 273 K) and pressure (P2 = 1.00 atm) are known. Rearranging the equation, we can solve for V2: V2 = (nRT2) / P2.

First, we need to calculate the number of moles (n) of ammonia in the initial sample using the ideal gas law equation: PV = nRT. Rearranging the equation, we can solve for n: n = PV / RT. Substituting the given values, n = (0.850 atm)(0.250 L) / (0.0821 L·atm/(mol·K))(300 K) = 0.00886 mol NH₃.

Finally, we can calculate the final volume (V2) using the equation: V2 = (nRT2) / P2. Substituting the values we know, V2 = (0.00886 mol)(0.0821 L·atm/(mol·K))(273 K) / (1.00 atm) = 0.188 L.