The pressure of a gaseous mixture of NH3 and N2 decreased from 1.50 kPa to
1.00 kPa after the NH3 was absorbed from the mixture. Assuming ideal gas
behavior, find the composition of the original mixture.
XNH3 = pNH3/total P = 0.5/1.5 = ?
XN2 = pN2/total P = 1.0/1.5 = ?
Without additional information I don't think this can be converted to grams.
To find the composition of the original mixture, we can make use of Dalton's Law of Partial Pressures. According to this law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas.
Let's assume that the partial pressure of NH3 in the original mixture is P(NH3), and the partial pressure of N2 is P(N2). We are given that the total pressure of the mixture decreased from 1.50 kPa to 1.00 kPa after all the NH3 was absorbed.
Using Dalton's Law, we can write the following equation:
P(NH3) + P(N2) = 1.50 kPa (equation 1)
After the NH3 is absorbed, we are left with only the partial pressure of N2, which is 1.00 kPa. Therefore, we can rewrite equation 1 as:
P(N2) = 1.50 kPa - P(NH3) (equation 2)
Substituting the value of P(N2) from equation 2 into equation 1, we get:
P(NH3) + (1.50 kPa - P(NH3)) = 1.00 kPa
Simplifying the equation, we have:
1.50 kPa - P(NH3) + P(NH3) = 1.00 kPa
1.50 kPa = 1.00 kPa + P(NH3)
P(NH3) = 0.50 kPa
Now that we know the partial pressure of NH3 is 0.50 kPa, we can substitute this value back into equation 1 to find the partial pressure of N2:
0.50 kPa + P(N2) = 1.50 kPa
P(N2) = 1.50 kPa - 0.50 kPa
P(N2) = 1.00 kPa
So, the partial pressure of NH3 in the original mixture is 0.50 kPa, and the partial pressure of N2 is 1.00 kPa. Therefore, the composition of the original mixture is 0.50 kPa NH3 and 1.00 kPa N2.