I understand that you've already made good progress on this problem. Let's continue with finding the answers to part B and C.
To determine the total pressure of the products in the collecting flask after the reaction, we can use the ideal gas law equation: PV = nRT.
In this case, we have the volume (V) of the flask, which is 15.0 L, the temperature (T) of the products, which is 25°C or 298.15 K, and we need to find the pressure (P). We also need the number of moles (n) for both ammonia (NH3) and nitrogen monoxide (NO).
For part B, we assume that the reaction goes to completion, which means all of the nitrogen reacts with steam to form ammonia and nitrogen monoxide. Therefore, the moles of NH3 and NO produced will be the same as the moles of nitrogen that reacted.
To find the moles of nitrogen, we need to use the ideal gas law again, rearranged to solve for moles (n):
n = PV / RT
Substituting the given values: P = 1.016 atm, V = 20.0 L, T = 446.15 K, and R = 0.0821 L·atm/(mol·K), we can calculate the moles of nitrogen.
Now that we know the moles of NH3 and NO, we can use the ideal gas law once again to find the total pressure of the products in the flask. Since the flask is evacuated, the pressure is solely due to the products.
Now, let's move on to part C, which asks for the partial pressure of each of the products in the flask.
To find the partial pressure of NH3 and NO, we need to know their mole fractions. The mole fraction of a gas is the ratio of the moles of that gas to the total moles of gas in the flask.
Once we have the mole fractions, we can find the partial pressures using Dalton's law of partial pressures. According to Dalton's law, the total pressure in the flask is the sum of the partial pressures of each gas.
To calculate the partial pressures, we can multiply the mole fractions by the total pressure found in part B.
I hope this explanation helps you with part B and C of the problem. If you have further questions or need more assistance, feel free to ask!