An aqueous solution of ammonium nitrite decomposes when heated to give off nitogen gas and water. This reaction can be used to prepare pure nitrogen gas. How many grams of ammonium nitrite must have reacted if 3.75 liters of nitrogen gas was colleced over water at 25˚C and 97.8 kPa? I keep getting 11.8 but its saying im wrong.whats the correct steps to solve it
If you will show your work I will find the error.
Steps?
1. Write and balance the equation.
2. Find pressure H2O @ 25C and calculate pressure dry N2.
3. Find mols N2
4. Use the equation to convert mols N2 to mols NH4NO3.
I just re-read the problem. Are you using NH4NO3 or NH4NO2?
To solve this problem, you need to use the Ideal Gas Law equation, PV = nRT, where:
- P is the pressure of the gas
- V is the volume of the gas
- n is the number of moles of the gas
- R is the ideal gas constant (0.0821 L·atm/mol·K)
- T is the temperature in Kelvin
First, let's convert the temperature from Celsius to Kelvin by adding 273.15:
25°C + 273.15 = 298.15 K
Next, convert the volume of the gas from liters to moles using the Ideal Gas Law equation:
PV = nRT
n = PV / RT
Plug in the given values:
P = 97.8 kPa
V = 3.75 L
R = 0.0821 L·atm/mol·K
T = 298.15 K
Convert pressure to atm:
97.8 kPa * (1 atm / 101.325 kPa) = 0.964 atm
Now, plug these values into the equation to find the number of moles, n:
n = (0.964 atm * 3.75 L) / (0.0821 L·atm/mol·K * 298.15 K)
Calculating the above expression will give the moles of nitrogen gas generated from the decomposition of ammonium nitrite.
Next, we need to determine the stoichiometry of the reaction between ammonium nitrite and nitrogen gas. The balanced equation is:
NH4NO2(s) -> N2(g) + 2H2O(g)
According to the equation, 1 mole of ammonium nitrite produces 1 mole of nitrogen gas. Therefore, the moles of ammonium nitrite used in the reaction will be equal to the moles of nitrogen gas produced.
Now, you need to calculate the molar mass of ammonium nitrite (NH4NO2). The molar mass can be calculated by adding the atomic masses of each element in the formula:
Molar mass of NH4NO2 = (1 * atomic mass of N) + (4 * atomic mass of H) + atomic mass of O + (2 * atomic mass of O)
Once you have the molar mass of NH4NO2, you can calculate the number of grams of ammonium nitrite by multiplying the moles of ammonium nitrite by its molar mass.
So, the correct steps to solve the problem are:
1. Convert the temperature to Kelvin.
2. Convert the pressure to atm.
3. Use the Ideal Gas Law equation, PV = nRT, to find the moles of nitrogen gas produced.
4. Determine the stoichiometry of the reaction to find the moles of ammonium nitrite.
5. Calculate the molar mass of ammonium nitrite.
6. Multiply the moles of ammonium nitrite by its molar mass to find the number of grams.