What mass of ammonium nitrate is require to produce 145L of N2O at 2850 torr and 42 degree celcius
Note the correct spelling of celsius.
NH4NO3 --->N2O + 2H2O
Use PV = nRT and solve for n = number mols N2O at the conditions listed.
Use the coefficients in the balanced equation to convert mols N2O from the previous calculation to mols NH4NO3.
Then convert mols NH4NO3 to grams. g = mols x molar mass.
To find the mass of ammonium nitrate required to produce 145L of N2O at 2850 torr and 42 degrees Celsius, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 42 + 273.15
T(K) = 315.15 K
Next, convert the given pressure from torr to atm:
1 atm = 760 torr
P(atm) = P(torr)/760
P(atm) = 2850/760
P(atm) = 3.75 atm
Now we have the pressure, volume, temperature, and constant needed to calculate the number of moles of N2O produced.
PV = nRT
n = PV/RT
n = (3.75 atm) * (145 L) / (0.0821 L.atm/mol.K * 315.15 K)
Calculating n, we get:
n = 16.0825 moles
The balanced chemical equation for the decomposition of ammonium nitrate is:
NH4NO3 (s) -> N2O(g) + 2H2O(g)
From the balanced equation, we can see that each mole of ammonium nitrate produces one mole of N2O. Therefore, the mass of ammonium nitrate required would be equal to the molar mass of ammonium nitrate multiplied by the number of moles of N2O produced.
Molar mass of NH4NO3:
N = 14.01 g/mol
H = 1.01 g/mol
O = 16.00 g/mol
Molar mass of NH4NO3 = (14.01 g/mol + 4 * 1.01 g/mol + 3 * 16.00 g/mol)
Molar mass of NH4NO3 = 80.04 g/mol
Mass of ammonium nitrate required = (16.0825 moles) * (80.04 g/mol)
Calculating the mass, we get:
Mass of ammonium nitrate required = 1281.47 grams
Therefore, approximately 1281.47 grams of ammonium nitrate is required to produce 145L of N2O at 2850 torr and 42 degrees Celsius.
To calculate the mass of ammonium nitrate required to produce 145L of N2O at a given temperature (42°C) and pressure (2850 torr), we need to follow these steps:
1. Determine the balanced chemical equation for the reaction: Ammonium nitrate (NH4NO3) decomposes to produce nitrogen gas (N2) and oxygen gas (O2):
NH4NO3 -> N2O + 2H2O
2. Convert the given volume from liters (L) to moles (mol) using the Ideal Gas Law equation: PV = nRT, where P is pressure (in atm), V is volume (in L), n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature (in Kelvin).
First, convert the given temperature from Celsius to Kelvin:
Kelvin = Celsius + 273.15
T = 42 + 273.15 = 315.15 K
Now, rearrange the Ideal Gas Law equation to solve for the number of moles (n):
n = PV / RT
Plugging in the values:
n = (2850 torr * 145L) / (0.0821 L·atm/mol·K * 315.15 K)
n = 1489.75 mol
3. Determine the stoichiometric ratio between ammonium nitrate (NH4NO3) and nitrogen gas (N2O) using the balanced chemical equation:
From the balanced equation:
NH4NO3 -> N2O + 2H2O
The stoichiometric ratio is:
1 mol NH4NO3 produces 1 mol N2O
Therefore, the number of moles of N2O is also 1489.75 mol.
4. Calculate the molar mass of ammonium nitrate (NH4NO3):
Molar mass of NH4NO3 = 14.01 g/mol (N) + 4(1.01 g/mol) (H) + 3(16.00 g/mol) (O) = 80.04 g/mol
5. Use the molar mass of ammonium nitrate to calculate the mass of ammonium nitrate required:
mass = number of moles × molar mass
mass = 1489.75 mol × 80.04 g/mol
The mass of ammonium nitrate required to produce 145L of N2O at 2850 torr and 42 °C is approximately 119.24 kg.