Ammonium sulfate, an important chemical fertilizer, can be prepared by the reaction of ammonia with sulfuric acid according to the following balanced equation:
2 NH3(g) + H2SO4(aq) → (NH4)2SO4(aq)
If a reaction vessel has 5.1 L of NH3 at 41.8°C and 25.6 atm, how many grams of H2SO4 are needed to completely react with it?
_________________ g H2SO4. Do NOT enter unit. Report your final answer with 3 SFs.
TBH i don't know how to do it. IF someone can help I'll Appreciate it! and Thank you! :)
I assume the 5.1 L NH3 is as a gas. So how many moles is that?
Use PV = nRT.
You know P = 25.5 atm
You know V = 5.1 L
n = ?
R = 0.0821 L*atm/mol*K
T = 41.8 C = 273 + 41.8 = ? K . Use K in the above equation.
Since the equation tells you 2 mol NH3 = 1 mol H2SO4, the mols H2SO4 = 1/2 mols NH3.
grams H2SO4 = mols H2SO4 x molr mass H2SO4 = ?
Post your work if you get stuck.
oops. Typo.
P = 25.6 atm.
N= PT v1/RT1 =
(25.6) (5.1) / (0.0821) (314.6) =
130.56 / 25.82866 = 5.0548
(5.0548) (
I don't know what I am doing LMAO
So far you're doing great, except for a typo. You copied the T twice and you meant n = P1V1/RT1. (N= PT v1/RT1 The T on the left is a typo). Also I think you meant 314.8 for K but that's not much of a problem. I obtained 5.05 as a rounded number. So
n = 5.0548 mols is essentially orrect. Now just do the rest.
You take half of that to get mols H2SO4 then multiply by molar mass of H2SO4.
I can see you're terribly confused. After you finish the problem tell me what is confusing you and why you don't think you know what you're doing.
To solve this problem, we need to use the ideal gas law to calculate the number of moles of ammonia (NH3) in the reaction vessel.
The ideal gas law is given by the equation:
PV = nRT
Where:
P = pressure of the gas in atmospheres (atm)
V = volume of the gas in liters (L)
n = number of moles of gas
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature in Kelvin (K)
First, we need to convert the temperature from Celsius to Kelvin. The equation to convert Celsius to Kelvin is:
T(K) = T(°C) + 273.15
So, let's convert the temperature from 41.8°C to Kelvin:
T(K) = 41.8°C + 273.15 = 314.95 K
Next, we rearrange the ideal gas law equation to calculate the number of moles (n):
n = PV / RT
Substituting the given values into the equation:
n = (25.6 atm) * (5.1 L) / (0.0821 L.atm/mol.K * 314.95 K)
Simplifying the expression:
n = 3.25 mol
Now, according to the balanced equation, the stoichiometric ratio between NH3 and H2SO4 is 2:1. This means that 2 moles of NH3 react with 1 mole of H2SO4.
So, 3.25 moles of NH3 will react with (3.25 / 2) moles of H2SO4.
Now, we need to calculate the molar mass of H2SO4, which is:
(2 * atomic mass of H) + atomic mass of S + (4 * atomic mass of O) = (2 * 1.01 g/mol) + 32.07 g/mol + (4 * 16.00 g/mol) = 98.09 g/mol
Finally, let's calculate the mass of H2SO4 needed:
Mass of H2SO4 = (3.25 / 2) * 98.09 g/mol = 162.15 g
Therefore, the mass of H2SO4 needed to completely react with 5.1 L of NH3 is 162.15 g.