A 3.00-L flask is filled with gaseous ammonia, . The gas pressure measured at 17.0 degree celsius is 2.35atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?

PV=nRT

change temp to K
solve for n.

then, grams=n*formulamassNH3

i need help on this too

To determine the number of grams of ammonia in the flask, we can use the ideal gas law equation:

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

1. Convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 17.0°C + 273.15 = 290.15 K

2. Convert the pressure from atm to Pa:
1 atm = 101325 Pa
P(Pa) = 2.35 atm × 101325 Pa/atm = 237538.75 Pa

3. Rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT

4. Substitute the values into the equation:
n = (237538.75 Pa) × (3.00 L) / [(0.08206 L.atm/mol.K) × (290.15 K)]

5. Solve for n, which gives the number of moles of ammonia in the flask.

6. Finally, calculate the mass of ammonia in grams using the molar mass of ammonia, which is 17.031 g/mol:
Mass (g) = n × molar mass (g/mol)

Following these steps, the number of grams of ammonia in the flask can be determined.