A 3.00- flask is filled with gaseous ammonia, . The gas pressure measured at 28.0 is 1.55 . Assuming ideal gas behavior, how many grams of ammonia are in the flask?
Please provide units, or the problem is not solvable.
use as a ideal gas behavior
It doesn't matter about ideal behavior or not. What Ryan means is the 3.00 flask 3.00 liters, 3.00 gallons, 3.00 box cars, just what? The 28.0 is what? Degrees Kelvin, degrees C, degrees F, Degrees Rankin, just what? 1.55 atmospheres, 1.55 mm Hg pressure, 1.55 bar, just what? I know its a chore to type in these questions BUT leaving out the unit(s) is not an option.
To determine the number of grams of ammonia in the flask, you can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in L)
n = number of moles of the gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature of the gas (in Kelvin)
First, you need to convert the given pressure from mmHg to atm. Since 1 atm = 760 mmHg, you can calculate the pressure as:
1.55 atm = 1.55 mmHg / 760 mmHg/atm = 0.002039 atm
Next, you need to convert the given temperature from Celsius to Kelvin. You can convert Celsius to Kelvin by adding 273.15. The temperature is given as 28.0°C, so the Kelvin temperature is:
T = 28.0°C + 273.15 = 301.15 K
Now you have the pressure, volume, and temperature. Rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
n = (0.002039 atm) x (3.00 L) / [(0.0821 L·atm/(mol·K)) x (301.15 K)]
Now, calculate the number of moles of ammonia using this equation.
Finally, you need to convert the moles of ammonia to grams. To do this, you need to multiply the number of moles by the molar mass of ammonia, which is 17.03 g/mol.
Mass of ammonia = number of moles of ammonia x molar mass of ammonia (17.03 g/mol)
By substituting the number of moles into the equation, you can calculate the mass of ammonia in grams.