150.0 mL flask contains 740. g of N2 at 0°C.
What is the pressure in atm.
What is the pressure in torr?
What is the pressure in psi?
I know you have to do:
n = grams/molar mass
Then PV = nRT
R in 0.08206 L.atm/mol.K gives P in atm
atm x 760 = p in torr
1 atm = 14.7 psi
Show your work. Probably you aren't following my instructions OR I goofed somewhere.
I really struggle in chemistry sometimes I know the formulas but I don't know how to put the correct numbers where they need to be .
Knowing the formulas won't do much good if you don't know how to use them. It is important to use the right units.
Looking at the last problem for which you posted your work, see if my correction helps you in the others. If post specific questions, show your work, and explain what your trouble is and we can help you through.
For PV = nRT
p is in atm, V in L, R is 0.08206 and T in kelvin.
If p in kPa, V in L, R is 8.314 and T in kelvin.
n in both cases is grams/molar mass
To find the pressure in atm, torr, and psi, 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.
Let's begin by finding the number of moles of N2.
Step 1: Calculate the molar mass of N2.
The molar mass of N2 is approximately 28 g/mol since nitrogen (N) has an atomic mass of 14 g/mol, and there are two nitrogen atoms in N2.
Step 2: Calculate the number of moles.
To find the moles of N2, divide the given mass (740 g) by the molar mass (28 g/mol).
n = 740 g / 28 g/mol ≈ 26.43 mol
Now, let's proceed to find the pressure in atm.
Step 3: Convert the temperature to Kelvin.
The given temperature is 0°C, which needs to be converted to Kelvin. To convert Celsius to Kelvin, simply add 273.15.
T = 0°C + 273.15 K = 273.15 K
Step 4: Use the Ideal Gas Law to find the pressure in atm.
Plug the values into the equation PV = nRT:
P * 150 mL = 26.43 mol * 0.08206 L.atm/mol.K * 273.15 K
First, we need to convert milliliters (mL) to liters (L). Since there are 1000 mL in a liter, the volume becomes:
150 mL * (1 L / 1000 mL) = 0.15 L
Now we can solve for P:
P * 0.15 L = 26.43 mol * 0.08206 L.atm/mol.K * 273.15 K
P = (26.43 mol * 0.08206 L.atm/mol.K * 273.15 K) / 0.15 L
P ≈ 4.53 atm
Therefore, the pressure in the 150.0 mL flask containing 740.0 g of N2 at 0°C is approximately 4.53 atm.
To find the pressure in torr, we can use the conversion factor: 1 atm = 760 torr.
Pressure in torr = 4.53 atm * 760 torr/atm
Pressure in torr ≈ 3,448.8 torr
Finally, to find the pressure in psi, we can use the conversion factor: 1 atm = 14.7 psi.
Pressure in psi = 4.53 atm * 14.7 psi/atm
Pressure in psi ≈ 66.591 psi
Therefore, the pressure of the N2 gas in the 150.0 mL flask at 0°C is approximately 4.53 atm, 3,448.8 torr, and 66.591 psi.