What is the predicted density of nitrogen gas (N2) at 1.00atm and 298.15K? hint: R=0.0821(Latm)/(molK)

Question

Question

What is the predicted density of nitrogen gas (N2) at 1.00atm and 298.15K?

hint: R=0.0821(L*atm)/(mol*K)

Answer 1

Answer #1

Answer:

From Ideal gas equation, PV=nRT

Where P=pressure, V=volume, R=gas constant, T=temperature,

n=number of moles =mass/molar mass.

PV=(mass/molar mass)RT

Mass/volume=(P x molar mass)/RT

Density=(P x molar mass)/RT (since density=mass/volume)

Given P= 1 atm, T=298.15 K, R=0.0821 L atm mol^-1 K^-1, molar mass of N2=28 g/mol.

Density=(1 atm x 28 g/mol)/(0.0821 L atm mol^-1 K^-1 x 298.15 K)

Density=1.144 g/L.

Therefore the predicted density of N2=1.144 g/L

Thanks and I hope you like it. Please let me know if you have any doubt.

Answer 2

Similar Homework Help Questions

calculate the density of nitrogen gas molar mass n2 28.0g/mol r=0.0821

calculate the density of nitrogen gas molar mass n2 28.0g/mol r=0.0821
1.Ideal Gas Law PV = nRT with atm: R = 0.0821 L*atm/(K*mol) If I have 4...

1.Ideal Gas Law PV = nRT with atm: R = 0.0821 L*atm/(K*mol) If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 2. If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? 3. If I have 7.7 moles of gas at a pressure of 0.09...
If 3.05 mol of a gas has a volume of 43.3 L and a pressure of 1.55 atm, what is the temperature? Use R= 0.0821 atm....

If 3.05 mol of a gas has a volume of 43.3 L and a pressure of 1.55 atm, what is the temperature? Use R= 0.0821 atm. L/mol K. K

Gas Laws Worksheet Name: ah Date: 1224/1g Gas constant R-0.0821 L-atm/K-mol torr I. I atm =...

Gas Laws Worksheet Name: ah Date: 1224/1g Gas constant R-0.0821 L-atm/K-mol torr I. I atm = mmHg = 2. What is Boyle's law? 3. What is Charles's law? 4. What is ideal gas law? 5. What is STP? 6. Write the assumptions made by the Kinetic Molecular Theory.
Use the ideal gas law to calculate the volume occupied by 0.600 mol of nitrogen gas...

Use the ideal gas law to calculate the volume occupied by 0.600 mol of nitrogen gas at 5.00 atm pressure and at 27°C. R = 0.0821 L* atm/(K * mol).
Which of the following are equivalent to 0.0821 (L*atm) / (mol*K)? 62.4 (torr*L) / (mol*K) 8.31...

Which of the following are equivalent to 0.0821 (L*atm) / (mol*K)? 62.4 (torr*L) / (mol*K) 8.31 (J) / (mol*K) 8.31 (Pa*m3) / (mol*K) 8.31 (kPa*L) / (mol*K)

Use the ideal gas law to calculate the volume occupied by 0.200 mol of nitrogen gas...

Use the ideal gas law to calculate the volume occupied by 0.200 mol of nitrogen gas at 1.00 atm pressure and at 27°C. R = 0.0821 L' atm/(K mol). Show your work for full credit.
1.) Use the ideal gas law to calculate the volume occupied by 0.500 mol of nitrogen...

1.) Use the ideal gas law to calculate the volume occupied by 0.500 mol of nitrogen gas at 1.60 atm pressure and at 27°C. R = 0.0821 L*atm/(K*mol). 0.694 L 7.10 L 7.70 L 7.89 L (separate question) 2.What will be the final gas temperature in kelvins?
The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas c...

The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas con- stant, and a (L- atm/mol-) and b (L/mol) are material constants. Determine the volume of 1.5 mol of nitrogen (a .39 L2 atm/mol2. b = 0.03913 L/mol) at temperature of 350 K and pressure of 70 atm. The van der Waals equation...

Determine the volume of 12.5 g of ammonia, NH_3, at STP. (R=0.0821 atm * L/mol*k) how...

Determine the volume of 12.5 g of ammonia, NH_3, at STP. (R=0.0821 atm * L/mol*k) how would you prepare 600 mL of a 0.25 M NaOH solution by diluting a 4.0 M NaOH solution?

What is the predicted density of nitrogen gas (N2) at 1.00atm and 298.15K? hint: R=0.0821(L*atm)/(mol*K)