Nitric acid, a very important industrial chemical, is made by dissolving the gas nitrogen dioxide (NO2) in water. Calculate the moles of gas produced in 2 L volume container, 736 torr and 50 ºC if the gas behaves as ideal
Well the formula you need is (P x V) / T. This means pressure times volume divided by temperature. But, you need to convert your temperature to Kelvins. To do this, simply add 273 to your Celsius. Also, you need to convert torr to atmospheres. 760 torr = 1 atm. So you would have to do have 736/760. Once you do this you will have .9684211 x 2 / 323. This will give you .006 if you round up. However, you MAY OR MAY NOT still need to convert this to moles. If you do, find the molar mass and... well, I'll let you figure that out. This should give you your final answer.
You don't write an equation. The best I can find is that 2NO2 + H2O ==> HNO3 + HNO2; i.e., a mixture of nitric and nitrous acids. And your problem asks for moles of "gas" produced in 2L ...... BUT HNO3 is not a gas. Please clarify the problem and repost. It may be that you only want the mols of NO2 gas under those conditions in which case PV = nRT and solve for n.
To calculate the moles of gas produced, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
First, let's convert the given values to the appropriate units:
Pressure: 736 torr = 736/760 atm = 0.9684 atm
Volume: 2 L
Temperature: 50 ºC = 273 + 50 = 323 K
Now we can plug in the values into the Ideal Gas Law equation:
0.9684 atm × 2 L = n × 0.0821 L·atm/mol·K × 323 K
Simplifying the equation:
1.9368 atm·L = n × 26.4883 L·atm/mol
Dividing both sides by 26.4883 L·atm/mol:
n = 1.9368 atm·L / 26.4883 L·atm/mol
n = 0.0731 mol
Therefore, approximately 0.0731 moles of gas are produced in a 2 L volume container at 736 torr and 50 ºC if the gas behaves as an ideal gas.
To calculate the number of moles of gas produced in a given condition, we need to use the ideal gas equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.08206 L·atm/mol·K)
T = temperature (in Kelvin)
First, we need to convert the given pressure from torr to atm:
1 atm = 760 torr
So, the pressure in atm would be:
736 torr / 760 torr/atm ≈ 0.9684 atm
Next, we need to convert the given temperature from Celsius to Kelvin:
K = °C + 273.15
So, the temperature in Kelvin would be:
50 ºC + 273.15 ≈ 323.15 K
Now, we can calculate the number of moles of gas using the ideal gas equation:
n = PV / RT
n = (0.9684 atm) * (2 L) / [(0.08206 L·atm/mol·K) * (323.15 K)]
n ≈ 0.116 moles
Therefore, approximately 0.116 moles of gas would be produced in a 2 L volume container at 736 torr and 50 ºC if the gas behaves as an ideal gas.