What volume does 3.01 x 10^21 molecules of N2 occupy at STP?
divide the molecules by 6.022*10^23 to give you how many moles of gas you have. then multiply that by the fact that 1 mole of any ideal gas at stp occupies a volume of 22.4L. you should get .112L
Why did the molecule go to therapy?
Because it had separation anxiety!
Now, back to your question. To find the volume of 3.01 x 10^21 molecules of N2 at STP (Standard Temperature and Pressure), we can use Avogadro's law.
At STP, one mole of any gas occupies 22.4 liters of volume. Since you have the number of molecules, you can convert it to moles by dividing it by Avogadro's number (6.022 x 10^23). Then, multiply the number of moles by 22.4 liters to find the volume.
But let's keep the suspense! Can you guess the volume before we calculate it?
To calculate the volume that 3.01 x 10^21 molecules of N2 occupy at STP (Standard Temperature and Pressure), we can use the ideal gas law formula.
The ideal gas law formula is: PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant = 0.0821 L·atm/(mol·K)
T = temperature (in Kelvin)
STP conditions are defined as 1 atmosphere of pressure and a temperature of 273.15 Kelvin.
First, we need to calculate the number of moles of N2:
To do this, we divide the given number of molecules by Avogadro's number (6.02 x 10^23 molecules/mol):
n = (3.01 x 10^21 molecules) / (6.02 x 10^23 molecules/mol) = 4.99 x 10^-3 mol (rounded to three decimal places)
Now, we can substitute the values into the ideal gas law formula and solve for V:
PV = nRT
(1 atm) * V = (4.99 x 10^-3 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K)
V = [(4.99 x 10^-3 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K)] / (1 atm)
V = 11.2 L (rounded to three significant figures)
Therefore, 3.01 x 10^21 molecules of N2 occupy approximately 11.2 liters of volume at STP.
To find the volume occupied by 3.01 x 10^21 molecules of N2 at STP (Standard Temperature and Pressure), we will use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 atm L/mol K)
T = temperature (in Kelvin)
At STP, the pressure is 1 atm and the temperature is 273.15 K.
First, let's calculate the number of moles (n) of N2:
n = (number of molecules) / (Avogadro's number)
Avogadro's number is approximately 6.022 x 10^23 molecules/mol.
n = (3.01 x 10^21) / (6.022 x 10^23)
= 0.004994 mol
Now, we can rearrange the ideal gas law equation to solve for the volume (V):
V = (nRT) / P
Plugging in the values:
V = (0.004994 mol)(0.0821 atm L/mol K)(273.15 K) / (1 atm)
= 1.21 L
Therefore, 3.01 x 10^21 molecules of N2 occupy approximately 1.21 liters of volume at STP.