calculate the mass of 120 cc of nitrogen at NTP. How many number of molecules are present in it?
5.35 Moles at NTP
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To calculate the mass of nitrogen in 120 cc (cubic centimeters) at NTP (normal temperature and pressure), we need to know the molar mass of nitrogen. The molar mass of nitrogen (N₂) is approximately 28 grams/mole.
Now, let's convert the volume from cc to liters. 1 cc is equal to 0.001 liters (since there are 1000 cc in one liter). Therefore, 120 cc is equal to 0.12 liters.
Next, we can use the ideal gas equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature.
At NTP, the pressure (P) is 1 atmosphere and the temperature (T) is 273 Kelvin.
By rearranging the ideal gas equation to solve for moles (n), we get:
n = PV / RT
Plugging in the values:
n = (1 atm * 0.12 L) / (0.0821 L·atm/mol·K * 273 K)
n ≈ 0.005 moles
Now, to find the mass, we multiply the moles by the molar mass:
mass = moles * molar mass
mass = 0.005 moles * 28 g/mol
mass ≈ 0.14 grams
So, the mass of 120 cc of nitrogen at NTP is approximately 0.14 grams.
To find the number of molecules, we can use Avogadro's number, which is approximately 6.022 x 10²³ molecules per mole.
Number of molecules = moles * Avogadro's number
Number of molecules = 0.005 moles * (6.022 x 10²³ molecules/mol)
Number of molecules ≈ 3.01 x 10²¹ molecules
Therefore, there are approximately 3.01 x 10²¹ molecules of nitrogen in 120 cc at NTP. That's a whole lot of little nitrogen guys!
To calculate the mass of nitrogen, we need to know its molar mass. The molar mass of nitrogen (N2) is 28 g/mol.
Step 1: Convert the volume from cc to liters.
1 cc = 1 mL
1 L = 1000 mL
So, 120 cc = 120 mL = 120/1000 L = 0.120 L
Step 2: Use the ideal gas law equation to calculate the number of moles of nitrogen.
The ideal gas law equation is: PV = nRT
At NTP (Normal Temperature and Pressure), the values are:
P = 1 atm
V = 0.120 L
T = 273 K
R = 0.0821 L·atm/(mol·K)
Substituting these values into the equation and solving for n, we have:
(1 atm)(0.120 L) = n(0.0821 L·atm/(mol·K))(273 K)
0.120 = n(0.0821)(273)
0.120 = n(22.414)
n = 0.120 / 22.414
n = 0.00536 mol
Step 3: Calculate the mass of nitrogen.
The mass of nitrogen is equal to the molar mass (28 g/mol) multiplied by the number of moles (0.00536 mol):
mass = molar mass × moles
mass = 28 g/mol × 0.00536 mol
mass = 0.15008 g
So, the mass of 120 cc of nitrogen at NTP is approximately 0.15008 grams.
Next, let's calculate the number of molecules present in it.
Step 4: Use Avogadro's number to convert moles to molecules.
Avogadro's number (NA) is 6.022 × 10^23 molecules/mol.
Number of molecules = moles × Avogadro's number
Number of molecules = 0.00536 mol × 6.022 × 10^23 molecules/mol
Number of molecules = 3.22592 × 10^21 molecules
Therefore, there are approximately 3.22592 × 10^21 molecules of nitrogen in 120 cc at NTP.
To calculate the mass of nitrogen at NTP (Normal Temperature and Pressure) and the number of molecules present in it, we need to use a series of steps.
1. Convert the volume from cubic centimeters (cc) to liters (L):
Since 1 L is equivalent to 1000 cc, we can calculate:
Volume in L = Volume in cc / 1000 = 120 cc / 1000 = 0.12 L
2. Determine the molar mass of nitrogen (N₂):
The molar mass of nitrogen is the sum of the atomic masses of two nitrogen atoms (N):
Molar mass of N₂ = 2 * atomic mass of N = 2 * 14.01 g/mol = 28.02 g/mol
3. Use the ideal gas equation to calculate the number of moles of nitrogen:
The ideal gas equation is given by: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin.
At NTP, the temperature is 273.15 Kelvin and the pressure is 1 atmosphere. Substituting these values into the ideal gas equation, we can solve for the number of moles (n):
n = PV / RT = (1 atm) * (0.12 L) / (0.0821 L·atm/(mol·K) * 273.15 K)
4. Calculate the mass of nitrogen:
To find the mass of nitrogen, we multiply the number of moles (n) by the molar mass of nitrogen (Molar mass of N₂):
Mass of nitrogen = n * Molar mass of N₂
5. Calculate the number of molecules:
To find the number of molecules, we use Avogadro's number (6.02214x10²³ molecules/mol). Multiply the number of moles (n) by Avogadro's number:
Number of molecules = n * Avogadro's number
Now, let's calculate the mass of nitrogen and the number of molecules present in 120 cc of nitrogen at NTP.
Step 1: Volume in L = 0.12 L
Step 2: Molar mass of N₂ = 28.02 g/mol
Step 3: Calculate the number of moles (n):
n = (1 atm) * (0.12 L) / (0.0821 L·atm/(mol·K) * 273.15 K)
Step 4: Mass of nitrogen = n * Molar mass of N₂
Step 5: Number of molecules = n * Avogadro's number
Using these steps, you can calculate the mass of nitrogen and the number of molecules in 120 cc of nitrogen at NTP.
well, one mole at STP occupies 22.4L
mass of sample: .120/22.4 * molmassN2
number of molecules: .120/22.4* avagradros Number