A sample of Nitrogen(N2)& Helium has a volume of 250mL @ 30degrees celsius & a total pressure of 745 mmHg a)If the pressure is 32mmHg what is the partial pressure of the Nitrogen? b) What is the volume of the Nitrogen at STP?
Did not understand previous answer given!
To answer these questions, we need to use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure in atm (or any other appropriate unit)
V = volume in liters (or any other appropriate unit)
n = moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin
Now, let's break down the given information and solve the questions step by step:
a) If the total pressure is 745 mmHg and the pressure of nitrogen is 32 mmHg, we can find the partial pressure of nitrogen by subtracting the pressure of helium from the total pressure. In this case:
Partial pressure of nitrogen = Total pressure - Pressure of helium
Partial pressure of nitrogen = 745 mmHg - 32 mmHg
Partial pressure of nitrogen = 713 mmHg
So, the partial pressure of nitrogen is 713 mmHg.
b) To find the volume of nitrogen at STP (standard temperature and pressure), we need to convert the given volume and temperature to the appropriate units.
1. Convert volume from 250 mL to liters:
Volume = 250 mL * (1 L/1000 mL)
Volume = 0.25 L
2. Convert temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 30°C + 273.15
T(K) = 303.15 K
Now, we can apply the concept of the Avogadro hypothesis, which states that equal volumes of gases at the same temperature and pressure contain an equal number of particles (moles). At STP, 1 mole of gas occupies 22.4 liters.
So, we can set up the following proportion:
Volume of nitrogen / Volume at STP = Moles of nitrogen / Moles at STP
Since the volume at STP is given as 22.4 liters, we can rearrange the equation:
Volume of nitrogen = (Moles of nitrogen / Moles at STP) * Volume at STP
To find the number of moles of nitrogen, we use the ideal gas law equation:
PV = nRT
First, we need to convert the given pressure to atm:
Pressure = 713 mmHg * (1 atm/760 mmHg)
Pressure = 0.9395 atm
Now, we can rearrange the ideal gas law equation to solve for moles:
n = PV / RT
Moles of nitrogen = (0.9395 atm * 0.25 L) / (0.0821 L·atm/mol·K * 303.15 K)
Moles of nitrogen = 0.00936 mol
Now we can substitue the values into the equation for volume at STP:
Volume of nitrogen = (0.00936 mol / 1 mol) * 22.4 L
Volume of nitrogen = 0.209 L
Therefore, the volume of nitrogen at STP is 0.209 liters.