At o degrees celcius, a 1.0-L flask contains 5.0 x 10^-2 mol N2, 1.5 x 10^2 mg O2 and 5.0 x 10^21 molecules of NH3. What is the p00artial pressure of each gasnand what is the total pressure in the flask?
I need to understand how to calculate it, formula and how to get the proper answer..please!
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This is not a complicated problem but it is long and involves several steps.
1. Convert the gases to mols.
a. you have mols N2 as 0.05.
b. Convert 150 mg O2 to grams, then mols = grams/molar mass. mols O2 = ?
c. Convert 5E21 molecules NH3 to mols. That is 5E21 molecules x (1 mol/6.02E23 molecules) = ? mols NH3.
2. Find individual pressure of each gas. Use PV =nRT. Substitute n for each gas. You know R and T (remember T must be in kelvin), P is in atm and volume in L.
3.. Now find the total pressue by adding the partial pressures of each gas. The sum is Ptotal.
Post your work if you have trouble so I will know where you are going wrong.
To calculate the partial pressure of each gas, we need to use the ideal gas law and consider the number of moles or molecules and their individual gas constants. The ideal gas law is given by the equation:
PV = nRT
where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
First, we need to convert the temperature from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature. So, 0 degrees Celsius is equal to (0 + 273.15) = 273.15 Kelvin.
Let's calculate the partial pressure of each gas step by step:
1. N2:
Given: n(N2) = 5.0 x 10^-2 mol
We can calculate the partial pressure of N2 using the formula:
P(N2) = (n(N2) * R * T) / V
Substituting the values:
P(N2) = (5.0 x 10^-2 * 0.0821 * 273.15) / 1.0
2. O2:
Given: m(O2) = 1.5 x 10^2 mg
We need to convert the mass to moles to use the ideal gas law. The molar mass of O2 is 32 g/mol.
First, convert the mass from mg to g:
m(O2) = 1.5 x 10^5 g
Next, convert the mass to moles:
n(O2) = m(O2) / molar mass(O2)
Substituting the values:
n(O2) = (1.5 x 10^2 / 32)
Once we have the number of moles, we can calculate the partial pressure of O2:
P(O2) = (n(O2) * R * T) / V
3. NH3:
Given: n(NH3) = 5.0 x 10^21 molecules
To use the ideal gas law, we need to convert the number of molecules to moles. The molar mass of NH3 is 17 g/mol.
First, convert the number of molecules to moles:
n(NH3) = 5.0 x 10^21 / Avogadro's number
Substituting the values:
n(NH3) = (5.0 x 10^21 / 6.022 x 10^23)
Once we have the number of moles, we can calculate the partial pressure of NH3:
P(NH3) = (n(NH3) * R * T) / V
Finally, to calculate the total pressure in the flask, we add up the partial pressures of each gas:
Total Pressure = P(N2) + P(O2) + P(NH3)
You can now substitute the variables and values into the equations and perform the calculations to get the answers.