The partial pressures of the four gases contained in a 6 L cylinder at 100 °C were: CO2 = 63.1 atm; H2 = 21.1atm; CO = 84.2 atm; H2O = 31.6 atm. How many grams of CO2 were in the cylinder?
Can someone please help me. These pressure/gas problems are so difficult for me as I can never seem to do much of them
The real purpose of this problem is for you to realize that the gases and their pressures are independent of each other; i.e., You have Liters, partial pressure of CO2, and T. So use PV = nRT, solve for n to find moles, then mols = grams/molar mass to find grams. Remember to convert T to kelvin.
Post your work if you get stuck.
That's right. Dalton's law tells us that each gas has a partial pressure that is its own and is independent of other gases present in the mixture. So you know the pressure of the CO2 will give you the mols from PV = nRT FOR CO2. You could find mols and grams for each of the other gases, too. The total pressure of course is the sum of each of the partial pressures.
So that means I don't need the partial pressure of H2, CO and H2O?
Oh no, it seems like you're feeling a little deflated when it comes to these gas problems! Don't worry, I'll inflate your spirits and help you out!
To find the number of grams of CO2 in the cylinder, we need to use the ideal gas law which states:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, let's convert the temperature from °C to Kelvin. We add 273 to the temperature to get 373 K.
Next, we can calculate the number of moles of CO2 using the ideal gas law:
(n = PV / RT)
Let's plug in the values:
P = 63.1 atm
V = 6 L
R = 0.0821 L·atm/(mol·K)
T = 373 K
n = (63.1 atm * 6 L) / (0.0821 L·atm/(mol·K) * 373 K)
Now, let's calculate that:
n ≈ 146.16 mol
Finally, to find the mass of CO2, we can use the molar mass of CO2, which is approximately 44 g/mol.
Mass = (n * molar mass) = (146.16 mol * 44 g/mol)
So, the number of grams of CO2 in the cylinder is about 6431.04 g.
But hey, don't let these gas problems get to your head. Keep breathing, take a break, and remember that we're here to support you!
Sure, I'd be happy to help you solve this problem! Gas law problems can be challenging, but let's go through the solution step by step.
The first step is to understand the given information. We have a 6 L cylinder containing four gases: CO2, H2, CO, and H2O. We are given their respective partial pressures: CO2 = 63.1 atm, H2 = 21.1 atm, CO = 84.2 atm, and H2O = 31.6 atm. We need to find the number of grams of CO2 in the cylinder.
To solve this problem, we will use the ideal gas law equation: PV = nRT. This equation relates the pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T) of a gas.
To find the number of moles of CO2, we need to rearrange the ideal gas law equation:
n = PV / RT
where n is the number of moles of gas, P is the pressure, V is the volume, R is the gas constant, and T is the temperature in Kelvin.
However, before we proceed, we need to convert the temperature from Celsius to Kelvin. The temperature in Kelvin (T) is equal to the temperature in Celsius (T°C) plus 273.15.
Given that the temperature is 100 °C, we can convert it to Kelvin:
T = 100 °C + 273.15 = 373.15 K
Now, let's calculate the number of moles of CO2:
n(CO2) = (CO2 pressure) x (cylinder volume) / (gas constant) x (temperature)
n(CO2) = (63.1 atm) x (6 L) / (0.0821 L·atm/mol·K) x (373.15 K)
Calculating this expression gives us the number of moles of CO2 present in the cylinder.