a mixture of 0.156 moles of C is reacted with 0.117 moles of O2 in a sealed, 10.0L vessel at 500K, producing a mixture of CO amd CO2. The total pressure is 0.640 atm. what is partial pressure of CO?
Well, this seems like a tricky chemistry question, but fear not, for Clown Bot is here to make it more entertaining! So, grab your lab coat and let's dive in!
First, let's calculate the moles of CO and CO2 produced. Since the balanced equation for the reaction C + O2 -> CO + CO2 tells us that the ratio of moles of C to moles of CO is 1 to 1, we know that 0.156 moles of C will produce 0.156 moles of CO. As for CO2, the ratio is 1 to 2, so 0.156 moles of C will produce 0.312 moles of CO2.
Now, let's calculate the total moles of gas in the vessel. We have 0.156 moles of CO and 0.312 moles of CO2, so in total, we have 0.156 + 0.312 = 0.468 moles of gas.
To find the partial pressure of CO, we need to know the mole fraction of CO in the mixture. The mole fraction is the moles of CO divided by the total moles of gas. So, the mole fraction of CO is 0.156 moles / 0.468 moles = 0.333.
Finally, let's calculate the partial pressure of CO. We know that the total pressure in the vessel is 0.640 atm, so the partial pressure of CO is equal to the mole fraction of CO multiplied by the total pressure. Thus, the partial pressure of CO is 0.333 * 0.640 atm = 0.21312 atm.
So, the partial pressure of CO is approximately 0.21312 atm. Don't worry if this math-made dance made you dizzy, I'm always here to entertain and break down the chemical mysteries for you!
To find the partial pressure of CO, we first need to calculate the number of moles of CO produced.
We have the following balanced chemical equation for the reaction between C and O2 to produce CO and CO2:
C + O2 → CO + CO2
By examining the balanced equation, we can see that for every 1 mole of C reacted, we produce 1 mole of CO. So, in this case, the moles of CO produced will be equal to the moles of C.
Given that we have 0.156 moles of C, the moles of CO produced will also be 0.156 moles.
To find the partial pressure of CO, we need to calculate its mole fraction. The mole fraction (X) of a component in a mixture is the ratio of moles of that component to the total moles in the mixture.
Total moles in the mixture = moles of CO + moles of CO2
Total moles in the mixture = 0.156 moles of CO + unknown number of moles of CO2
Since we don't know the number of moles of CO2 yet, we'll represent that as x.
Total moles in the mixture = 0.156 moles of CO + x moles of CO2
The total moles in the mixture can also be calculated as the sum of the moles of C and moles of O2 initially present in the reaction vessel.
Total moles in the mixture = 0.156 moles of C + 0.117 moles of O2
Setting these two expressions for the total moles equal to each other, we have:
0.156 + x = 0.156 + 0.117
Simplifying:
x = 0.117
So, we have found that the number of moles of CO2 produced is 0.117 moles.
Now, to find the mole fraction of CO (X_CO), we'll divide the moles of CO by the total moles in the mixture:
X_CO = moles of CO / total moles in the mixture
X_CO = 0.156 moles of CO / (0.156 moles of CO + 0.117 moles of CO2)
X_CO = 0.156 / (0.156 + 0.117)
X_CO = 0.156 / 0.273
X_CO ≈ 0.571
Finally, to find the partial pressure of CO, we'll multiply the mole fraction by the total pressure:
Partial pressure of CO = X_CO * total pressure
Partial pressure of CO = 0.571 * 0.640 atm
Partial pressure of CO ≈ 0.366 atm
Therefore, the partial pressure of CO is approximately 0.366 atm.
To find the partial pressure of CO, we need to use the mole ratios from the balanced chemical equation and the ideal gas law equation.
First, let's determine the balanced chemical equation for the reaction between carbon (C) and oxygen (O2):
C + O2 -> CO + CO2
From the equation, we can see that for every one mole of carbon reacted, we get one mole of CO produced.
Given that we have 0.156 moles of carbon, we also have 0.156 moles of CO produced. The moles of CO2 can be determined by subtracting from the total moles of carbon and oxygen:
Moles of CO2 = Total moles of carbon and oxygen - Moles of CO
Moles of CO2 = 0.156 moles (C) + 0.117 moles (O2) - 0.156 moles (CO)
Moles of CO2 = 0.156 moles (O2)
Now we know the moles of CO and CO2 produced. To find the partial pressure of CO, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Gas constant
T = Temperature in Kelvin
We are given that the total pressure (P) is 0.640 atm, the volume (V) is 10.0 L, and the temperature (T) is 500K. We can use these values to find the partial pressure of CO.
First, let's calculate the total moles of gas in the mixture:
Total moles = Moles of CO + Moles of CO2
Total moles = 0.156 moles (CO) + 0.156 moles (O2) + 0.156 moles (CO2)
Total moles = 0.468 moles
Now we can calculate the partial pressure of CO using the ideal gas law equation:
P(CO) = (n(CO) / n(total)) * P(total)
P(CO) = (0.156 moles / 0.468 moles) * 0.640 atm
P(CO) = 0.333 * 0.640 atm
P(CO) = 0.213 atm
Therefore, the partial pressure of CO is 0.213 atm.
3C + 2O2 ==> 2CO + CO2
If total pressure at the end is 0.640 atm (the problem doesn't say 0.640 at the end of the reaction but I'm assuming that) then use PV = nRT and solve for n = total moles. I get about 0.1 mol total.
Since CO2 and CO are produced in the ratio of 1:2, then
2*molsCO + 1*mol CO2 = 0.1
2x + x = 0.1 and
x = about 0.033 and 2x = about 0.67. These are approximate; you should use more significant figures than that.
Then pCO = XCO*Ptotal.