IM SO CONFUSED PLEASE HELP!
H2 +CO2-->H2O + CO
When H2 is mixed with CO2 at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.
[H2]= 0.20mol/L
[CO2]= 0.30mol/L
[H2O]=[CO]= 0.55mol/L
a/ what is the mole fraction of CO in the equilibrium mixture?
b/ using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constanst for the reaction.
c/ determine Kp in terms of Kc for this system.
d/ when the system is colld rom 2,000K to a lower temperature, 30.0 percent of the CO is converted back to CO2. Calculate the valu of Kc at this lower temperature.
e/in a different experiment, 0.50mole of H2 is mixed with 0.50 mole of CO2 in a 3.0-liter reaction vessel at 2,000K. Calculate the equilibrium concentration, in moles per liter, of CO at this temperature.
You may be confused but surely you know how to do parts of this? Tell me what you don't understand about it and I can help you through it. For starters, the mole fraction of CO = mols CO/total mols.
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we're doing this in class right now.... :/
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Behold my glory!
Can someone please answer this
How do you do D & E
I'm not so sure about E, but if you do the ICE chart, and equate Kc to 5, you can solve by plugging in the values of your Equilibrium concentrations into your Kc equation(again, refer to b). My answer is 0.118M CO, but I could be wrong.
Sure! Let's break down each part of the problem and I'll explain how to solve it.
a/ To find the mole fraction of CO in the equilibrium mixture, we need to calculate the moles of CO and the total moles in the system.
Given:
[H2] = 0.20 mol/L
[CO2] = 0.30 mol/L
[H2O] = [CO] = 0.55 mol/L
To calculate the moles of CO:
Since [CO] = 0.55 mol/L, we know that the number of moles of CO is equal to the concentration multiplied by the volume of the system. Let's assume the volume is V.
moles of CO = [CO] * V
To calculate the total moles in the system:
Since we have the concentrations of H2, CO2, H2O, and CO, we can calculate the total moles by adding the moles of each component.
total moles = moles of H2 + moles of CO2 + moles of H2O + moles of CO
Once you have calculated the moles of CO and the total moles, you can find the mole fraction of CO using the formula:
mole fraction of CO = moles of CO / total moles
b/ To calculate the value of Kc, the equilibrium constant for the reaction, we need to use the equilibrium concentrations given.
The equilibrium constant expression for this reaction is:
Kc = ([H2O] * [CO]) / ([H2] * [CO2])
Simply substitute the given equilibrium concentrations into the expression to find the value of Kc.
c/ To determine Kp in terms of Kc for this system, we need to know the difference in the number of moles of gas on both sides of the equation.
The balanced equation for the reaction is:
H2 + CO2 -> H2O + CO
In this equation, we have 4 moles of gas on the left side (H2 and CO2) and 2 moles of gas on the right side (H2O and CO).
The relation between Kp and Kc for this system is:
Kp = Kc * (RT)^(delta n)
Where R is the ideal gas constant, T is the temperature in Kelvin, and delta n is the difference in the number of moles of gas on the product side and the reactant side.
Calculate the value of delta n (delta n = 2 - 4) and substitute the known values into the equation to find Kp in terms of Kc.
d/ To calculate the value of Kc at a lower temperature when 30.0 percent of CO is converted back to CO2, we need to apply the concept of the shift in equilibrium due to a change in temperature.
Since the reaction is exothermic (it releases heat), decreasing the temperature will favor the forward reaction. As a result, some of the CO will be converted back to CO2.
To calculate the new value of Kc, we need to determine the new equilibrium concentrations of all species. We know that 30.0 percent of the initial moles of CO have been converted, so we can calculate the new equilibrium concentrations based on this information.
e/ To calculate the equilibrium concentration of CO in a different experiment where 0.50 mol of H2 is mixed with 0.50 mol of CO2 in a 3.0-liter reaction vessel at 2,000K, we can use the initial moles and the volume to determine the concentrations.
First, calculate the initial concentrations of H2 and CO2 by dividing the number of moles by the volume. Then, use the concept of stoichiometry to determine the change in moles for each species. Finally, calculate the new equilibrium concentrations based on the information given.