A <---> 2B + C
at a certain temperature the equilibrium pressure of the system is 0.318atm. Determine Kp for this reaction.
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2B + C = 0.318atm /3 = 0.106
CO2 = 0.106 atm
NH3 = 2(1.06) atm =0.212 atm
Kp = PNH3 ^2 x PCO2
kp = 0.212^2 x 0,106
is that how this question is done?
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For % completion, how do you do it for this question?
Consider the rxn; 4A + B <---> 3C. Initially we had 12 mol of A 12 mol of B in a 2.00L flask, At equilibrium, there is 7.5mol of C in the flask.
Find K and % completion?
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I've got K and all the mols at equilibrium when i set up an ice chart for it to go right to equilibrium it goes like this:
4A + B ---> 3C
||4A|B|3C
I| 6 6 0
C|
E|
What must i do to get the %completion because i don't know which is the limiting reactant. thanks!
Can't you calculate the limiting reagent.
Starting with 6 mols B, how many mols A would you need for 100% reaction? That would be 6 mols B x (4 mols A/1 mol B) = 24 mols A and you don't have that much A; therefore, A must be the limiting reagent. Just to check that, how much B would you need for 100% reaction. That would be
6 mols A x (1 mol B/4 mols A) = 1.5 mols B and you have that much (which just proves A is the limiting reagent). Looks to me like you started with 12 mols and ended up with 2 mols (using 10 mols).
To determine the percent completion of a reaction, you need to first determine the limiting reactant. In this case, since you have the initial moles of A, B, and the moles of C at equilibrium, you can compare their stoichiometric ratios to find the limiting reactant.
The stoichiometric ratios for the reaction are:
4A + B --> 3C
Let's compare the moles of A and B to see which one is limiting:
12 mol A / 4 mol A = 3
12 mol B / 1 mol B = 12
Since the stoichiometric ratio of B is higher, it means B is the limiting reactant.
Now, you can calculate the percent completion using the stoichiometry of the reaction.
Percentage completion = (mol of limiting reactant consumed / initial mol of limiting reactant) * 100
Percentage completion = (12 mol B - 7.5 mol C) / 12 mol B * 100
Now you can calculate the percentage completion.
To calculate the percent completion of the reaction, you first need to determine the limiting reactant. The limiting reactant is the one that gets completely consumed and determines the maximum amount of product that can be formed.
In the given equation, 4A + B <---> 3C, we have 12 moles of A and 12 moles of B initially. To find the limiting reactant, we can compare the ratio of moles between A and B to the stoichiometry of the reaction. The stoichiometry tells us that 4 moles of A react with 1 mole of B to form 3 moles of C.
Since we have 12 moles of A and 12 moles of B, the ratio of moles is 12:12, which is equivalent to 1:1. However, the stoichiometric ratio is 4:1. This tells us that B is the limiting reactant because we don't have enough moles of B to react with all the moles of A.
To find the percent completion, we can calculate the moles of C formed and compare it to the maximum moles of C that can be formed from the limiting reactant.
From the stoichiometry, we know that 1 mole of B produces 3 moles of C. Since B is the limiting reactant, we can calculate the maximum moles of C formed using the moles of B.
moles of C = (moles of B) x (moles of C / moles of B) = 12 x (3/1) = 36 moles
Given that at equilibrium, there are 7.5 moles of C in the flask, we can calculate the percent completion.
Percent completion = (moles of C formed / maximum moles of C formed) x 100
= (7.5 / 36) x 100
= 20.8%
Therefore, the percent completion of the reaction is approximately 20.8%.