Be sure to answer all parts. The equilibrium constant (K_c) for the formation of
ID: 970287 • Letter: B
Question
Be sure to answer all parts. The equilibrium constant (K_c) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine 2NO(g) + cl_2(g) 2NOCl(g) is 2 Times 10^7 at a certain temperature. In an experiment, 1.80 Times 10^-2 mole of NO, 6.30 Times 10^-3 mole of cl_2-, and 9.40 moles of NOCl are mixed ina 1.10-L flask What is Q_c for the experiment? Times 10 (Enter your answer in scientific motation.) In which direction will the system proceed to reach equilibrium? The reaction will Proceed to the left The reaction will Proceed to the right The reaction is at equilibrium.Explanation / Answer
2 NO + Cl2 --- > 2NOCl
Given that; Kc = 2*10^7
Moles of NO = 1.80*10^-2, Cl2= 6.30*10^-3 and NOCl =9.40 mol
Volume = 1.10 L
Molarity = moles / volume
[NO]= 1.80*10^-2/ 1.10=0.0164
[Cl2]= 6.30*10^-3/ 1.10=5.28*10^-3
[NOCl]= 9.40/ 1.10=8.55
Q for this reaction is given as follows:
Q = [NOCl]^2/ [NO] [Cl]2
Q= (8.55)^2/0.0164* (5.28*10^-3)2
Q= 4.3*10^4
Relation between equilibrium constant and reaction quotient are following:
When both are equal means Q = K then the system is at equilibrium and there is no shift to either the left or the right.
When the value of Q is smaller than Equilibrium constant means Q < K
Thus there are more reactants than products. As a result, the reaction will shift to the right direction or towards products
When the value of Q is greater than Equilibrium constant means Q > K
Thus there are more products than reactants. As a result, the reaction will shift to the left direction or towards reactants.
Here Q is smaller than Equilibrium constant means Q < K
Q= 4.3*10^4< Kc = 2*10^7
Thus there are more reactants than products. As a result, the reaction will shift to the right direction or towards products
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