Determine the value of the equilibrium constant,Kgoal , for the reaction
N2(g)+O2(g)+H2(g)<=> (1/2)N2H4(g) + NO2(g)
Kgoal=?
by making use of the following information:
1.N2(g)+O2(g)<=>2NO(g), K1=4.1010x10^-31
2.N2(g)+2H2(g)<=>N2H4(g), K2=7.40x10^-26
3.2NO(g)+O2(g)<=>2NO2(g), K3=6.00x10^-13
express your answer numerically:
K_goal=(K1×K2×K3)^1/2
Take 1/2 equation 1, add to 1/2 equation 3, add to equation 2 to get the equation you want. K for that reaction is
(sqrt k1) x (sqrt k3) x k2
To determine the value of the equilibrium constant Kgoal for the given reaction, we can use the concept of equilibrium constant expressions.
The given reaction:
N2(g) + O2(g) + H2(g) <=> (1/2)N2H4(g) + NO2(g)
can be obtained by combining reactions 1, 2, and 3 in the given information. The following steps will guide us through the process:
Step 1: Write down the balanced equations for reactions 1, 2, and 3.
1. N2(g) + O2(g) <=> 2NO(g)
2. N2(g) + 2H2(g) <=> N2H4(g)
3. 2NO(g) + O2(g) <=> 2NO2(g)
Step 2: Combine the balanced equations to obtain the desired reaction.
By multiplying reaction 1 by 1/2 and combining with reaction 2 and reaction 3:
1/2 N2(g) + O2(g) + H2(g) <=> (1/2)N2H4(g) + NO2(g)
The corresponding equilibrium constant expression is:
Kgoal = (K2 * K3) / K1
Step 3: Substitute the values of K1, K2, and K3.
Kgoal = (7.40x10^-26 * 6.00x10^-13) / 4.1010x10^-31
Step 4: Perform the calculation.
Kgoal = 1.14x10^6
Therefore, the value of the equilibrium constant Kgoal for the given reaction is 1.14x10^6.
To determine the value of the equilibrium constant, Kgoal, for the reaction provided, we need to use the concept of equilibrium constants for reactions that can be combined to give the overall desired reaction.
The given reaction can be obtained by combining three previous reactions mentioned, i.e.,
N2(g)+2H2(g) <=> N2H4(g) (Multiplying the second reaction by 2)
2NO(g)+O2(g) <=> 2NO2(g) (Third reaction as it is)
To find the value of Kgoal, we need to multiply the equilibrium constants of the individual reactions together. However, since the third reaction is reversed in the desired reaction, we need to take the inverse of K3.
Therefore,
Kgoal = (K2) x (1/K3)
Substituting the values gives us:
Kgoal = (7.40x10^-26) x (1/(6.00x10^-13))
Now, we can calculate the numerical value of Kgoal by performing the multiplication and division:
Kgoal = 1.23 x 10^-13
Therefore, the value of the equilibrium constant, Kgoal, for the given reaction is 1.23 x 10^-13.