For the reaction below, K_c = 0.060 at a certain temperature. N_2(g) + 3H_2(g) 2

Question

For the reaction below, K_c = 0.060 at a certain temperature. N_2(g) + 3H_2(g) 2NH_3(g) A flask contains 1.0 M N_2, 1.0 M H_2 and 1.0 M NH_3. Is this system at equilibrium? If not, will the equilibrium concentration of NH_3 be greater than, or less than 1.0 M? Justify your answers. For the reaction below, K_e = 0.143 at a particular temperature 2BrCl_2(g) Br_2(g) + Cl_2(g) A flask initially contains 1.0 M of each of the three substances. What will be the equilibrium concentration of each chemical?

Explanation / Answer

6)

Qc = [NH3]^2 / [N2] [H2]^3

= (1.0)^2 / (1.0) * (1.0)^3

= 1.0

here QC > Kc,

So, reaction must shift to left to reestablish equilibrium. This will decrease the concentration of NH3

So, concentration of NH3 will be less than 1

Answer: less than 1

I am allowed to answer only 1 question at a time

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