Use the References to access important values if needed for this question. Consi

Question

Use the References to access important values if needed for this question. Consider the following reaction where K- 1.80 10 at 298 K i moles of NH·HS(s), s 6610' moles of NH @l and 134 101 moles of His A reaction mixture was found to contain 5.6310 1.00 liter container Is the reaction at equilibrium If not, what direction must it run in order to reach equilibrium The reaction quotient, Q. equals The reaction A. must run in the forward direction to reach equilibrium B. must run in the reverse direction to reach equalibrium C. is at equilibriom 1 more group attempt remaining

Explanation / Answer

NH4HS(s)        <-------->        NH3(g)        +        H2S(g)

Molarity = Moles / Liter

Moles of
NH4HS(s) = 5.63 x 10-3 moles
NH3(g) = 8.66 x 10-3 moles
H2S(g) = 1.34 x 10-3 moles

Volume = 1 L

So, molarity are
NH4HS(s) = 5.63 x 10-3 M
NH3(g) = 8.66 x 10-3 M
H2S(g) = 1.34 x 10-3 M

Kc = 1.80 x 10-3 = [NH3]eq [H2S]eq / [NH4HS]eq

The reaction quotients,

Qc = [NH3] [H2S] / [NH4HS]
     = (8.66 x 10-3) (1.34 x 10-3) / (5.63 x 10-3)
     = 2.06 x 10-3

So,
Qc = 2.06 x 10-3
Kc = 1.80 x 10-3

Qc > Kc

So, the reaction is not in equilibrium, since Qc is not equal to Kc.

The reaction must run reverse (backward) direction to increase the concentration of [NH4HS], to decrease the value of Qc. That is when the denominator term will increase, the quotient will decrease.

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