Question

Nickel and carbon monoxide react to form nickel carbonyl like this: Ni(s) + 4CO(g) ⇔ Ni(CO)4(g)...

Nickel and carbon monoxide react to form nickel carbonyl like this:

Ni(s) + 4CO(g) ⇔ Ni(CO)4(g)

A 7.8 L vessel contains a mixture of nickel, carbon monoxide, and nickel carbonyl with the composition tabulated below. What is the value of the equilibrium constant, Kc?

compound amount

Ni 50.1

CO 1.9

Ni(CO)4 .307

A. 0.16

B. 4.0 × 10^4

C. 2.4 × 10^-2

D. 4.7 × 10^-4

E. 3.7 × 10^5

Homework Answers

Answer #1

Number of moles of CO = 1.9/28 = 0.0678 moles

Since the volume of vessel is 7.8L

Hence molarity of CO = number of moles/Volume of solution(L) = 0.00869 M

Molar mass of Ni(CO)4 = 170.73 gm/mol

moles of Ni(CO)4 = 0.307/170.73 = 0.00179 moles

Molarity of Ni(CO)4 = 0.0179/7.8 = 2.3053 * 10^(-4)

Kc = [Ni(CO)4]/[CO]^4 (conc of Ni doesn't matter since it is present in the solid phase)

=> 2.3053 * 10^(-4)/(0.00869)^4

=> 4.0424 * 10^(4)

Hence the correct answer is Option B

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the reaction: NiO(s)+CO(g)⇌Ni(s)+CO2(g) Kc=4.0×103 at 1500 K If a mixture of solid nickel(II) oxide and...
Consider the reaction: NiO(s)+CO(g)⇌Ni(s)+CO2(g) Kc=4.0×103 at 1500 K If a mixture of solid nickel(II) oxide and 0.10 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of CO2?
In the Mond process for the purification of nickel, carbon monoxide is reacted with heated nickel...
In the Mond process for the purification of nickel, carbon monoxide is reacted with heated nickel to produce Ni(CO)4, which is a gas and can therefore be separated from solid impurities: Ni(s) + 4CO(g) ⇌ Ni(CO)4(g) Given that the standard free energies of formation of CO(g) and Ni(CO)4(g) are −137.3 and −587.4 kJ/mol, respectively, calculate the equilibrium constant of the reaction at 78.0 ° C. Assume that Δ G o f is temperature-independent.
The following reaction describes the formation of nickel tetracarbonyl: Ni(s) + CO(g) --> Ni(CO)4(g) Consider a...
The following reaction describes the formation of nickel tetracarbonyl: Ni(s) + CO(g) --> Ni(CO)4(g) Consider a reaction which produces 12.4 g of nickel tetracarbonyl. a) balance the reaction equation b) Find the number of grams of Ni(s) and CO(g) which reacted.
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An...
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An equilibrium mixture in a 1.50 −L vessel is found to contain 7.17×10−2 mol CH3OH, 0.170 mol CO, and 0.301 mol H2 at 500 K. Calculate Kc at this temperature.
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An...
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An equilibrium mixture in a 1.50 −L vessel is found to contain 7.17×10−2 mol CH3OH, 0.170 mol CO, and 0.301 mol H2 at 500 K. Part A Calculate Kc at this temperature.
CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 464...
CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 464 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.780 Cl2 1.22 COCl2 0.120 What is the equilibrium constant, Kp, of this reaction? Part B The following reaction was performed in a sealed vessel at 767 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.75M and [I2]=2.05M. The equilibrium concentration...
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2HNO3 (aq)...
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2HNO3 (aq) + NO (g) → 3NO2 (g) + H2O (l) At a certain temperature, a chemist finds that a 9.5L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 15.5g NO 16.6g NO2 22.5g H2O 189.0g Calculate the value of the equilibrium constant Kc for this reaction. Round your answer to...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are equal b)the value of the equilibrium constant is 1 c)all chemical reactions have ceased d)the rate constants of the forward and reverse reactions are equal e)the limiting reagent has been consumed 2)The equilibrium-constant expression depends on the ________ of the reaction. a) stoichiometry b) mechanism c) the quantities of reactants and products initially present d) temperature e) stoichiometry and mechanism 3)Given the following reaction...