Nickel metal will react with CO gas to form a compound called nickel tetracarbon

Question

Nickel metal will react with CO gas to form a compound called nickel tetracarbonyl (Ni(CO)4), which is a gas at temperatures above ~45°C.

A 1.50-L glass bulb is filled with CO gas to a pressure of 1.20 atm at 73.0°C, and then 0.5869 g of pure Ni is added. If the reaction described above occurs and goes to completion at constant temperature, what will the final total pressure in the bulb be? (You can assume that any volume occupied by the solid nickel is negligible compared to the volume of the flask.)

Explanation / Answer

Assuming ideal behaviour of the gases involved.

Moles of CO initiallly = n = PV/RT = 1.2x1.5/0.0821x350 =0.0626 moles

(nickel is the limiting reagent so consumed all)

            Ni (s)                     +         4 CO (g)    -------->   Ni(CO)4 (g)

t=o               0.5869/58.69           .0626 moles                        0

                .01 mole                    .0626 mole                           .01 mole formed

After reaction   .01-.01 =0                     .0626-.04 = .0226 moles         .01 mole formed

Total Moles of All gases = .0226 + .01 = .0326 moles

Applying PV=nRT

P = nRT/V = .0326x0.0821x 350/1.5 = .624 atm

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