The mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl: ni(co)4 (l) → ni (s) + 4co (g). what volume (l) of co is formed from the complete decomposition of 444 g of ni(co)4 at 752 torr and 22.0 °c?

The volume of CO formed is 254.43 L.

Explanation:

To calculate the number of moles, we use the equation:

Given mass of = 444 g

Molar mass of = 170.73 g/mol

Putting values in above equation, we get:

For the given chemical reaction:

By stoichiometry of the reaction:

1 mole of nickel tetracarbonyl produces 4 moles of carbon monoxide.

So, 2.60 moles of nickel tetracarbonyl will produce = of carbon monoxide.

Now, to calculate the volume of the gas, we use ideal gas equation, which is:

PV = nRT

where,

P = Pressure of the gas = 752 torr

V = Volume of the gas = ? L

n = Number of moles of gas = 10.4 mol

R = Gas constant =

T = Temperature of the gas =

Putting values in above equation, we get:

Hence, the volume of CO formed is 254.43 L.

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