Question

Canadian chemists have developed a modern variation of the 1899 Mond process for preparing extremely pure metallic nickel. A sample of impure nickel reacts with carbon monoxide at 50°C to form gaseous nickel carbonyl, Ni(CO)₄.
(a) How many grams of nickel can be converted to the carbonyl with 3.55 m³ of CO at 100.7 kPa?

Answer 1

There are 1952.31g of nickel can be converted to the carbonyl with 3.55 m³ of CO at 100.7 kPa.

Given data

The reaction can be written as:

Ni+4CO ⟶$Ni(CO)_{4}$

V(CO)=3.55$m^{3}$

T=50°C=323.5K

p=100700Pa

Now, use the formula:

pV=nR*T  

Where, P is pressure, V is volume and T is temperature.                         n=p∗V / R∗T

n=100700∗3.55  / 8.314∗323.15

It is known that,

n(CO)=133.059mol                            

n(Ni)=n(CO)/4=33.26mol

Mass can be determined by the formula:

Mole = mass / molar mass

Now, put the value of given data in above formula:

m(Ni)=nAr=33.26mol/58.69g/mol      

m(Ni)=1952.31g

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