an evil chemist would like to produce 2.4 toones of sulphur dioxide to pollute his city. the chemist know that zinc sulphide and oxygen can react to produce zinc oxide and sulphure dioxide. how much oxygen and zinc will he need to purchase to make his evil, but chemically plausible, plan a reality??? (1 tonne = 1000kg)
i know i post many questions today u guys can find it under my name...i would really like to have all questions answered plzzzz, this is my last question for today thanks again to everyone who can help me out :)
Another stoichiometry problem (maybe two in the same problem). Just follow the steps. Learn to do stoichiometry and you won't have many problems. ;-)
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the amount of oxygen and zinc needed to produce 2.4 tonnes (2400 kg) of sulfur dioxide, we need to calculate the stoichiometric quantities of the reactants.
The balanced chemical equation for the reaction of zinc sulfide (ZnS) with oxygen (O2) to produce zinc oxide (ZnO) and sulfur dioxide (SO2) is:
ZnS + O2 -> ZnO + SO2
From the balanced equation, we can see that the ratio of ZnS to SO2 is 1:1, meaning that for every mole of ZnS, one mole of SO2 is produced.
First, let's calculate the molar mass of SO2:
S (sulfur) has an atomic mass of 32 g/mol
O (oxygen) has an atomic mass of 16 g/mol
So, the molar mass of SO2 is:
32 g/mol (S) + 2 x 16 g/mol (2 O) = 64 g/mol
Now, let's calculate the number of moles of SO2 needed to produce 2400 kg (2.4 tonnes) of it:
Number of moles = mass / molar mass
Number of moles = 2400 kg / (64 g/mol)
Number of moles = 37500 moles
Since the ratio of ZnS to SO2 is 1:1, the number of moles of ZnS needed will be the same as the number of moles of SO2, which is 37500 moles.
Now, let's calculate the molar mass of ZnS:
Zn (zinc) has an atomic mass of 65 g/mol
S (sulfur) has an atomic mass of 32 g/mol
So, the molar mass of ZnS is:
65 g/mol (Zn) + 32 g/mol (S) = 97 g/mol
Finally, let's calculate the mass of zinc needed to produce 2.4 tonnes (2400 kg) of SO2:
Mass of Zn = number of moles x molar mass
Mass of Zn = 37500 moles x 97 g/mol
Mass of Zn = 3637500 g = 3637.5 kg
Therefore, the evil chemist will need to purchase approximately 3637.5 kg of zinc and the same amount of oxygen to produce 2.4 tonnes of sulfur dioxide.