The molar mass of Al(OH)3 = 27+(16+1)*3 = 78 g/mol. Dividing the 200.0 g by the molar mass of 78 g/mol = 2.564 moles. From the balanced equation, 2 moles of Al(OH)3 are equivalent to 1 mole of Al2(SO4)3, so if 2.564 moles of Al(OH3) are used, we divide by 2 to find that 1.282 moles of Al2(SO4)3 are formed. The molar mass of Al2(SO4)3 is 27*2+(32.07+16*4)*3 = 342.21 g/mol, so multiplying this by 1.282 moles gives 438.71 grams of aluminum sulfate produced.
The correct option is C. The paragraph is biased, not taking into consideration the other great inventions that have been made. The information given are vague, over generalised, without providing any evidence to support its claims. They are blanket statementso and are not useful at all.
Answer:
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Explanation:
Explanation:
It is known that the oxidation of to is catalyzed by
. In this process, two steps are involved as follows.
(a)
whereas, the second step is
(b)
Balancing the above reaction by multiplying equation (a) by 2 as follows.
(c)
Now, on adding both reaction equations (b) and (c) the net reaction equation will be as follows.
Thus, we can conclude that the equation for the final overall oxidation of by to give is as follows.
Hello,
The correct answer is C
Hope this helps
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