a compound had a molecular weight of 112.124 atomic mass units and the empirical formula C3H4O what is the molecular formula of
1 answer:
Answer : The molecular of the compound is,
Solution : Given,
Molecular weight of compound = 112.124 amu
The Empirical formula =
First we have to calculate the empirical formula weight.
The empirical formula weight = 12(3) + 4(1) + 1(16) = 56 gram/eq
Now we have to calculate the molecular formula of the compound.
Formula used :
Molecular formula =
Therefore, the molecular of the compound is,
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Answer : The balanced chemical equation is,
Explanation :
Rules for the balanced chemical equation in basic solution are :
- First we have to write into the two half-reactions.
- Now balance the main atoms in the reaction.
- Now balance the hydrogen and oxygen atoms on both the sides of the reaction.
- If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the more number of oxygen are present.
- If the hydrogen atoms are not balanced on both the sides then adding hydroxide ion
at that side where the less number of hydrogen are present.
- Now balance the charge.
The half reactions in the basic solution are :
Reduction : ......(1)
Oxidation : .......(2)
Now multiply the equation (1) by 2 and then added both equation, we get the balanced redox reaction.
The balanced chemical equation in a basic solution will be,