Name two commercial use of oxygen
2 answers:
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Answer : The oxidation state of nitrogen in is, (+5)
Explanation :
Rules for the oxidation numbers :
- The oxidation number of a free element is always be zero.
- The oxidation number of a monatomic ion equal to the charge of the ion.
- The oxidation number of Hydrogen (H) is +1.
- The oxidation number of oxygen (O) in compounds is usually -2, but it is -1 in the peroxides.
- The oxidation number of a Group 1 element in a compound is +1.
- The oxidation number of a Group 2 element in a compound is +2.
- The oxidation number of a Group 17 element in a binary compound is -1.
- The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
- The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.
The given compound is,
Let the oxidation state of 'N' be, 'x'
Hence, the oxidation state of N is, (+5)
Answer : The heat of the reaction is, 1.27 kJ/mole
Explanation :
First we have to calculate the heat released.
Formula used :
or,
where,
Q = heat = ?
m = mass of sample = 1.50 g
c = specific heat of water =
= initial temperature =
= final temperature =
Now put all the given value in the above formula, we get:
Now we have to calculate the heat of the reaction in kJ/mol.
where,
= enthalpy change = ?
Q = heat released = 0.0238 kJ
n = number of moles NH₄NO₃ =
Therefore, the heat of the reaction is, 1.27 kJ/mole