Answer:
The chemical equation that is properly balanced is;
e. Sn + 4HNO₃ → SnO₂ + 4NO₂ + 2H₂O
Explanation:
To solve the question, we note the reactions thus and we look for a reason why the reaction is not balanced as follows.
a. CH₃CHO + 3O₂ → 2CO₂ + 2H₂O
Here we have 7 oxygen atoms in the reactant and 6 in the products
Not balanced
b. NH₄NO₃ → 2H₂O + N₂
Here we have three oxygen in the reactant and four in the products = Not balanced
c. Na₂CO₃ + 2H₂SO₄ → Na₂SO₄ + 2H₂O + CO₂
Here we have 11 oxygen atoms in the reactant and 8 in the products = Not balanced
d. 2Na₂SO₄ + 3Bi(NO₃)₃ → Bi₂(SO 4)₃ + 9NaNO₃
Here we have 2 Na in the reactants and 9 Na in the products = Not balanced
e. Sn + 4HNO₃ → SnO₂ + 4NO₂ + 2H₂O
Here we have equal number of products and reactants = Balanced chemcal reaction equation.
The element <u>Oxygen</u> is always present in a combustion reaction.
Answer:
Honestly, I'm not even sure what the incorrect student was trying to do. The correct answer is:
( ) = the number of elements
(1)N2 and (3)H2
I think the student added the N2 and H2 to "balance" the chemical equation when instead they should have tried the balance the equation by making sure the atoms on the reactant side are equal to the atoms on the product side. You do this by multiplying the atoms on the reactant side until they equal the product side (not by adding them, as the student did).
Explanation:
The given data is as follows.
Molecular weight of azulene = 128 g/mol
Hence, calculate the number of moles as follows.
No. of moles = 
= 
= 0.0030625 mol of azulene
Also, 
Now, putting the given values as follows.
= 11748.67 J
So, 
= 1886.4 J
Therefore, heat of reaction will be calculated as follows.
= (11748.67 + 1886.4) J
= 13635.07 J
As,
13635.07 J = 
dE = 
= 4452267.75 J/mol
or, = 4452.26 kJ/mol (as 1 kJ = 1000 J)
Thus, we can conclude that 
for the given combustion reaction per mole of azulene burned is 4452.26 kJ/mol.
I'm assuming false but really have no clue
