Answer:
C₅H₈N₂O
Explanation:
The molecular formula denotes the various forms of atoms contained in a molecule at a particular fixed proportion.
The molecular ion M⁺ = 112.0499
and the exact mass values are given as follows:
C = 12.000
H = 1.0078
N = 14.003
O = 15.995
By assumption:
C = 12.000 × 5 = 60.0000
H = 1.0078 × 8 = 1.0078
N = 14.003 × 2 = 28.0060
<u>O = 15.995 × 1 = 15.9950 </u>
<u> = 112.0634 </u>
This is approximtely equal to 112.0499.
As such the Molecular formula for the compound = C₅H₈N₂O
<h3>
Answer:</h3>
Ag⁺(aq) +Cl⁻(aq) → AgCl(s)
<h3>
Explanation:</h3>
The questions requires we write the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate.
<h3>Step 1: Writing a balanced equation for the reaction.</h3>
- The balanced equation for the reaction between aqueous potassium chloride and aqueous silver nitrate will be given by;
KCl(aq) + AgNO₃(aq) → KNO₃(aq) +AgCl(s)
- AgCl is the precipitate formed by the reaction.
<h3>Step 2: Write the complete ionic equation.</h3>
- The complete ionic equation for the reaction is given by showing all the ions involved in the reaction.
K⁺(aq)Cl⁻(aq) + Ag⁺(aq)NO₃⁻(aq) → K⁺(aq)NO₃⁻(aq) +AgCl(s)
- Only ionic compounds are split into ions.
<h3>Step 3: Write the net ionic equation for the reaction.</h3>
- The net ionic equation for a reactions only the ions that fully participated in the reaction and omits the ions that did not participate in the reaction.
- The ions that are not involved directly in the reaction are known as spectator ions and are not included while writing net ionic equation.
Ag⁺(aq) +Cl⁻(aq) → AgCl(s)
Answer:
False
Explanation:
The first reaction is;
NO(g) + 1/2O2(g) ---->NO2(g)
K= [NO2]/[NO] [ O2]^1/2
The second reaction is;
2NO(g) + O2(g) ---->2NO2(g)
K'= [NO2]^2/[NO]^2 [O2]
It now follows that;
K'= K^2
Hence the statement in the question is false
