A sample of sulfuryl fluoride, SO2F2, has a mass of 19.2 g. What amount, in moles, does this mass represent?
2 answers:
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Answer:
Explanation:
NO₃⁻ + Sn²⁺ + __ → NO₂ + Sn⁴⁺ + __
Step 1: Separate into two half-reactions.
NO₃⁻ ⟶ NO₂
Sn²⁺ ⟶ Sn⁴⁺
Step 2: Balance all atoms other than H and O.
Done
Step 3: Balance O.
NO₃⁻ ⟶ NO₂ + H₂O
Sn²⁺ ⟶ Sn⁴⁺
Step 4: Balance H
NO₃⁻ + 2H⁺ ⟶ NO₂ + H₂O
Sn²⁺ ⟶ Sn⁴⁺
Step 5: Balance charge.
NO₃⁻ + 2H⁺ + e⁻ ⟶ NO₂ + H₂O
Sn²⁺ ⟶ Sn⁴⁺ + 2e⁻
Step 6: Equalize electrons transferred.
2 × [NO₃⁻ + 2H⁺ + e⁻ ⟶ NO₂ + H₂O]
1 × [Sn²⁺ ⟶ Sn⁴⁺ + 2e⁻]
Step 7: Add the two half-reactions.
2 × [NO₃⁻ + 2H⁺ + e⁻ ⟶ NO₂ + H₂O]
<u>1 × [Sn²⁺ ⟶ Sn⁴⁺ + 2e⁻] </u>
2NO₃⁻ + Sn²⁺ + 4H⁺ ⟶ 2NO₂ + Sn⁴⁺ + 2H₂O
Step 8: Check mass balance.
On the left: 2 N, 6 O, 1 Sn, 4H
On the right: 2 N, 6 O, 1 Sn, 4H
Step 9: Check charge balance.
On the left: -2 + 6 = +4
On the right: +4
The equation is balanced.
Answer :
The rate law expression for zero order reaction will be:
The rate law expression for first order reaction will be:
The rate law expression for second order reaction will be:
Zero order reaction : There is no affect on the rate law.
First order reaction : The rate law becomes doubled.
Second order reaction : The rate law becomes quadrupled.
Explanation :
Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.
The given reaction is:
The rate law expression for zero order reaction will be:
The rate law expression for first order reaction will be:
The rate law expression for second order reaction will be:
Now we have to determine that if doubling of the concentration of A then the rate of reaction will be:
As we know that the zero order reaction does not depend on the concentration of reactant. So, there is no affect on the rate law.
As we know that the first order reaction depend on the concentration of reactant. So, the rate law becomes doubled.
As we know that the second order reaction depend on the concentration of reactant. So, the rate law becomes quadrupled.