Answer:
1) Rate = K [ClO⁻]²
2) Rate = K [C6H5N2Cl]
3) - Double the concentration of H3PO4.
- Double the concentration of I⁻
4) Check Explanation
Explanation:
A reaction's rate law is written as a product of the reaction's rate constant, k, and the concentration of the respective reactant(s) raised to the power of the order of reaction.
The order of a reaction with respect to a reactant is the power that the concentration of that specific reactant has in the rate law. It shows how dependent on each reactant , the rate of the reaction.
1) 3ClO⁻ (aq) → ClO³⁻ (aq) + 2 Cl⁻ (aq)
Doubling the concentration of ClO⁻ quadruples the initial rate of formation of ClO³⁻. What is the rate expression for the reaction?
Rate = k [ClO⁻]ⁿ
When [ClO⁻] is doubled, Rate is quadrupled, this shows that the reaction is second order with respect to the only reactant.
Rate = K [ClO⁻]²
2. The reaction
C6H5N2Cl (aq) + H2O (l) → C6H5OH (aq) + N2 (g) + HCl (aq) is first order in C6H5N2Cl and zero order in H2O. What is the rate expression?
Normally, the rate of reaction is equal to the rate constant multiplied by the each reactant's concentration raised ti the power of the order, so,
Rate = K [C6H5N2Cl]¹ [H2O]
Rate = K [C6H5N2Cl]
3. For the reaction
H3PO4 (aq) + 3I⁻ (aq) + 2H + (aq) → H3PO3(aq) + I³⁻(aq) + H2O
(l) the rate expression under certain conditions is R = k[H3PO4][I⁻][H⁺]² . What method(s) could be used if you want to double the reaction rate?
Rate = k[H3PO4][I⁻][H⁺]²
Indicating a first order relationship between the rate and the concentration of H3PO4 & I⁻ and second order with respect to H⁺.
So, any attempt to double the rate of reaction will entail a direct doubling of the one of the reactants with a first order relationship with the rate of reaction.
4. What is the overall order of reaction for each of the following.
a) R = k[NO2]² b) R = k c) R = k[H2][Br2] ½ d) Rate = k[NO]² [O2]
Note that overall order of a reaction is the sum of all the orders of the reactants that appear in the rate law.
a) R = k[NO2]²
Overall order is obviously 2.
b) R = k
Overall order is evidently 0.
c) R = k [H2] [Br2]^ ½
Overall order = 1 + ½ = (3/2)
d) Rate = k[NO]2 [O2]
Overall order = 2 + 1 = 3
Hope this Helps!!!
