Which is not true regarding reaction rates? (2 points)
1 answer:
Let us consider each statement one by one
a) Catalysts are the substance which alter the reaction pathway where activation energy of reaction is less that the un catalyzed reaction. They are not used up in the reaction . the catalyst is restored in the reaction.
b) As mentioned above, the catalyst speed up reaction by lowering the activation energy
c) During a reaction the reactants are consumed up and products are formed. so there is a decrease in concentration of reactant.
Thus all the above statements are true.
D) the rate of decrease in concentration of reactants depends upon the coefficient of reactant in balanced chemical reaction.
For example
Here the rate of decrease in concentration of hydrogen will be double the rate of decrease in concentration of oxygen.
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Answer:
pH ≅ 4.80
Explanation:
Given that:
the volume of HN₃ = 25 mL = 0.025 L
Molarity of HN₃ = 0.150 M
number of moles of HN₃ = 0.025 × 0.150
number of moles of HN₃ = 0.00375 mol
Molarity of NaOH = 0.150 M
the volume of NaOH = 13.3 mL = 0.0133
number of moles of NaOH = 0.0133× 0.150
number of moles of NaOH = 0.001995 mol
The chemical equation for the reaction of this process can be written as:
1 mole of hydrazoic acid react with 1 mole of hydroxide to give nitride ion and water
thus the new number of moles of HN₃ = 0.00375 - 0.001995 = 0.001755 mol
Total volume used in the reaction = 0.025 + 0.0133 = 0.0383 L
Concentration of =
= 0.0458 M
Concentration of =
= 0.0521 M
GIven that :
Ka =
Thus; it's pKa = 4.72
pH ≅ 4.80