Be sure to answer all parts. determine the overall orders of the reactions to which the following rate laws apply: (a) rate = k[no2]2 (b) rate = k zero order first order 1.5 order second order 2.5 order third order zero order first order 1.5 order second order 2.5 order third ord

Answer :

(a) The rate of reaction is, second order reaction.

(b) The rate of reaction is, zero order reaction.

Explanation :

Rate of reaction : It is defined as the rate of change in concentration of reactant or product with respect to time.

Order of reaction : It is defined as the sum of the exponents or powers to which the molar concentration in the rate law equation are raised to express the observed rate of reaction.

The order of reaction depends on the power of reactant concentration.

(a) The given rate expression is,

From this expression we conclude that the power of concentration of reactant is 2.  

That means it is a second order reaction.

(b) The given rate expression is,

From this expression we conclude that the rate of reaction is equal to rate constant.

That means it is a zero order reaction.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: