Nitrosyl bromide decomposes by the reaction 2 NOBr(g) → 2 NO(g) + Br2(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. A zero-order reaction is linear when [NOBr] on the y-axis. A first-order reaction is linear when ln[NOBr] is on the y-axis. A second-order reaction is linear when 1/[NOBr] is on the y-axis. t 0 5 10 15 50 85 s [NOBr] 0.0653 0.0514 0.0424 0.0361 0.0177 0.0117 M What is the rate law for the reaction? (Rate equations take the general form 'rate = k . [A] . [B]'.) chemPadHelp rate = k. [NOBr]2 rate = k. [NOBr]^2 Correct. What is the value of the rate constant at the temperature of the experiment? WebAssign will check your answer for the correct number of significant figures. 0.830 Incorrect: Your answer is incorrect.

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:

the maximum mass of nh3 is nh3 in grams