This graph shows the concentration of the reactant a in the reaction a→b.

determine the average rate of the reaction between 0 and 10 seconds.

0.007 m/s
0.014 m/s
0.86 m/s
0.07 m/s

0.014 M/s

Explanation:

The rate of a reaction depends on the concentration of a particular compound and it stoichmetry coefficient. For the reaction:

aA + bB → cC +dD

The rate can be calculated:

r = -(1/a)xΔ[A]/Δt = -(1/b)xΔ[B]/Δt = (1/c)xΔ[C]/Δt = (1/d)xΔD/Δt

The minus signal for the reagents its because they are being consumed, so Δ[A] and Δ[B] will be negative, and r must be positive. Δt is the time variation.

So, for the reaction given, in t = 0, [A] =1 M, and in t= 10s, [A] = 0.86 M, then

Δ[A] = -0.14 M

r = -(Δ[A]/Δt)

r = -(-0.14/10)

r = 0.014 M/s

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:

a electronegativity decreases beacuse the size of nucleus is bigger.