3. Write the balanced net ionic equation for the reaction that occurs when NaCl

ID: 895410 • Letter: 3

Question

3. Write the balanced net ionic equation for the reaction that occurs when NaCl and AgNO3 are mixed.

4. Write the balance net ionic equation for the reaction that occurs when some of your product(sulfur) is added

D. Calculate the theoretical yield of Na2S2O3.5H2O in 0.149 g

E. Calculate the percentage yield of 0.149g

5- Given the reaction A + B -> products, and the following data at 25 degrees celcius

a.Determine the rate law for this hypothetical reaction.

b.Calculate the value of the specific rate constant for this reaction at 25 degrees celcius

c.Calculate the intial rate for (A)o = 0.75 M and (B)o=2.0 M

(A) concentration (B) Concentration Initial Rate M/sec 1.0 1.0 1.0 X 10 ^ - 4 1.0 0.5 5.0 X 10 ^ -5 0.5 0.5 2.5 X 10 ^ -5 0.5 1.0 5.0 X 10 ^-5

3. molecular equation : AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)

net ionic : Ag+(aq) + Cl-(aq) ---> AgCl(s)

4. question not clear

5. a) let rate law be,

rate = k[A]^x[B]^y

with x and y be the order with respect to A and B and k be rate constant

from run 1 and 2, concentration of A is constant,

rate1/rate2 = 1 x 10^-4/5 x 10^-5 = (1/0.5)^y

taking log on both sides,

log(2) = ylog(2)

y = 1

From run 2 and 3, concentration of B is constant,

rate2/rate3 = 5 x 10^-5/2.5 x 10^-5 = (1/0.5)^x

taking log and solving for x,

log(2) = xlog(2)

x = 1

So rate law becomes,

rate = k[A][B]

b. specific rate constant k = rate/[A][B]

k = 1 x 10^-4/(1 x 1) = 1 x 10^-4 M-1s-1

c. Initial rate = 1 x 10^-4 (0.75)(2.0) = 1.5 x 10^-4 M/s

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