I have came up with the molarity of bothsolutions , time, seconds and rate. the

Question

I have came up with the molarity of bothsolutions , time, seconds and rate. the only problem that I am having is how to come up with it in joules and how to plot the graph . it would be nice if u can explain it in details to me . I would really appreciate the help since I'm finding the chapter of kinetics a little difficult for me.. thanks.

1).Effect of Concentration on Rate TABLE M)HS (M) KIO (SEC) H,SO, time c) H2SO3 H2O KIO Total MOLARITY H,SO,IO, Total MOLARITY TIME RATE (MS) TEMP 0.5m-6.5mL 13.0mLU|10mL 0.5mL | 7.5mL | 2.0mL )110mL 0.5mL 8.5mL 1.0mL 10mL 0.5mL 9.0mL o.5mL10mL Xiu 25 rage Temperature 25

Explanation / Answer

This was a iodine clock reaction

IO3 - + 3 H2SO3 = I- + 3 SO4 2- + 6 H+    (the slow step)

The rate law is first order for both reactants

Rate = k[IO3 -][ H2SO3]

Your TIME values look wrong.

In the 1st table replace 39s by 23 s and recalculate rate.

In the 2nd table replace 54 s by 84 s , 105 s by 155 s and recalculate rates.

For each concentration of KIO3 calculate the ratio R1/R2 = k1/k2   (4 values). Calculate the average value for k1/k2.

To simplify, I will suppose you have obtained the average k1/k2=2

The activation energy (Arrhenius law)

Ea = - 8.314 J/mol.K ln 2 / (1/298K – 1/283K)

     = - 5.763J/mol.K / (0.003356 K-1 – 0.003534 K-1) =

     = - 5.763J/mol.K / ( - 0.000178 K-1)

     = 32 400 J/mol = 32.4 kJ/mol

The plot Rate vs [KIO3] is a straight line (plot R1 and R2 as separate lines).

The plot Rate vs Time is also common. I suggest you to plot also Rate vs. 1/t to obtain a line.

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