Answer:
Rate = k [OCl] [I]
Explanation:
OCI+r → or +CI
Experiment [OCI] M I(-M) Rate (M/s)2
1 3.48 x 10-3 5.05 x 10-3 1.34 x 10-3
2 3.48 x 10-3 1.01 x 10-2 2.68 x 10-3
3 6.97 x 10-3 5.05 x 10-3 2.68 x 10-3
4 6.97 x 10-3 1.01 x 10-2 5.36 x 10-3
The table above able shows how the rate of the reaction is affected by changes in concentrations of the reactants.
In experiments 1 and 3, the conc of iodine is constant, however the rate is doubled and so is the conc of OCl. This means that the reaction is in first order with OCl.
In experiments 3 and 4, the conc of OCl is constant, however the rate is doubled and so is the conc of lodine. This means that the reaction is in first order with I.
The rate law is given as;
Rate = k [OCl] [I]
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Answer:
Take the measuring cylinder and measure its mass, in grams, as accurately as possible.
Take the measuring cylinder off the balance and add the water carefully. Put the measuring cylinder back on the balance. Measure and record the new mass .
Repeat the procedure, recording the volume and total mass, until the measuring cylinder is full. Then, for each volume calculate the mass of the liquid alone.Repeat steps 1 to 3 Draw a graph of mass of liquid against volume . Calculate the density of each liquid from the gradient of its graph line.
Explanation:
Answer:
7% 4)2(10
Explanation:
beacouse if you divide it you can get the answer
Answer:
- answer c is the answer
Explanation:
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