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Answer:
Zero order
Explanation:
Looking at the data we can note a linear dependence between concentration and time.
Time Conc.
0 2
15 1.82
30 1.64
48 1.42
75 1.10
In the first 15 min it was consumed 2-1.82=0.18. So the rate is
From 15 to 30 min (it has passed 15 min) is consumed 1.82-1.64=0.18, so as in the previous calculation the rate is .
From 30 to 48 (it has passed 18 min)the rate is
From 48 to 75 (it has passed 27 min) the rate is
So these results suggest that despite of the ever minor concentration of the reactant the rate is ever the same. Hence the reaction rate could be expressed as that is, the reaction is the zero order respect to C2H5I since it is not depending on concentration of C2H5I.
Answer:
Explanation:
In order to answer this question, we need to be familiar with the law of freezing point depression. The law generally states that mixing our solvent with some particular solute would decrease the freezing point of the solvent.
This may be expressed by the following relationship:
Here:
is the change in the freezing point of the solvent given its initial and final freezing point temperature values;
is the van 't Hoff factor (i = 1 for non-electrolyte solutes and i depends on the number of moles of ions released per mole of ionic salt);
is the freezing point depression constant for the solvent;
is molality of the solute, defined as a ratio between the moles of solute and the mass of solvent (in kilograms).
We're assuming that you meant 1.7-molal solution, then:
Given ethylene glycol, an organic non-electrolyte solute:
The freezing point depression constant:
Initial freezing point of pure water:
Rearrange the equation for the final freezing point and substitute the variables: