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The solubility of michael amine is 25 ° C. The temperature is 8.49 times higher in water than in chloroform. Determine the percentage of base remaining in the following cases in 1000 ml, chloroform. (a) Four times, 200 ml each time. Extraction from water. (b) Extraction from 400 ml of water twice, each time. (c) Extraction from 800 ml of water once.
The distribution of iodine between carbon tetrachloride and water is constant. The value of K is cccl4 / cH2o = 85. How many ml of carbon tetrachloride would be required to extract 95% iodine from 100 ml of aqueous solution in a single phase?
The distribution of iodine between carbon tetrachloride and water is constant. The value of K is cccia / cH2o = 85. How many ml of carbon tetrachloride would be required to extract 959% iodine from 100 ml of aqueous solution in a single phase?
25 ° C. An aqueous solution of iodine containing 0.0516 g liter at temperature 4: 412 g liter containing CCL, is in equilibrium with the solution. 25 C If the solubility of iodine in water at temperature is 0.34 g liter-1, multiply its solubility in cc.
The solubility of michael amine is 25 ઈ C. The temperature is 8.49 times higher in water than in chloroform. Determine the percentage of base remaining in the following cases in 1000 ml, chloroform. (a) Four times, 200 ml each time. Extraction from water. (b) Extraction from 400 ml of water twice, each time. (c) Extraction from 800 ml of water once.
25 ° C. An aqueous solution of iodine containing 0.0516 g liter at temperature 4: 412 g liter containing CCL, is in equilibrium with the solution. 25 C If the solubility of iodine in water at temperature is 0.34 g liter-1, multiply its solubility in cc.
A current of 1.50A was passed through an electrolytic cell containing AgNO3 solution with inert electrodes. The weight of Ag deposited was 1.50g . How long did the current flow? (Given: Ag = 108; N = 14; O = 16; F = 96500 C/mol)
Consider the data presented from the following reaction: A(g) —> B(g):
time(sec): 0, 40, 80, 120, 160
[A](moles/liter): .100, .067, .045, .030, .020
a) determine if the reaction is of the 1st order or 2nd order using the appropriate data and graphs.
b) what is the value of the rate constant.
c) what is half-life of the reaction.
If the total air pressure is 1.05 atm, the partial pressure of carbon dioxide is 0.08 atm, and the partial pressure of hydrogen sulfide is 0.05 atm, what is the partial pressure of the remaining air?
The activation energy of a reaction is 22.5 k Cal mol-1 and the value of rate constant at 40°C is 1.8 ×10−5 s−1. Calculate the frequency factor, A.
