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Compound Z has a solubility limit of 32.5 g/L in diethyl ether. Compund Z has a solubility limit od 2.5 g/L in water. You are given a 100 mL aqueous solution that contains 200 mL of compund Z. If you do three 33.3 mL extractions of Z using diethyl ether:
1) what is the K value for compound Z in the biphasic system
2) how much do you remove in each individual extraction
3) how much of compoun Z is extracted with each of those 33.3 mL extractions added together
4) how much is still in the water layer at the end of all three extractions?
If 138 mL of wet H2 is collected over water at 24°C and a barometric pressure of 748 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr at 24°C.)
Concentration of Fe(SCN)2+ in calibration Solutions-Recall that the concentration of Fe(SCN)2+ in the calibration solutions is essentially the concentration of SCN- initially in the solution
What is the pH when enough 0.100 base is added to neutralize 8.00 mL of 0.100 M acid? Note: Make simplifying assumptions
Draw a titration curve for both of these peptides. Be sure to label the axes properly, indicate the pKa values, the equivalence points and the buffering regions.
A gaseous hydrocarbon fuel is burned in 26.84% excess oxygen and the exhaust gas analyzed. On a dry basis, the ratio of carbon dioxide to carbon monoxide to oxygen in the exhaust gas
A particular brand of gasoline has a density of 0.737 g/mL. How many grams of this gasoline would fill a 14.4 gal tank?
What is the estimated quantity of energy released in the combustion of methanol?
What are the boiling point and freezing point of a 2.47 m solution of naphthalene in benzene? (The boiling point and freezing point of benzene are 80.1°C and 5.5°C, respectively.
The enthalpy of formation of compound X is -612 kJ/mol, and the sole product of its combustion has a enthalpy of formation of -671 kJ/mol. What is the enthalpy of combustion of compound X?
Nickel nitrate and potassium carbonate react to form nickel carbonate and potassium nitrate. How many milliliters of 0.55M Ni(NO3)¬2 are needed to react with 85 mL of 0.25M K2CO3? First, write a balanced equation.
Calculate E when 900.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
If the reaction is carried out in a 2.0 L container and 0.010 mol of PH3 is consumed each second, what are the rates of production of P4 and H2?
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