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Taking 100 kg of the 20% feed solution as a basis, draw and label a flowchart of this process labeling both masses and volumes, and do the degree-of-freedom analysis. Calculate the feed ratio (liters 20% solution/liter 60% solution).
Calculate the change in pH when 8.00 mL of .100 M HCl(aq) is added to 100.0 ml of a buffer solution that is 0.100M in NH3(aq) and 0.100M in NH4CL(aq) change in pH=
A first order reaction has a half life of 26.4 sec. How long will it take for the concentration of the reactant to fall to 1/8 of its original value
How do i calculate the volume of SO2 at standard conditions (25 degrees C and 1.00 atm pressure) produced from the heat treatment of 10.00 metric tons of NiS, assuming the reaction goes to completion with 100% conversion of S to SO2
Oxalic acid is a diprotic acid that occurs naturally in some plants. Calculate the pH and the concentrations of all species present in a 0.72-M solution
At equilibrium the total pressure and density of the gaseous mixture were 1.80atm and 1.60g L-1, respectively. Calculate Kc and Kp.
The compound 1-iodododecane is a nonvolatile liquid with a density of 1.20g/ml. the density of mercury is 13.6g/ml. what do you predict for the hight of a barometer column based on 1-iodododecane, when the atmospheric pressure is 752 torr
equilibrium constant-the concentration of solute in the organic phase is in the numerator of the KD expression and the concentration of solute in the aqueous phase is in the denominator.
What is the ph of a solution that is 0.0020 M acetic acid and 0.010 M sodium acetate? Note: the pKb for sodium acetate is 9.25
Metallic magnesium reacts with steam to produce magnesium hydroxide and hydrogen gas. a. If 16.2 g Mg are heated with 12.0 g H2O, what is the limiting reactant?
Organic hydrogenation reactions, in which H2 and an "unsaturated" organic compound combine, are used in the food, fuel, and polymer industries.
how much energy is required to vaporize 98.6 g of ethanol at its boiling point if its Hvap is 40.5 kj/ mol ?
How many molecules of oxygen are produced from the decomposition of 8.75 g of hydrogen peroxide in the following equation Mg + H2O2 --> MgH2 + O2
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