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Value of E: 1.3 g x 1 mole/100.09=1.29 x 10-2 moleCaCO3
Using the value in your answer to question., calculate the number of moles of HCl that two TUMS® tablets can neutralize.
A mixture of CO, CO2 and O2 is contained within a 275 mL ?ask at 0?C. If the total pressure is 780 torr, the CO has a partial pressure of 330 torr and the CO2 has a partial pressure of 330 torr.
Calculate how the amount of AgCl(s )will change when the equilibrium is disturbed by Adding AgNO 3
Determine the value of pH of given solutions that are (a) a solution that is 0.40 M CH3CO2H, (b) a 0.40 M CH3CO2H solution, (c) 0.20 M NaCH3CO2. And explain your answer too?
Metallic magnesium can be made by the electrolysis of molten MgCl2. What mass of Mg is formed by passing a current of 6.40 A through molten MgCl2 for 4.90 days?
In a saturated solution of lead (II) fluoride the concentration of lead was measured to be .0021 M. What is the value of Ksp for PbF2?
What mass of water (in g) would need to evaporate from your skin in order to dissipate 0.8 x 10 5 J of heat from your body?
how much energy is required to vaporize 48.7 g of CH2Cl2 at its boiling point if its Hvap = 31.6 kg/mol
A 4.70 g nugget of pure gold absorbed 278 J of heat. The initial temperature was 28.0°C. What was the final temperature.
if you dissolve the weighed mass of zinc in water which had not been deionized, how would the volume of EDTA required to reach the indicator end-point
Consider that a benzene molecule could fit nicely within a two-dimensional square box with each side having length of 5 degree A. a. Calculate the four lowest energy levels for an electron confined
Calculate the pH of CO2-saturated water at 25 degrees C, given that the CO2 concentration in air is 366 and that for carbon dioxide the Henry's Law constant KH=3.4E-2 mol L-1 atm-1 at 25 degrees C.
Calculate the [H3O+], pH, and the fraction of dissociation (α) in an aqueous 0.140 M NH3 solution. (Hint: You will need the Ka, located in the back of your textbook.)
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