Determining the same mass of solute
Mass of solvent=134.4 g/mol
The same mass of solute is dissolved in 9.82 g of t-butanol instead of cyclohexane. What is the expected freezing pt. change of this solution?
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680 mL of a solution of unknown concentration is diluted to a final volume of 1700 mL where the concentration is found to be 1.2 M. What was the initial molarity
An equilibrium mixture of SO2, O2, and SO3 at a high temperature contains the gases at the following concentrations: [SO2] = 3.77 x 10^-3 mol/L, [O2] = 4.30 x 10^-3 mol/L, and [SO3] = 4.13 x 10^-3 mol/L. Calculate the equilibrium constant, Kc for
Assume that the ?Ho and ?So of vaporization do not change significantly with temperature. Calculate the vapor pressure of CH3OH at 70 oC (in atm).
How is it possible for temperatures below the ice to be actually warmer than surface temperatures
Calculate the pH of a solution made by dissolving 2.89 g of sodium fluoride and 17.1 mL of 0.309 M hydrofluoric acid in enough water to make 177 mL of solution.
How many grams of ammonia gas would be formed when 11.2 Liters of hydrogen gas at STP reacts with 4.72 Liters of nitrogen gas? Be sure to determine which reagent is the limiting reagent to determine the theoretical amount of ammonia possible.
Consider the reaction. N2(g) + O2(g) --> 2NO(g) How many moles of NO are obtained when 0.029 mol of N2 is completely reacted
A solid hydrate weighing 2.691g was heated to drive off the water. A solid anhydrous residue remained, which weighed 2.259g. Calculate the per cent water in the hydrate. If the anhydrous residue has a formula weight of 282
What happened when CaCO3 was combined with hydrochloric acid? was a chemical reaction obvious here ? what about NaOH added to HCl? Was a reaction obvious in this case? Why indicators are important to tell if an acid-base reaction has occurred.
The temperature of the water rose from 25.00 degree C to 28.21 degree C. Assuming all the heat from the metal was transferred to the water, calculate the specific heat of the metal.
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