Find the expected mass of calcium carbonate CollectedVolume sodium carbonate (mL)98.0Molarity sodium carbonate (M)0.20Volume calcium chloride (mL)100.0Molarity calcium chloride (M)0.10Observationsprecipitation reaction occurred. As a result, the transparency ofthe liquid became a cloudy white solid.Mass filter paper (g)0.22Mass filter paper + precipitate (g)1.07CalculatedObserved mass calcium carbonate0.85(g)Identify limiting reactantCalcium chlorideExpected mass calcium carbonate(g)Percent yield (%)>

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Collected Volume sodium carbonate (mL) 98.0 Molarity sodium carbonate (M) 0.20 Volume calcium chloride (mL) 100.0 Molarity calcium chloride (M) 0.10 Observations precipitation reaction occurred. As a result, the transparency the liquid became a cloudy white solid. Mass filter paper (g) 0.22 Mass filter paper + precipitate (g) 1.07 Calculated Observed mass calcium carbonate 0.85 (g) Identify limiting reactant Calcium chloride Expected mass calcium carbonate (g) Percent yield (%)

Collected Volume sodium carbonate (mL) 98.0 Molarity sodium carbonate (M) 0.20 Volume calcium chloride (mL) 100.0 Molarity calcium chloride (M) 0.10 Observations precipitation reaction occurred. As a result, the transparency the liquid became a cloudy white solid. Mass filter paper (g) 0.22 Mass filter paper + precipitate (g) 1.07 Calculated Observed mass calcium carbonate 0.85 (g) Identify limiting reactant Calcium chloride Expected mass calcium carbonate (g) Percent yield (%)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.82PAE

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The following is a thought experiment. Imagine that you put a little water in a test tube and add some NaF crystals. Immediately after you add NaF, you observe that the crystals begin dissolving. The quantity of solid NaF decreases, hut before long, it appears that no more NaF is dissolving. The solution is saturated. The equation for the dissolution of NaF in water is NaF(s) —* Na (aq) + F~(aq). As NaF dissolves, what do you think happens to the rate of dissolution? Describe w hat is occurring on the molecular level. Assume that the reverse reaction, Na+(aq) + F“(aq) —* NaF(s), also occurs as the crystal dissolves. In other words, both dissolution and precipitation are taking place. When it appears that there is no more change in the quantin’ of NaF dissolving (the solution is saturated), w hat has happened to the rates of the forward and reverse reactions? Explain your answer.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
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