Part 2: Dehydration of a hydrate salt 5. 6. Explain why a change in the mass of the chemical occurred during heating. Cite your data. Was the law of conservation of mass followed in this experiment? What else must be measured to demonstrate that this reaction followed the law of conservation of mass? Cite your data. Part 3: Model kits 7. Which mass difference was bigger: the unbalanced or the balanced? Explain your answer in terms of the law of conservation of mass. 4

Part 2: Dehydration of a hydrate salt 5. 6. Explain why a change in the mass of the chemical occurred during heating. Cite your data. Was the law of conservation of mass followed in this experiment? What else must be measured to demonstrate that this reaction followed the law of conservation of mass? Cite your data. Part 3: Model kits 7. Which mass difference was bigger: the unbalanced or the balanced? Explain your answer in terms of the law of conservation of mass. 4

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 70E: You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into...

See similar textbooks

Similar questions

You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.
The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry textbook estimates that if 1.00 × 108 tons Mg were taken out of the sea each year, it would take one million years for the Mg concentration to drop to 0.12%. Do sufficient calculations to either verify or refute this statement. Assume that Earth is a sphere with a diameter of 8000 mi, 67% of which is covered by oceans to a depth of 1 mi, and that no Mg is washed back into the oceans at any time.
(For Exercises 4546) Solutions containing nickel(II) ion are usually bright green in color. When potassium hydroxide is added to such a nickel(II) solution, a pale-green fluffy solid forms and settles out of the solution. The fact that a reaction takes place when potassium hydroxide is added to a solution of nickel(II) ions is an example of a properly. . The fact that a solution of nickel(II) ion is bright green is an example of a property.
What does it mean to say an equation is balanced? Why is it important for an equation to be balanced?
What is true about the chemical properties of the product? a. The properties are more like chemical A. b. The properties are more like chemical B. c. The properties are an average of those of chemical A and chemical B. d. The properties are not necessarily like either chemical A or chemical B. e. The properties arc more like chemical A or more like chemical B, but more information is needed. Justify your choice, and for choices you did not pick, explain what is wrong with them.
A student performed the identical experiment to isolate Fe, NaCl, and SiO2 in a mixture. They performed every step correctly except they extracted with 10 mL of deionized water only once rather than the recommended four times. a.) Will this error make the calculated mass percent of Fe, NaCl, and SiO2 accurate or inaccurate. Explain your answer. b.) Will the calculated mass percents of Fe, NaCl, and SiO2 be higher or lower than the true values? - Mass percent of Fe (HIGHER or LOWER) Must explain answer. - Mass percent of NaCl (HIGHER or LOWER) Must explain answer. - Mass percent of SiO2 (HIGHER or LOWER) Must explain answer.
1000 kg of calcium phosphate is made to react with 10% excess silica, SiO2 and 90% excess carbon to produce 100 kg of phosphorous. The other products are calcium silicate and carbon dioxide. a) What is the degree of completion of the reaction?b) Illustrate the Law of Conservation of Mass.
The mineral iron pyrite (FeS2), typically, has a mass percentage of what is known as fool’s gold of 90-95%. The actual percentage in a sample can be determined using gravimetric analysis. To find the % mass of FeS2 the sulphur in FeS2 is firstly converted to sulphate (SO42-). These sulphate ions (SO42-) is mixed with an excess of barium chloride (BaCl2) to form barium sulphate (BaSO4), according to the following reaction: Ba2+(aq) + SO42- (aq) à BaSO4 (s) When the reaction has gone to completion, the BaSO4 precipitate is collected in a filter paper and carefully washed. The filter paper and its contents are then transferred to a crucible. The crucible and its contents are heated until constant mass is achieved. The data for the analysis of a mineral sample is shown in the table below: Initial Mass of mineral sample 17.5 g Mass of crucible and filter paper 144.60 g Mass of crucible, filter paper and dry BaSO4 196.89 g Molar mass…
You are asked to weigh 2 g of lithium and add it to 1500 ml of distilled water +2drops of indicator, knowing that the density of water is 1 at room temperaturewhile conducting this experiment. -a-What does stoichiometry mean?-b-Is it safe to conduct this experiment in the lab, and why ?-c-‘Describe the characteristic features of the Li that are reflecting its group,and name the group, and determine its density. -d-What indicator will you add in the water and what will happen in thecolor of the water after adding the 2 g of Li? Explain your answer.
What is the same on the left and the right side of a balanced chemical equation? Which scientific LAW does this related to (e.g. Conservation of Energy, Conservation of Matter, etc.)
What is the mass of H2SO4 in a 48.1 cm3 sample of concentrated sulfuric acid that has a density of 1.84 g/cm3? Assume that the Sulfuric acid solution has a 98.3% of mass to mass percentage.
A student attempted to identify an unknown compound by the method used in this experiment. She found that when she heated a sample weighing 0.4862 g, the mass barely changed, dropping to 0.4855 g. When the product was converted to chloride, the mass went up to 0.5247 g. A. Is the sample a carbonate? ________ B. What are the two compounds that might be in the unknown? ______________ or ___________ C. Write the balanced chemical equation for the overall reaction that occurs when each of these two original compounds is converted to a chloride. If the compound is hydrogen carbonate, use the sum of Reactions 1 and 2. If the sample is a carbonate, use Reaction 2. Write the equation for sodium salt and then for potassium salt. D. How many moles of the chloride salt would be produced from one mole of original compound? _____________