eff followed to procedure for Experiment 4, and collected the following data, which he recorded on his "Data and Calculations" sheet: Row A Mass of flask = 97.85 g Row B Mass of flask + unknown = 99.86 g Row C Mass of graduated cylinder + HCl( aq) = 37.470 g Row D Mass of emptied graduated cylinder = 26.941 g Row E Mass of flask containing reaction mixture = 109.55 g 1) What was the mass in grams of Jeff's products, after the reaction was complete ? 2) What was the mass in grams of the CO 2 lost in Jeff's reaction ?

eff followed to procedure for Experiment 4, and collected the following data, which he recorded on his "Data and Calculations" sheet: Row A Mass of flask = 97.85 g Row B Mass of flask + unknown = 99.86 g Row C Mass of graduated cylinder + HCl( aq) = 37.470 g Row D Mass of emptied graduated cylinder = 26.941 g Row E Mass of flask containing reaction mixture = 109.55 g 1) What was the mass in grams of Jeff's products, after the reaction was complete ? 2) What was the mass in grams of the CO 2 lost in Jeff's reaction ?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter6: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 100AE

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Jeff followed to procedure for Experiment 4, and collected the following data, which he recorded on his "Data and Calculations" sheet: Row A Mass of flask = 97.85 g Row B Mass of flask + unknown = 99.86 g Row C Mass of graduated cylinder + HCl( aq) = 37.470 g Row D Mass of emptied graduated cylinder = 26.941 g Row E Mass of flask containing reaction mixture = 109.55 g What was the mass in grams of Jeff's products, after the reaction was complete ?
Patty followed the experimental procedure for Experiment 4 Part 1, and collected the following data. Use this data to calculate the mass of gas produced in Patty’s reaction. A Mass of flask 96.167 g B Mass of flask + unknown 98.108 g C Mass of graduated cylinder + HCl(aq) 37.947 g D Mass of emptied graduated cylinder 27.023 g E Mass of flask containing reaction mixture 108.549 g
Mass of vial + AgNO3 __16.9209g Mass of empty Vial ________6.8951g Mass of copper wire BEFORE the reaction ____4.3168g Mass of copper wire AFTER the reaction _____2.6851g Mass of filter paper __0.7253g Mass of filter paper with dry silver ______6.3254g Calculations: Please do the following three calculations, showing the math set-up for each. Mass of AgNO3 used in reaction (this is the mass of just the AgNO3, without the vial) Mass of copper wire consumed in the reaction (this is the mass of the Cu that was used up in the reaction, NOT the mass of the entire wire) Mass of silver metal produced in reaction (this is your EXPERIMENTAL yield, NOT including the mass of the filter paper)!
Potassium nitrate was synthesized in an experiment using 10 mL of nitric acid and excess potassium hydroxide. The mass data obtained from the experiment is shown in Table 1 below. Given that the percentage yield of potassium nitrate was 88.3 %, calculate the concentration (% m/v) of the nitric acid used in the experiment. Table 1: Mass data for the synthesis of potassium nitrate from nitric acid and potassium hydroxide Mass of clock glass and crystallized potassium nitrate/ g 45.55 Mass of empty clock glass/ g 39.18 I got this question for my exam and didn't know if I did correctly but if I did wrong I would have learn from my mistake
a student finds that they have 0.2929 g of NH4Cl, 0.6234 g of NaCl, and 1.3841 g of SiO2. Calculate the percent gained or lost during this experiment if the initial mass of the mixture was 2.5127 g.
Mercury and bromine will react with each other to produce mercury (II) bromide:a. What mass of HgBr2(s) can be produced from the reaction of 5.00 mL Hg(l) (density = 13.6 g/mL) and 5.00 mL Br2(l) (density = 3.10 g/mL)? ((l) stands for liquid)b. What mass of which reagent is left unreacted?
A 1.6 g sample of a compound is transfered to a 100 mL volumetric flask, filled to the mark with distilled water, and thoroughly mixed. Twenty five milliters of this solution is drawn from the flask using a volumetric pipet, transfered to another 100 mL volumetric flask, and filled to the mark and mixed. The grams of compound in the second volumetric flask is: A. 1.6 B. 1.2 C. 0.80 D. 0.40
You are given a mixture of CuCO3 and CuO. You place the mixture in a crucible and heat it to decompose the CuCO3 into CO2 gas and CuO. You made sure that the CuCO3 had completely decomposed by constantly heating it, cooling it, and weighing it until the mass remains the same. Using the data below from the experiment, calculate the % CuCO3 in the original sample. Mass of empty crucible: 22.19 g Mass of crucible + sample before heating: 23.193 g Mass of crucible + sample at constant mass: 22.851 g PLease show and create one solution map: i made this solution map, is it correct? 1.561g CO2 x (1mol CO2/44.01g CO2) x (1mol CrCO3/1mol CO2) x (112.01g CrCO3/1mol CrCO3)= 3.973g CrCO3 than, (3.973/25.422) x 100% = 15.63% 2.) A 12.622 g sample of a compound that contains sulfur is analyzed by precipitating all the sulfur as BaSO4. If 11.957 g of BaSO4 are obtained in the analysis, what is the percentage of sulfur in the original compound? (Need help with this one too)
A 0.8102 g sample of impure Al2(CO3)3 (MM= 234 g/mol) decomposed with HCl; the liberated CO2 was collected on calcium oxide (CaO, MM = 56 g/mol) and precipitated as CaCO3 (MM =100 g/mol). The precipitated was weigh to 0.0515 g. Calculate the percent of aluminium (atomic mass = 27 amu) in the sample. (Express answer in proper significant figures and do not include units.)
A sample of an iron oxide weighing 14.8 g is heated in a stream of H2(g) until it is completely converted to iron. If the iron produced weighs 10.36 g, the percentage of oxygen in the original oxide must have been: 30.0% None of the following 85.7% 14.3% 70.0% If a 1.000 g mixture of Cu2O and CuO is quantitatively reduced to 0.865 g of Cu then the mass of Cu2O in the original sample of the mixture must have been: 0.742 g 0.258 g None of the following 0.174 g 0.250 g
Aqueous hydrobromic acid HBr will react with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O.Suppose 61. g of hydrobromic acid is mixed with 44.1 g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits. I keep getting this problem wrong because of the sig. digits, dont round till the end because if it is off by 0.1, it will be incorrect.
Mercury and bromine will react with each other to produce mercury (II) bromide:What mass of HgBr2(s) can be produced from the reaction of 5.00 mL Hg(l) (density = 13.6 g/mL) and 5.00 mL Br2(l) (density = 3.10 g/mL)? ((l) stands for liquid)