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How do I calculate the molarity of the solution

How do I calculate the molarity of the solution

Chemistry
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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How do I calculate the molarity of the solution
e of Dioxygen Name Name Separations of Food Dyes by Paper Chromatography 9-1 Date Sources of Error There are two sources of error in this experiment, which fortuitously almost cancel one another. Circle the cor- rect answer in the following statements. (a) Initially the flask that you weigh is filled with air. At the end of the reaction it is filled with oxygen. Because oxygen is denser than air, at the end of the reaction the flask is (heavier, lighter) than it would be if filled with air. (b) If the oxygen that is evolved is saturated with water vapor, some water will be carried over as well as evolved oxygen. At the end of the reaction, this effect would cause the flask to be (heavier, lighter) than if no water were carried over. Calculate the molarity of a solution that is 3.0 % hydrogen peroxide by weight (3 g H2O2/100 g solution), assum- ing that the density of the solution is 1.00 g/mL. For one of your trials, calculate the moles of hydrogen per- oxide that you put in the flask, the moles of oxygen evolved, and the ratio mol O2/mol H2O2. Is the value you calculate for the ratio consistent with the stoichiometry of the decomposition reaction? H₂O2(aq) H₂O(1) + O2(g) eviations from the Ideal Gas Law real gases deviate to some extent from the behavior of perfect gases. At standard conditions, the density o g) is 0.0014290 g/mL, that of H2(g) is 0.00008988 g/mL, and that of CO₂(g) is 0.0019769 g/mL. (a) Using these values and the exact atomic weights, calculate the molar volume of each of these gases, i milliliters, to five significant figures. 02
Transcribed Image Text:e of Dioxygen Name Name Separations of Food Dyes by Paper Chromatography 9-1 Date Sources of Error There are two sources of error in this experiment, which fortuitously almost cancel one another. Circle the cor- rect answer in the following statements. (a) Initially the flask that you weigh is filled with air. At the end of the reaction it is filled with oxygen. Because oxygen is denser than air, at the end of the reaction the flask is (heavier, lighter) than it would be if filled with air. (b) If the oxygen that is evolved is saturated with water vapor, some water will be carried over as well as evolved oxygen. At the end of the reaction, this effect would cause the flask to be (heavier, lighter) than if no water were carried over. Calculate the molarity of a solution that is 3.0 % hydrogen peroxide by weight (3 g H2O2/100 g solution), assum- ing that the density of the solution is 1.00 g/mL. For one of your trials, calculate the moles of hydrogen per- oxide that you put in the flask, the moles of oxygen evolved, and the ratio mol O2/mol H2O2. Is the value you calculate for the ratio consistent with the stoichiometry of the decomposition reaction? H₂O2(aq) H₂O(1) + O2(g) eviations from the Ideal Gas Law real gases deviate to some extent from the behavior of perfect gases. At standard conditions, the density o g) is 0.0014290 g/mL, that of H2(g) is 0.00008988 g/mL, and that of CO₂(g) is 0.0019769 g/mL. (a) Using these values and the exact atomic weights, calculate the molar volume of each of these gases, i milliliters, to five significant figures. 02
The Molar Volume of Dioxygen Name Data Date Locker . Section Instructor_ Data Mass of flask A, contents, stopper, and glass tube before reaction Mass of flask A, contents, stopper, and glass tube after reaction Temperature of the gas in flask A Temperature of the gas in flask D Volume of oxygen collected Barometer reading (temperature of barometer 205 °C) 36 Trial 1 20mc Trial 2 143.40178 140,44118 143.6420 140.07118 24.3 °C 25.0°C °C 22.6 22.1°C °C 318.9mL 279.37 mL 754.70 torr 5.06torr Aqueous vapor pressure at temperature of gas (average the two temperatures) 20.38 torr 21.78 torr Observations 1. Describe the visible changes that take place during the reaction. There is Fizzy when the iron (ni) Chloride reacts with the hydrogen peroxide. There is a visual movement of the water being pushed out und into the beaker. There TS a and then turns at the middle Erlenpuyer Flu dark color initially. a brisht brown 2. As the reaction proceeds, does flask A get warmer or cooler to the touch? Does the reaction absorb or evolve heat (energy)? The flask set warmer as the reaction progress. The reaction. rs relasy heat so it is exothermic
Transcribed Image Text:The Molar Volume of Dioxygen Name Data Date Locker . Section Instructor_ Data Mass of flask A, contents, stopper, and glass tube before reaction Mass of flask A, contents, stopper, and glass tube after reaction Temperature of the gas in flask A Temperature of the gas in flask D Volume of oxygen collected Barometer reading (temperature of barometer 205 °C) 36 Trial 1 20mc Trial 2 143.40178 140,44118 143.6420 140.07118 24.3 °C 25.0°C °C 22.6 22.1°C °C 318.9mL 279.37 mL 754.70 torr 5.06torr Aqueous vapor pressure at temperature of gas (average the two temperatures) 20.38 torr 21.78 torr Observations 1. Describe the visible changes that take place during the reaction. There is Fizzy when the iron (ni) Chloride reacts with the hydrogen peroxide. There is a visual movement of the water being pushed out und into the beaker. There TS a and then turns at the middle Erlenpuyer Flu dark color initially. a brisht brown 2. As the reaction proceeds, does flask A get warmer or cooler to the touch? Does the reaction absorb or evolve heat (energy)? The flask set warmer as the reaction progress. The reaction. rs relasy heat so it is exothermic
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