A student investigated the stoichiometry of the reaction of zinc (Zn) with HCI solutionand reported the following data: When 0.2158 g of Zn reacted with 10.00 mLof 1.000M HCI, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 102MNaOH solution was required to titrate the HCI remaining in the reaction mixture atthe end of the reaction. The room temperature was 27.0°C and the barometricpressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol The density ofwater at 27.0 °C is 0.9965 g mLand its vapor pressure is 27.0 torr. R = 8.21 X 10 --1atm K-1 mol 1Calculate the number of millimoles of Zn reacting

Given, mass of Zinc = 0.2158 g volume of HCl = 10 mL concentration of HCl = 1.00 M mass of water…

A student investigated the stoichiometry of the reaction of zinc (Zn) with HCI solution and reported the following data: When 0.2158 g of Zn reacted with 10.00 mL of 1.000M HCI, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 102M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol 1. The density of water at 27.0 °C is 0.9965 g mL and its vapor pressure is 27.0 torr. R = 8.21 X. 102 L- atm K1 mol 1 Calculate the number of millimoles of Zn reacting

A student investigated the stoichiometry of the reaction of zinc (Zn) with HCI solution and reported the following data: When 0.2158 g of Zn reacted with 10.00 mL of 1.000M HCI, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 102M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol 1. The density of water at 27.0 °C is 0.9965 g mL and its vapor pressure is 27.0 torr. R = 8.21 X. 102 L- atm K1 mol 1 Calculate the number of millimoles of Zn reacting

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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Questions in bold A student investigated the stoichiometry of the reaction of zinc (Zn) with HCl solution and reported the following data. When 0.2158 g of Zn reacted with 10.00 mL of 1.000M HCl, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 10-2M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol-1. The density of water at 27.0 °C is 0.9965 g mL-1 and its vapor pressure is 27.0 torr. R = 8.21 X 10-2 L-atm K-1 mol-1 a) determine the volume of the water displaced. = 0.08235L b) Calculate the pressure of the H2 collected. = 750 torr c) Calculate the number of moles of H2 collected, using the ideal gas equation. = 0.0033 mol d) Calculate the number of moles of HCl originally present in the reaction flask. e) Calculate the number of moles of HCl remaining in the flask at the end of the reaction. f)…
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Questions in bold A student investigated the stoichiometry of the reaction of zinc (Zn) with HCl solution and reported the following data. When 0.2158 g of Zn reacted with 10.00 mL of 1.000M HCl, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 10-2M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol-1. The density of water at 27.0 °C is 0.9965 g mL-1 and its vapor pressure is 27.0 torr. R = 8.21 X 10-2 L-atm K-1 mol-1 a) determine the volume of the water displaced. = 0.08235L b) Calculate the pressure of the H2 collected. = 750 torr c) Calculate the number of moles of H2 collected, using the ideal gas equation. = 0.0033 mol d) Calculate the number of moles of HCl originally present in the reaction flask. e) Calculate the number of moles of HCl remaining in the flask at the end of the reaction. f)…
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