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-1a) determine the volume of the water displaced. = 0.08235Lb) Calculate the pressure of the H2 collected. = 750 torrc) Calculate the number of moles of H2 collected, using the ideal gas equation. = 0.0033 mold) 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) Calculate the number of moles of HCl reacting.g) Calculate the number of moles of Zn reacting.h) Calculate the ratio of the number of moles of HCl reacting to the number of moles of Zn reacting.i) Calculate the ratio of the number of moles of H2 collected to the number of moles of Zn reacting.j) Write a stoichiometric equation for the reaction of Zn and HCl solution on the basis of the experimental data.

From the experimental data we can see that Zn is reacting with HCl to evolve H2 gas. Hence Zn will…

Answered: Write a stoichiometric equation for the…

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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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^-1and 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) Calculate the number of moles of HCl reacting.

g) Calculate the number of moles of Zn reacting.

h) Calculate the ratio of the number of moles of HCl reacting to the number of moles of Zn reacting.

i) Calculate the ratio of the number of moles of H₂ collected to the number of moles of Zn reacting.

j) Write a stoichiometric equation for the reaction of Zn and HCl solution on the basis of the experimental data.

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