Name How Much is Too Much? Partner\'s Name Exp #6 Post-Laboratory Questions (Pag

Question

Name How Much is Too Much? Partner's Name Exp #6 Post-Laboratory Questions (Page 5 of 5) 8. Ca lculate the percent zinc in your sample using the Dalton's Law of Partial Pressure and the Ideal Gas Law. Show all calculations to receive full credit. What are the gases present in the inverted graduated cylinder? a. gas and wattr vapor ort re Write the equation to calculate the pressure of H2tg) in the graduated cylinder using Dalton's Law. b. Calculate the pressure of Hatg) using the equation in part b. c. Assuming that hydrogen gas exhibits ideal gas behavior, calculate the mass percent zinc in the mixture using your experimental data and the calculated pressure of H2(g) gas from part c. d. Compare the percent zinc calculated using R3 to the calculated value using gas laws above. Which is a more accurate method for determining the percent zinc in the mixture? e.

Explanation / Answer

B). Eqation to calculate the pressure of H2(g) in the graduated cylinder using Dalton’s Law is -

                                       Ptotal = P_H2 + P_H2O

C). Calculate the pressure of H2(g) using the equation in part b:-

735 = x + 15      

                                         x = 720 mmHg

D). Assuming that hydrogen gas exhibits ideal gas behavior, calculate the mass percent zinc in the mixture using your experimental data and the calculated pressure of H2(g) gas from part c :-

    use reaction PV = nRT to get moles of H2

     (720/760) (0.400) = (n) (0.08206) (288)

   n = 0.0160345 mol

reaction:-

      Zn + 2HCl ---> ZnCl2 + H2

      Zn to H2 molar ratio is 1 to 1.

      This means 0.0160345 mol of Zn was consumed.

      0.0160345 mol times 65.409 g/mol = 1.049 g of Zn in sample.

Mass percent zinc ---> (1.049 g / 1.500 g) * 100 = 69.9%

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