Discuss the below:
Erlenmeyer flask contains 0.25g Zn then add 10 mL 6M of HCl then when it cools back down to 21 degrees Celsius connect it to a Gas piston I got these for the pressure O2 moles 0.000524 vol 102.14 N2 0.002096 moles vol 102.14 and nothing for H2
Q1. Record and calculate the following for the first half of the experiment:
(a) Mass of zinc used (g) 0.25g
(b) Moles of zinc used: 0.00382 moles of Zn
(c) Volume of 6M HCl used (mL)
(d) Moles of HCl used: 0.0274 Mole
(e) Molecular weight of zinc (g/mol) 65.39
(f) Moles of zinc reacted:
(g) Moles of hydrogen produced
(h) Molar volume of the ideal hydrogen gas at room temperature (Volume/moles), expressed as L/mol at X degrees C and a pressure of 1 atmosphere
Erlenmeyer Flask contains 0.25 g of Zn then add 20 mL 6M of HCl when it cools back down to 21 degrees Celsius connect it to the Gas piston and the O2 pressure is 0.001159 moles vol. 226.33 and N2 0.004637 vol. 226.33 and nothing for H2
Q2. For the second part of the experiment, everything was the same except that twice as much HCl was used. Record and calculate the following for this second reaction
(a) Mass of zinc used (g) 0.25g
(b) Volume of 6M HCl used (mL)
(c) Molecular weight of zinc (g/mol) 65.39
(d) Moles of zinc reacted:
(e) Moles of hydrogen produced
(f) Molar volume of the ideal hydrogen gas at room temperature (Volume/moles), expressed as L/mol at X degrees C and a pressure of 1 atmosphere
Q3. Compare the molar volumes obtained in the two parts of the experiment.
What difference did using twice the amount of HCl in the second part?
Was all of the zinc used up in the reaction?
Which of the zinc and HCl is the limiting reactant
Q4. Compare the experimental value for the molar volume at 21C with the value listed in the Background section of the lab manual.
Calculate the experimental error according to
% error = | experimental molar volume - listed molar volume | / (experimental molar volume) * 100