Question

Section - Date Name Lab Partner DATA Trial Mass of Mg (g) - 0.0301 3 Temperature (°C) Volume of H, gas (mL) 30.1 Barometric Pressure (mmHg)_latm 349 38.6 lamm CALCULATIONS A. Experimental Determination of the gas constant, R 1. Write the balanced chemical equation for the reaction between magnesium and hydrochloric acid 2. How many moles of Mg were consumed? 3. Based upon the chemical equation how many moles of H, gas were produced? 4. What volume of H, gas was produced? 5. What was the temperature of the H, gas if it was in thermal equilibrium with the water? 6. What is the vapor pressure of the water in the tube? mm Hg mm Hg mm Hg 7. Determine the pressure of the dry H, in the tube. atm. atm. atm. 8. Determine the experimental value of R L atm mole K Latm mole K Latm mole K 9. Mean value of R 10. Percent Error

Answer 1

Mgctz 12 2t CL Moleular weight of Mg 24.2 2 o.0373 6 0301 Mam Mars no.of Mous O.o30 o.0273 no.of moles 24.3 2 4.3 Zo.0012 20.001S 3. Based on tre chumcal ole of ldz 1 mo e ot M produces mo le of o.0015 O 0012 moles of Ma my pnodncer 0.0015 prodnces o.o012 Moles moles of Hz of H2 1 mo le of H2 ecepies 1 moles of t2 : 22. L of C afstP z 22.4 L of o.0015 mno Les of t2 0 DO12 mm les of 1f 2 22.4xo.o01s 2 22-4xo-o O12 Lof 42 0.033G =0.0269 LOf H2