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Need help with part B
99 LAB 7 DETERMINATION OF THE MOLAR VOLUME OF A GAS AND THE GAS CONSTANT, R Name Section Date Lab Partner DATA 2 3 Trial 1 Mass of Mg (g) 0-05 Temperature (°C) 20.06 Volume of H, gas (mL) 54.40 Barometric Pressure (mmHg) 746.4 used 1000 ml water 0.0543 20:00 53.90 746-4 CALCULATIONS A. Experimental Determination of the gas constant, R 2 1. Write the balanced chemical equation for the reaction between magnesium and hydrochloric acid. + Mgco + 2HCl > MgCl₂ (94) 20 6x10m 2.23x10 moi -3 2. How many moles of Mg were consumed? mol 3. Based upon the chemical equation how many moles of H, gas were produced? 2.0 6x103 mol 2.23x10 mol mol 4. What volume of H, gas was produced? 0.0541 L 0.054 L 5. What was the temperature of the H, gas if it was in thermal equilibrium with the water? 293.216 K 293-15k K 6. What is the vapor pressure of the water in the tube? 17:54 mm Hg 17.54 mm Hg mm Hg 7. Determine the pressure of the dry H, in the tube. 0-959 atm. 0-0959 atm. atm. 8. Determine the experimental value 0.08b -079 L atm of R Latm mole K mole K L atm mole K 9. Mean value of R 0-08 0-90% 10. Percent Error gjore CamScanner
B. Experimental Determination of molar volume of a gas at STP. 1. Determine the volume of the dry H, gas collected if the gas was at STP. By using equation 2, determine the volume. 2. Determine the volume of dry collected at STP per mole of H, gas. 3. Mean value of molar volume. 4. Percent oror CamScanner