Pre-Laboratory Assignment 1. A student following the procedure described in this

Question

Pre-Laboratory Assignment 1. A student following the procedure described in this module collected the following data: 0.0243 mass Mg, g initial syringe volume, ml. final syringe volume, ml barometric pressure, torr temperature, K 1.0 26.5 754 298 Calculate the gas law constant. answer 2. What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K? Use the value for R found in Pre-Laboratory Assignment 1. answer 3. The results of this experiment are greatly affected by the care with which each of the steps is completed. (1) Describe the error that would occur if the magnesium were to slide into the HCl in the test tube before the system is sealed off.

Explanation / Answer

Moles of Mg = 0.0243 g/ 24 g/mol = 0.001 moles

Volume = 26.5-1 mL. = 25.5 mL = 0.0255 L

Pressure = 754/760 atm

Temperature = 298 K

R = PV/nT

= 754 x0.0255 L / (760*0.001*298)

= 0.0849 L atm/mol K

2)

Volume = nRT/P = 0.01 moles x 0.0849 x 298 K *760 /(750)

= 0.256 L

According to Chegg rules only one question should be answered .pls post remaining questions separately

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