A student following the procedures in this lab exercise collected the following

Question

A student following the procedures in this lab exercise collected the following data: mass Mg, g 0.0243 initial syringe volume, ml. 1.0 final syringe volume, mL 26.5 barometric pressure, torr 75.4 temperature, K 298 Calculate the value of the universal gas constant, R. What would be the volume of hydrogen gas produced by the reaction of 0.0243 g of magnesium metal, collected at 750 ton and 208 K? Use the value of R found in question 1. The results of this experiment are affected by the care with which each step is completed. Describe how each of the following errors would affect the calculated value of R. The Mg slid into the HCl in the test tube before the system was sealed off. The room temperature increased by 3 degree C between the time that the final volume was measured and the temperature was recorded. The MgO coating was not removed before the Mg sample was placed in the HCl. The test tube was filled with 4 mL of 0.10 M HCl instead of 4 mL of 1 M HCl.

Explanation / Answer

Hi,

1. The following data is given,

barometric pressure (P)= 754 torr= 754*133.322 Pa= 100525 Pa

volume occupied= final volume of syringe- initial volume of syringe= 26.5-1.0 ml= 25.5 ml= 25.5*10^-6 m^3

temperature (T)= 298 K

moles of Mg (n)= mass/molecular mass of Mg= 0.0243/24= 1.0125*10^-3

by applying ideal gas equation,

PV=nRT, where R= universal gas constant

R= PV/nT= (100525*25.5*10^-6)/(298*1.0125*10^-3)= 8.49 J / mol. K

Thank you

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