1. A student following the procedure described in this module collected the following data: mass Mg, g 0.0243 initial syringe volume, mL 1.0 final syringe volume, mL 26.5 barometric pressure, torr 754 temperature, K 298 Determination#1 The value of the gas law constant (R) is 0.0822 L.atm/mol.K Determination #2 he volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K = 248 mL The results of this experiment are greatly affected by the care with which each of the steps is completed (a) Describe the error that would occur if the magnesium were to slide into the HCl in the test tub before the system is sealed off
1. A student following the procedure described in this module collected the following data:
mass Mg, g 0.0243
initial syringe volume, mL 1.0
final syringe volume, mL 26.5
barometric pressure, torr 754
temperature, K 298
Determination#1 The value of the
Determination #2 he volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K = 248 mL
The results of this experiment are greatly affected by the care with which each of the steps is completed
(a) Describe the error that would occur if the magnesium were to slide into the HCl in the test tub before the system is sealed off
(b) What would be the effect on the results of a rise in the room temperature from 22.0 celcius, when determination #1 was done, to 25.3 celcius, when determination #2 was made?
(c) Why must the surface coating of MgO be removed prior to determining the mass of magnesium used in the experiment?
(d) What would be the effect on the results of mistakenly adding 2.43 * 10^-3 g Mg to 4.0mL of 0.1M HCl, rather than to 4.0 mL of 1.0 M HCl as instructed?
(e) If temperature and pressure remain constant, how does the voule of a gas sample vary with the number of moles of gas present?
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