A student, following the procedure described to evaluate the Gas Law Constant, collected the following data in an exercise: mass Mg, g 0.0243 final gas volume, mL 25.0 barometric pressure, torr 754 vapor pressure of H2O at 25 °C 23.76 temperature, K 298 a) The gas collected in the eudiometer is a mixture of hydrogen and water vapor. Calculate the gas law constant. b) What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr (corrected pressure) and 298 K? Use the value of R found in question A
A student, following the procedure described to evaluate the Gas Law Constant, collected the following data in an exercise: mass Mg, g 0.0243 final gas volume, mL 25.0 barometric pressure, torr 754 vapor pressure of H2O at 25 °C 23.76 temperature, K 298 a) The gas collected in the eudiometer is a mixture of hydrogen and water vapor. Calculate the gas law constant. b) What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr (corrected pressure) and 298 K? Use the value of R found in question A
A student, following the procedure described to evaluate the Gas Law Constant, collected the following data in an exercise:
mass Mg, g
0.0243
final gas volume, mL
25.0
barometric pressure, torr
754
vapor pressure of H2O at 25 °C
23.76
temperature, K
298
a) The gas collected in the eudiometer is a mixture of hydrogen and water vapor. Calculate the gas law constant.
b) What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr (corrected pressure) and 298 K? Use the value of R found in question A.
2. 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(aq) in the beaker before the eudiometer is sealed off.
b) What would be the effect on the results of a rise in the room temperature from 21.5℃, when determination #1 was done, to 25.8℃, when determination #2 was made? Assume both experiments were done at a constant temperature.
c) Why must the surface coating of MgO be removed prior to determining the mass of magnesium used in the experiment?
3. If the temperature and pressure remain constant, how does the volume of the gas sample vary with the number of moles of the gas present?
Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
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