Which of the following deviations from the experiment could cause a decrease in the calculated mass of Mg(s)? a. Incorrectly recording the barometric pressure. b. Using a beaker with a wider diameter. c. Using a eudiometer of different length. d. Not accounting for the vapor pressure of water. Which of the following deviations from the experiment would most considerably cause an increase in the final calculated %yield of the Mg(s)? a. Placing 13.0 mL instead of 10.0 mL of 6.0 M HCI into the eudiometer. b. Immediately reading the volume of gas right after the reaction ceased. Not adding enough water to fill the eudiometer to the brim, leaving a headspace after inverting the eudiometer. С. d. Consciously inserting 15.0 mg of folded Mg ribbon instead of the prescribed 20 to 30 mg into the eudiometer. Which of the following correctly explains why the vapor pressure of water has to be included in the calculations? a. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. b. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor. has to be added to Pdry gas. vapor С. Recap of the Experiment Record Volume of the Place 10.0 Cover the enclosed gas, the height difference Insert folded mL of 6.0 M mouth of the Mg ribbon (approx. 0.02-0.03 g) Add water HCI into a eudiometer with to fill between the water finger and invert into a glass that is 2/3 filled w/ eudiometer eudiometer levels inside and partially filled w/ distilled to the brim. into the outside the eudiometer, eudiometer. and the temperature of water. water. the water outside.
Which of the following deviations from the experiment could cause a decrease in the calculated mass of Mg(s)? a. Incorrectly recording the barometric pressure. b. Using a beaker with a wider diameter. c. Using a eudiometer of different length. d. Not accounting for the vapor pressure of water. Which of the following deviations from the experiment would most considerably cause an increase in the final calculated %yield of the Mg(s)? a. Placing 13.0 mL instead of 10.0 mL of 6.0 M HCI into the eudiometer. b. Immediately reading the volume of gas right after the reaction ceased. Not adding enough water to fill the eudiometer to the brim, leaving a headspace after inverting the eudiometer. С. d. Consciously inserting 15.0 mg of folded Mg ribbon instead of the prescribed 20 to 30 mg into the eudiometer. Which of the following correctly explains why the vapor pressure of water has to be included in the calculations? a. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. b. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor. has to be added to Pdry gas. vapor С. Recap of the Experiment Record Volume of the Place 10.0 Cover the enclosed gas, the height difference Insert folded mL of 6.0 M mouth of the Mg ribbon (approx. 0.02-0.03 g) Add water HCI into a eudiometer with to fill between the water finger and invert into a glass that is 2/3 filled w/ eudiometer eudiometer levels inside and partially filled w/ distilled to the brim. into the outside the eudiometer, eudiometer. and the temperature of water. water. the water outside.
Which of the following deviations from the experiment could cause a decrease in the calculated mass of Mg(s)? a. Incorrectly recording the barometric pressure. b. Using a beaker with a wider diameter. c. Using a eudiometer of different length. d. Not accounting for the vapor pressure of water. Which of the following deviations from the experiment would most considerably cause an increase in the final calculated %yield of the Mg(s)? a. Placing 13.0 mL instead of 10.0 mL of 6.0 M HCI into the eudiometer. b. Immediately reading the volume of gas right after the reaction ceased. Not adding enough water to fill the eudiometer to the brim, leaving a headspace after inverting the eudiometer. С. d. Consciously inserting 15.0 mg of folded Mg ribbon instead of the prescribed 20 to 30 mg into the eudiometer. Which of the following correctly explains why the vapor pressure of water has to be included in the calculations? a. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. b. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor. has to be added to Pdry gas. vapor С. Recap of the Experiment Record Volume of the Place 10.0 Cover the enclosed gas, the height difference Insert folded mL of 6.0 M mouth of the Mg ribbon (approx. 0.02-0.03 g) Add water HCI into a eudiometer with to fill between the water finger and invert into a glass that is 2/3 filled w/ eudiometer eudiometer levels inside and partially filled w/ distilled to the brim. into the outside the eudiometer, eudiometer. and the temperature of water. water. the water outside.
Hi! I need answers on these multiple-choices questions. The recap of the experiment can be seen below. This experiment is about testing the Ideal Gas Law.
Transcribed Image Text:Which of the following deviations from the experiment could cause a decrease in the calculated mass of
Mg(s)?
a. Incorrectly recording the barometric pressure.
b. Using a beaker with a wider diameter.
c. Using a eudiometer of different length.
d. Not accounting for the vapor pressure of water.
Which of the following deviations from the experiment would most considerably cause an increase in the
final calculated %yield of the Mg(s)?
a. Placing 13.0 mL instead of 10.0 mL of 6.0 M HCI into the eudiometer.
b. Immediately reading the volume of gas right after the reaction ceased.
Not adding enough water to fill the eudiometer to the brim, leaving a headspace after inverting
the eudiometer.
С.
d. Consciously inserting 15.0 mg of folded Mg ribbon instead of the prescribed 20 to 30 mg into the
eudiometer.
Which of the following correctly explains why the vapor pressure of water has to be included in the
calculations?
a. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by
water in the aqueous solution, effectively decreasing the measured pressure above.
b. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor,
thus Pwater
Some of the liquid water evaporates into the gas, and increases the total pressure generated by
the trapped gas.
d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the
contribution of partial pressure of water vapor.
has to be added to Pdry gas.
vapor
С.
Transcribed Image Text:Recap of the Experiment
Record Volume of the
Place 10.0
Cover the
enclosed gas, the
height difference
Insert folded
mL of 6.0 M
mouth of the
Mg ribbon
(approx.
0.02-0.03 g)
Add water
HCI into a
eudiometer with
to fill
between the water
finger and invert
into a glass that
is 2/3 filled w/
eudiometer
eudiometer
levels inside and
partially filled
w/ distilled
to the brim.
into the
outside the eudiometer,
eudiometer.
and the temperature of
water.
water.
the water outside.
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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