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13 Dec 2019

My Lab Notes I added 10 mL of water to the flask. I added 10 mL of hydrochloric acid to the flask. I closed the flask. The temperature was 21.5. The pressure was 1.00. The volume of the liquid is 20, so the gas is 130. I put .1 g of magnesium into flask. The pressure went to 1.83 and dropped to 1.76. The temperature went to 34.7 and dropped to 21.6 The volume of the gas is 130.1. After inserting the gas syringe, the volume of the gas in the syringe was 99.5. The new temperature was 21.5. The new pressure was 1.00. The final liquid volume in the flask is 19.9.

Suppose magnesium is the limiting reagent, which of the following chemicals will be found in the flask after the completion of the reaction?

A. magnesium hydride B. hydrochloric acid C. magnesium D. hydrofloudic acid

Why did the solution bubble?

A. Hydrochloric acid gas was released. B. Carbon dioxide gas was produced by the reaction. C. The solution became too hot and the water started boiling. D. Hydrogen gas was produces in the reaction

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Related questions

My Lab Notes

I added 10 mL of water to the flask.
I added 10 mL of hydrochloric acid to the flask.
I closed the flask.
The temperature was 21.5.
The pressure was 1.00.
The volume of the liquid is 20, so the gas is 130.
I put .1 g of magnesium into flask.
The pressure went to 1.83 and dropped to 1.76.
The temperature went to 34.7 and dropped to 21.6
The volume of the gas is 130.1.
After inserting the gas syringe, the volume of the gas in the syringe was 99.5.
The new temperature was 21.5.
The new pressure was 1.00.
The final liquid volume in the flask is 19.9.

Questions:

1. The official molar mass of magnesium is 24.305 g/mol. Based on the number of grams of magnesium added, how many moles of magnesium were consumed? Choose the closest answer

A. 0.00411

B. 0.0411

C 0.0621

D. 0.00621

2. How many moles of hydrochloric acid were added to the flask? To calculate the number of moles of HCl, use the formula below. Choose the closest answer.
n = M × V
where n is the number of moles, M is the molarity of the solution, and V is the volume of the solution in L.

A.0.01 mol

B.0.03 mol

C.0.003 mol

D.0.06 mol

3. What is the limiting reagent for the reaction?

A.magnesium chloride

B.hydrochloric acid

C.magnesium

D.hydrogen

.

1. A 4.00 L flask at 25.0 degrees C contains Argon at a partial pressure of 0.0850 atmosphere. What would be the partial pressure of Argon after we add 1.00 g of Argon gas to the flask without changing the temperature or volume?

2. A 922 mL sample of CH4 gas at 641 torr and a temperature of 125.00 degrees C is compressed at constant temperature to 325 mL. Predict the pressure of the CH4 after this process. (Answer should be in torr)

3. A sample of gas held at constant volume of 5.00 L is cooled from 228 degrees C to -75.0 degrees C. The initial pressure is 805 mmHg. Predict the new pressure.

4. A sample of hydrogen gas was collected over water at 20 degrees C. The toal pressure of gas is 685.0 mmHg. Calculate the partial pressure of H2(g) in atmospheres.

5. What quantity is inversely proportional to the pressure of gas?
A. Speed
B. Atomic mass
C. Volume of gas
D. Formula mass

In this exercise, weighed samples of a solid unknown containing NaCl and NaHCO3react with hydrochloric acid. The volume of the CO2 liberated by the reaction in the gas phase is measured with a gas collection syringe. From the volume we can calculate the number of moles of CO2 in the gas phase using the ideal gas approximation.

Since the CO2 is generated in an aqueous environment (aqueous HCl), some CO2will dissolve in the liquid phase. The amount of CO2 dissolved in the liquid phase is computed using Henry's Law which requires knowing the partial pressure of CO2. As described in the exercise, this requires knowing the entire system gas volume in addition to the initial and final syringe readings.

The entire system gas volume is the sum of the quantities labeled Vtube and Vsyr in the diagram below, corrected for the liquid volume (the aqueous HCl).

Value Units
Gas Constant 0.0821 L-atm/mol K
Absolute Zero (0 K) -273.15 oC
Atmosphere 760.0 Torr
Molar Mass of NaHCO3 84.01 g/mol
Henry's Law Constant for CO2in water 3.2 X 10-2 mol/L-atm

The table below contains the data collected in one run of the reaction between an unknown and hydrochloric acid:

Value Units

Initial Weight of container and unknown

 18.4395 g
Final Weight of container and unknown 18.6185 g
Volume of hydrochloric acid 10.0 mL
Volume of tube, Vtube (see Figure above) 92.3 mL
Initial volume of syringe 5.0 mL
Final volume of syringe 50.7 mL
Temperature 26.5 oC
Pressure 764.4 Torr
Vapor Pressure of Water at 26.5 oC 25.8

Torr

The following questions deal with the above data. The appropriate units are specified in the questions. Pay close attention to the number of significant figures in your answers.

1). What is the volume of CO2 captured in the gas phase (in mL)?

2).What is the number of mmols of CO2 captured in the gas phase? (Remember to account for the vapor pressure of water.)

3). What is the weight of the sample in grams?

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