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# Determination of the molar volume of hydrogen gas Essay

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Introduction

We are going to determine the molar volume of hydrogen gas by letting known amount of magnesium react with dilute hydrochloric acid and carefully collecting the gas formed.

Materials

Gas syringe

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Hydrochloric acid, 2-molar

8 cm of magnesium ribbon

Ruler

Emery cloth

For details see instruction form

Methods

We connect the equipment according to the diagram and make sure we follow the instructions carefully, and then we weigh the 8 cm of magnesium ribbon and pour the HCl into the test tube. As we are ready to start the experiment we fold the mg ribbon on the hook and put the stopper into the test tube so that when we tilt the test tube the mg ribbon can easily fall into the acid. It is important to wait for the reaction to finish completely so that the equipment returns back to room temperature. For details see instruction form.

Results:

Measured weigh of 8 cm mg ribbon: 0.068 g (uncertainty is ï¿½ 0.0001)

Room temperature: 21.9 ï¿½C (uncertainty is ï¿½ 0.1)

Room pressure: 742.5 mmHg

Vapour pressure of water: 19.587 and 19.827

Vapour pressure: 19.587 + 19.827 / 2 = 19.707

1.333 x 102 x (mmHg) = Pa

Convert the room pressure in mmHg into Pa:

742.5 x 1.333 x 102 = 98975.25 Pa

Convert the vapour pressure of water into Pa:

19707 x 1.333 x 102 = 2626.9431

p(H2O) = 2626.9431 Pa

Room pressure (Pa) – Vapour pressure of water (Pa)

98975.25 Pa – 2626.9431 Pa = 96348.3069 Pa

p(H2) = 96348.3069 Pa

p(H2) + p(H2O) = p(room)

2626.9431 + 96348.3069 = 98975.25 p(room)

Calculation of molar volume for hydrogen gas at 0 C and 1 atmosphere

P1 x V1 / T1 = P2 + V2 / T2

1 atm = 1.013 x 105

P1 = 96348.3069 P2 = 1 atm = 101300

V1 = 70 cm3 (uncertainty is ï¿½1) V2 = 59cm3 (uncertainty is ï¿½0.5)

T1 = 21.9 ï¿½C = 294.9 K (uncertainty is ï¿½1.3466 ) T2 = 0 ï¿½C = 273 K

96348.3069 x 70 x 1 / 294.9 = 101300 x 59 x 0.5 / 273

Conclusion & Evaluation:

Our conclusion is that the molar volume of hydrogen gas at 0 ï¿½C and 1 atmosphere is -.

We reached the conclusion by first checking the room temperature and barometer pressure. Then we looked up the values for vapour pressure of water at the actual temperature from the Hand book of Chemistry and Physics. The full reference is: Chemistry for the IB diploloma G. Neuss. Oxford UP, 2001 p.28.

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Hi, I am Sara from Studymoose

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Hi, I am Sara from Studymoose

Hi there, would you like to get such a paper? How about receiving a customized one? Check it out https://goo.gl/CYf83b