We use cookies to give you the best experience possible. By continuing we’ll assume you’re on board with our cookie policy

Determination of the molar volume of hydrogen gas Essay

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

We will write a custom essay sample on Determination of the molar volume of hydrogen gas specifically for you
for only $16.38 $13.9/page

Order now

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 � 0.0001)

Room temperature: 21.9 �C (uncertainty is � 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 �1) V2 = 59cm3 (uncertainty is �0.5)

T1 = 21.9 �C = 294.9 K (uncertainty is �1.3466 ) T2 = 0 �C = 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 �C 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.

How to cite this page

Choose cite format:

Determination of the molar volume of hydrogen gas. (2017, Nov 17). Retrieved from https://studymoose.com/determination-of-the-molar-volume-of-hydrogen-gas-essay

We will write a custom essay sample onDetermination of the molar volume of hydrogen gasspecifically for you

for only $16.38 $13.9/page
Order now

Sorry, but copying text is forbidden on this website. If you need this or any other sample, we can send it to you via email.

By clicking "SEND", you agree to our terms of service and privacy policy. We'll occasionally send you account related and promo emails.

Our customer support team is available Monday-Friday 9am-5pm EST. If you contact us after hours, we'll get back to you in 24 hours or less.

By clicking "Send Message", you agree to our terms of service and privacy policy. We'll occasionally send you account related and promo emails.
No results found for “ image
Try Our service