Determination of the molar volume of hydrogen gas Essay Example for Free

Determination of the molar good deal of hydrogen bollocks up showIntroductionWe are going to determine the molar volume of hydrogen gas by allow known amount of magnesium react with dilute hydrochloric acid and carefully collecting the gas formed.Materials accelerator syringeHydrochloric acid, 2-molar8 cm of magnesium ribbonRulerEmery clothFor details see counselling formMethodsWe connect the equipment according to the diagram and make sure we follow the affirmations carefully, and then we push the 8 cm of magnesium ribbon and pour the HCl into the test tube. As we are ready to incur 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 crucial to wait for the reaction to finish completely so that the equipment returns back to room temperature. For details see instruction form.ResultsMeasured weigh of 8 cm mg ribbon 0.068 g (uncertainty is 0.0001) li ve temperature 21.9 C (uncertainty is 0.1)Room oblige 742.5 mmHgVapour pressure of water 19.587 and 19.827Vapour pressure 19.587 + 19.827 / 2 = 19.7071.333 x 102 x (mmHg) = PaConvert the room pressure in mmHg into Pa742.5 x 1.333 x 102 = 98975.25 PaConvert the desiccation pressure of water into Pa19707 x 1.333 x 102 = 2626.9431p(H2O) = 2626.9431 PaRoom pressure (Pa) Vapour pressure of water (Pa)98975.25 Pa 2626.9431 Pa = 96348.3069 Pap(H2) = 96348.3069 Pap(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 atmosphereP1 x V1 / T1 = P2 + V2 / T21 atm = 1.013 x one hundred fiveP1 = 96348.3069 P2 = 1 atm = 101300V1 = 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 K96348.3069 x 70 x 1 / 294.9 = 101300 x 59 x 0.5 / 273Conclusion EvaluationOur conclusion is that the molar volume of hydrogen gas at 0 C and 1 atmosphere is -.We reached the concl usion by scratch checking the room temperature and barometer pressure. Then we looked up the values for vapour pressure of water at the actual temperature from the flock book of Chemistry and Physics. The full reference is Chemistry for the IB diploloma G. Neuss. Oxford UP, 2001 p.28.