Question

With the advent of photosynthesis, the amount of oxygen in the atmosphere has varied over the eons up to 35% by volume, theoretically leading to larger plants and animals. The current concentration is 21% oxygen, 78 % nitrogen, and 1% other gases such as argon and carbon dioxide. Assuming an atmosphere of 31 % oxygen, to the nearest whole number (no decimal) what would be the ideal volume of water (in mL) initially placed in a 50 mL graduated cylinder (assuming the graduation goes up to the lip of the container) for optimal combustion (biggest explosion) if we collected pure hydrogen by displacement gases involved are diatomic, and that equal moles of different ideal gases occupy equal volumes at the same temperature. ? Make sure to account for the stoichiometry of the combustion, that all

Answer 1

page:04 Answen. Given information, the equation of Combustion of water 2H30 - atla + Og, Here, a moles of water giver a moles of Ha and imole of oa. The air contains 31% ca. SO, soma air contains ami of oa. from gas lawe anu 16 og ca : imod orci 22400 ml of.02 Imol og. Iml of oa = wamt of molog. 92000 na 7 mol oa 224oo Hmlof og 20.0003 mol 02. then,

*10 produce 0.0003 mol og we need page:ou. (0.0003 x 2) mol H20 - 0.0006 molligo. : Imol of Hao : 22400ml of H2og. - Won, 0.0006 mol of Hao = (22400 x0.0006 1 ml of Hyo 13. uum Hgo So, the initially will corstairs 13.44 ml of waten(heo).