Calculate the experimental molar volume (l/mol) for an ideal gas at stp using the information that follows. a 15.0 mg piece of solid magnesium was reacted completely with hydrochloric acid in a reaction flask with a volume of 135 ml. the temperature of the reaction was 22.3 °c and the pressure of the gas produced by the reaction was 11.3 kpa. calculate the volume of hydrogen gas that would have formed in this reaction had it been conducted under standard temperature and pressure conditions (use the combined gas law). use the volume you have just determined, along with the number of moles of hydrogen gas that would have formed from 15.0 mg of magnesium reactant, to calculate the molar volume of this gas at stp

answer: the figure is attached herewith.

step-by-step explanation:   we are given to sketch a unit circle and label the terminal points corresponding to

in the attached figure, we have drawn a unit circle, with centre at o(0,0) and radius 1 unit. we have labelled the points a, b, c, d and e corresponding to the angles below

∠aox = 60°,

∠box = 120°,

∠cox = 180°,

∠dox = 240°,

∠eox = 300°.

and the coordinates are a(0.5,1), b(-0.5,1), c(-1,0), d(-0.5,-1) and e(0.5,-1).

thus, the answer is complete.

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.

the answer is symmetrical : )