Consider the reaction

H2(g) + 1 2 O2(g) → H2O(ℓ) + 286 kJ

How much H2 would have to be burned to yield America’s daily energy share of 260,000 kcal? (1 cal = 4.184 J)

1.) 1900 mol

2.) 3800 mol

3.) 7600 mol

4.) 1 mol

The amount of hydrogen gas consumed is 3800 moles

Explanation:

We are given:

America's daily energy share =    (Conversion factor: 1 kCal = 1000 Cal)

Converting this into Joules, we use the conversion factor:

1 Cal = 4.184 J

So,

For the given chemical equation:

By Stoichiometry of the reaction:

286 kJ of energy is released, when 1 mole of hydrogen is consumed

So, of energy will be released when of hydrogen gas is consumed

Hence, the amount of hydrogen gas consumed is 3800 moles

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.