What is the theoretical yield of bismuth when 198 g of bi2o3 reacts with excess carbon as shown below? bi2o3 c(s)> bi(s) + co(g) (not balanced)

179.4306 g

Explanation:

Given that:

Mass of = 198 g

Molar mass of = 465.96 g/mol

The formula for the calculation of moles is shown below:

Thus,

From the balanced reaction,

1 mole of on reaction produces 2 moles of bismuth

So,

0.4293 mole of on reaction produces 2 × 0.4293 moles of bismuth

Moles of bismuth = 0.8586 moles

Molar mass of bismuth = 208.9804 g/mol

So, mass of bismuth = Moles × Molar mass = 0.8586 × 208.9804 g = 179.4306 g

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.