O https://digital.wwnorton.com/8300 93% 02/15/17 This is a Mixed Type question t

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O https://digital.wwnorton.com/8300 93% 02/15/17 This is a Mixed Type question tis worth 4 points/You have unlimited attempts/There is no attempt penalty See page 111 08 Question (4 points) A0.266 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid magnesium oxide. In the laboratory a student weighs the mass of the magnesium oxide collected from this reaction as0.244 g. 2nd attempt See Periodic Table Part 1 (1 point) The 0.266 g solid magnesium is the: Choose one: A. limiting reagent.

Explanation / Answer

first let see the balanced equation

2Mg (s) + O2 (g) -------> 2MgO

moles of Mg = mass / molar mass = 0.266 g / 23.985 g/mol = 0.01109 mol

since he did not mention the quantity of oxy gen we will consider it as excess

so limiting agent is Mg

from the balanced equation it is clear that

1 mole of Mg is producing 1 mole of MgO

accordingly

0.01109 mol of Mg will produce 0.01109 mol of MgO

so theritical mass of MgO = theritical moles x molar mass

= 0.01109 mol x 39.98 g/mol

= 0.4434 g

the actual mass obtained to student is 0.244 g

% of yield = (actual mass / theritical mass) x 100

= (0.244 g / 0.4434 g) x 100

= 55.03%

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