Answer:
Explanation:
To solve this problem, we need to obtain the number of moles of the solute we desired to prepare;
Number of moles = molarity x volume
Parameters given;
volume of solution = 500mL = 0.5L
molarity of solution = 0.5M
Number of moles = 0.5 x 0.5 = 0.25moles
Now to know the volume stock to take;
Volume of stock =
molarity of stock = 4M
volume = = 0.0625L or 62.5mL
Answers:
<em><u>a. Moles of oxygen formed:</u></em><u> 0.670 mol</u>
<em><u>b. Moles of water formed:</u></em><u> 1.34 mol</u>
<em><u>c. Mass of water formed:</u></em><u> 24.1 g</u>
<em><u>d. Mass of oxygen formed:</u></em><u> 21.4 g</u>
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Explanation:
Dihdyrogen dioxide is the chemical name for a compound made of two hydrogen atoms and two oxide atoms, i.e. H₂O₂, which is also known as hydrogen peroxide or oxygenated water.
The decomposition reaction of dihydrogen dioxide into water and oxygen gas is represented by the balanced chemical equation:
The mole ratios derived from that balanced chemical equation are:
<em><u>a. Moles of oxygen formed</u></em>
When you solve for x, you get:
<u />
<em><u>b. Moles of water formed</u></em>
When you solve for x, you get:
<em><u>c. Mass of water formed</u></em>
Using the number of moles of water calculated in the part b., you calculate the mass of water formed, in grams, using the molar mass of water:
⇒ mass in grams = number of moles × molar mass
⇒ mass in grams = 1.34 mol × 18.015 g/mol = 24.1 g
<em><u>d. Mass of oxygen formed</u></em>
Using the number of moles of oxygen determined in the part a., you calculate the mass in grams using the molar mass of O₂.