Answer:
67.5% ≅ 67.6%
Explanation:
Given data:
Mass of water = 17.0 g
Mass of oxygen produced (actual yield)= 10.2 g
Percent yield of oxygen = ?
Solution:
Chemical equation:
2H₂O → 2H₂ + O₂
Number of moles of water:
Number of moles = mass/ molar mass
Number of moles = 17.0 g/ 18.016 g/mol
Number of moles = 0.944 mol
Now we will compare the moles of oxygen with water to know the theoretical yield of oxygen.
H₂O : O₂
2 : 1
0.944 : 1/2×0.944 = 0.472 mol
Mass of oxygen:
Mass = number of moles× molar mass
Mass = 0.472 mol × 32 g/mol
Mass = 15.104 g
Percent yield:
Percent yield = [Actual yield / theoretical yield] × 100
Percent yield = [ 10.2 g/ 15.104 g] × 100
Percent yield = 0.675 × 100
Percent yield = 67.5%
A mole of anything contains 6.022x10^23 items. so we need to divide this
1.3 x 10^25 / 6.022 x 10^23 = 21.59 moles
Answer:
Applications of Chemistry:
Chemistry plays an important and useful role towards the development and growth of a number of industries. This includes industries like glass, cement, paper, textile, leather, dye etc. We also see huge applications of chemistry in industries like paints, pigments, petroleum, sugar, plastics, Pharmaceuticals.
Answer: Well 0-7 is acid, and 0-3 is a strong acid. 4-7 is a weak acid. 8-11 is strong base. 12-14 is weak base!
Explanation:
<h3>
Answer:</h3>
Ag⁺(aq) +Cl⁻(aq) → AgCl(s)
<h3>
Explanation:</h3>
The questions requires we write the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate.
<h3>Step 1: Writing a balanced equation for the reaction.</h3>
- The balanced equation for the reaction between aqueous potassium chloride and aqueous silver nitrate will be given by;
KCl(aq) + AgNO₃(aq) → KNO₃(aq) +AgCl(s)
- AgCl is the precipitate formed by the reaction.
<h3>Step 2: Write the complete ionic equation.</h3>
- The complete ionic equation for the reaction is given by showing all the ions involved in the reaction.
K⁺(aq)Cl⁻(aq) + Ag⁺(aq)NO₃⁻(aq) → K⁺(aq)NO₃⁻(aq) +AgCl(s)
- Only ionic compounds are split into ions.
<h3>Step 3: Write the net ionic equation for the reaction.</h3>
- The net ionic equation for a reactions only the ions that fully participated in the reaction and omits the ions that did not participate in the reaction.
- The ions that are not involved directly in the reaction are known as spectator ions and are not included while writing net ionic equation.
Ag⁺(aq) +Cl⁻(aq) → AgCl(s)