The volume of the 0.130 M sulfuric acid, H₂SO₄ required to react completely with 65.9 g sodium hydroxide, NaOH is 6.34 L
- We'll begin by calculating the number of mole of in 65.9 g sodium hydroxide, NaOH. This can be obtained as follow:
Mass of NaOH = 65.9 g
Molar mass of NaOH = 23 + 16 + 1 = 40 g/mol
<h3>Mole of NaOH =?</h3>
Mole = mass / molar mass
Mole of NaOH = 65.9 / 40
<h3>Mole of NaOH = 1.6475 mole</h3>
- Next, we shall determine the number of mole of H₂SO₄ needed to react with 1.6475 mole of NaOH. This can be obtained as follow:
2NaOH + H₂SO₄ —> Na₂SO₄ + 2H₂O
From the balanced equation above,
2 moles of NaOH reacted with 1 mole of H₂SO₄.
Therefore,
1.6475 mole of NaOH will react with = 
= 0.82375 mole of H₂SO₄.
- Finally, we shall determine the volume of 0.130 M sulfuric acid, H₂SO₄ required for the reaction.
Molarity of H₂SO₄ = 0.130 M
Mole of H₂SO₄ = 0.82375 mole
<h3>Volume of H₂SO₄ =? </h3>
Volume = mole / Molarity
Volume of H₂SO₄ = 0.82375 / 0.130
<h3>Volume of H₂SO₄ = 6.34 L </h3>
Therefore, the volume of the 0.130 M sulfuric acid, H₂SO₄ required for the reaction is 6.34 L
Learn more: brainly.com/question/7882345
The method used to separate oxygen from mercury oxide is by strong heating. In the lab mercury oxide is placed in strong glass test tube and strong heat applied to the test tube. Mercury oxide then undergoes a decomposition reaction to produce mecury and oxygen.
Antoine Lavoisier , the father of modern chemistry is the one credited as having proved the decomposition of mercuric oxide by heating, and that the result was production of mercury and oxygen.
A decomposition reaction is a reaction in which a compound breaks down into two or more simpler substances.
Answer is: 5,1 mol KOH.
V (KOH) = 0,8l = 0,8 dm³.
c (KOH) = 6,4 mol/dm³.
V - volume of solution.
c - concentration of solution.
c = n÷V
n - amount of substance.
n (KOH) = c·V = 6,4 mol/dm³ · 0,8 dm³ = 5,12 mol.
Potassium hydroxide (KOH) can<span> </span>dissolve<span> in water at room temperature.</span>
Answer:
0.846 moles.
Explanation:
- This is a stichiometric problem.
- The balanced equation of complete combustion of butane is:
C₄H₁₀ + 6.5 O₂ → 4 CO₂ + 5 H₂O
- It is clear from the stichiometry of the balanced equation that complete combustion of 1.0 mole of butane needs 6.5 moles of O₂ to produce 4 moles of CO₂ and 5 moles of H₂O.
<u><em>Using cross multiplication:</em></u>
- 1.0 mole of C₄H₁₀ reacts with → 6.5 moles of O₂
- ??? moles of C₄H₁₀ are needed to react with → 5.5 moles of O₂
- The number of moles of C₄H₁₀ that are needed to react with 5.5 moles of O₂ = (1.0 x 5.5 moles of O₂) / (6.5 moles of O₂) = 0.846 moles.
Rubidium is the alkali metal that would melt on a hot day.
