Answer:
Mass of reactant and mass of product must be equal.
Explanation:
Law of conservation of mass:
According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.
Explanation:
This law was given by French chemist Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.
For example:
In given photosynthesis reaction:
6CO₂ + 6H₂O + energy → C₆H₁₂O₆ + 6O₂
there are six carbon atoms, eighteen oxygen atoms and twelve hydrogen atoms on the both side of equation so this reaction followed the law of conservation of mass.
Answer:
add up the mass of protons and neutrons
Explanation:
Hello :))
Your question was:Lorek lives near the North Pole. The snow in his backyard adds water to the atomosphere through______.
The answer is: Sublimation
Hope this helps!
Good day! :D
Answer:
C. 2O₃ ⇌ 3O₂
Explanation:
Kp is the equilibrium constant calculated from the partial pressures of a gas-phase reaction equation.
For a general gas-phase reaction aA + bB ⇌ nC + xD
the expression for the Kp = (pC)ⁿ(pD)ˣ / (pA)ᵃ(pB)ᵇ
where pA = partial pressure of A; pB = partial pressure of B; pC = partial pressure of C; pD = partial pressure of D
From the given reaction in equilibrium; N₂ + 3H₂ ⇌ 2NH₃
Kp = (pNH₃)² / (pN₂)¹ * (pH₂)³ = 4/7
(pNH₃)² / (pN₂)¹ * (pH₂)³ = (2)²/ (1)¹ * (3)³
Therefore, number of mole of reactants and products is equivalent to partial pressure.
A. 2SO₂ ⇌ O₂ + 2SO₃
pSO₂ = 2, pO₂ = 1, pSO₃ = 2,
Kp = 2²/ (2² * 1²) = 4/4 = 1
B. N₂O₄ ⇌ 2NO₂
pN₂O₄ = 1, pNO₂ = 2
Kp = 2²/1² = 4
C. 2O₃ ⇌ 3O₂
pO₃ = 2, pO₂ = 3
Kp = 3³/2² = 27/4
D. PCl₅ ⇌ PCl₃ + Cl₂
pPCl₅ = 1, pPCl₃ = 1, pCl₂ = 1
Kp = (1¹ * 1¹) / 1¹ = 1
Answer:
0.0922 M
Explanation:
The problem first states that the titration is made using NaOH, and later asks about the addition of KOH. I'm going to assume NaOH was used throughout the whole problem. The result does not change if it was KOH instead.
The reaction that takes place is:
- HClO₄ + NaOH → NaClO₄ + H₂O
First we <u>calculate how many HClO₄ moles are there in the sample</u>, using the <em>given molarity and volume</em>:
- 0.624 M * 13.0 mL = 8.11 mmol HClO₄
Then we <u>calculate how many NaOH moles were added</u>:
- 0.258 M * 15.0 mL = 3.87 mmol NaOH
Now we calculate how many HClO₄ remained after the reaction:
- 8.11 - 3.87 = 4.24 mmol HClO₄
As <em>HClO₄ is a strong acid</em>, 4.24 mmol HClO₄ = 4.24 mmol H⁺
Finally we <u>calculate the molarity of H⁺</u>, using the<em> calculated number of moles and final volume</em>:
- Final volume = 31.0 mL + 15.0 mL = 46.0 mL
- 4.24 mmol / 46.0 mL = 0.0922 M
