The correct answer is A. PH value
If a substance is very acidity it has a high PH, if it is less acidic (alkalinity) is has a lower PH. For instance, water has a PH of 7 because it is in between of being acidic and alkaline.
Answer:
2360J
Explanation:
Given parameters:
Mass of aluminum = 25g
Melting point = 658°C
Latent heat of melting = 94.4j/g
Unknown:
Amount of heat require for melting = ?
Solution:
The amount of heat required for this melting will be the product of the mass of the aluminum and the latent heat of melting;
H = m L
m is the mass
L is the latent heat of melting
Insert the parameters and solve;
H = 25 x 94.4 = 2360J
Democritus *suggested* the existence of the atom, that everything was made up of tiny particles, but wasn't really able to get more specific than that. Dalton also theorized that everything was made up of indivisible particles, but went further basing his theory on actual scientific principles, such as the Law of Conservation of Mass and the Law of Constant Composition. He also said that atoms weren't created or destroyed in a chemical reaction, just rearranged. There's more to it than that, but basically, Dalton's theory was based more on science while Democritus' theory was too general to be useful in chemical situations.
I believe the answer is the third one.
The pounds of alum produced when 0.26 g of hydrogen was produced are 0.0434 lb.
First, let's convert 0.126 g of hydrogen to moles using its molar mass (2.02 g/mol).
Let's consider the steps to make alum (KAl(SO₄)₂⋅12H₂O) from aluminum (Al).
-
2 Al(s) + 2 KOH(aq) + 6 H₂O(l) →2 KAl(OH)₄(aq) + 3 H₂(g)
-
2 KAl(OH)₄(aq) + H₂SO₄(aq) → 2 Al(OH)₃(s) + K₂SO₄(aq) + 2 H₂O(l)
-
2 Al(OH)₃(s) + H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 6 H₂O(l)
-
K₂SO₄(aq) + Al₂(SO₄)₃(aq) + 24 H₂O(l) → 2 KAl(SO₄)₂⋅12H₂O(s)
To relate H₂ to KAl(SO₄)₂⋅12H₂O, we need to consider the appropriate molar ratios:
- In step 1, the molar ratio of H₂ to KAl(OH)₄ is 3:2.
- In step 2, the molar ratio of KAl(OH)₄ to Al(OH)₃ is 2:2.
- In step 3, the molar ratio of Al(OH)₃ to Al₂(SO₄)₃ is 2:1.
- In step 4, the molar ratio of Al₂(SO₄)₃ to KAl(SO₄)₂⋅12H₂O is 1:2.
The moles of KAl(SO₄)₂⋅12H₂O produced from 0.0624 moles of H₂ are:
The molar mass of alum is 474.38 g/mol. The mass corresponding to 0.0416 moles is:
Finally, we convert 19.7 grams to pounds using the conversion factor 1 lb = 454 g.
The pounds of alum produced when 0.26 g of hydrogen was produced are 0.0434 lb.
You can learn more about molar ratios here: brainly.com/question/15973092