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stiks02 [169]
2 years ago
8

*WILL GIVE BRAINLIEST TO CORRECT ANSWER * Question in picture

Chemistry
2 answers:
sineoko [7]2 years ago
5 0
The Answer for this question is : A

1 & 2
solong [7]2 years ago
5 0
1 and 2
The answer is A ^ _ ^
1 and 2
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Moles of cations are in 1.35 mol of K2SO4
KatRina [158]

1.35 mole of K₂SO₄ contain 2.7 moles of cation.

Cations are positive ions. They are the ions of metallic elements.

To obtain the answer to the question, we'll begin by calculating the number of mole of cations in 1 mole of K₂SO₄.

K₂SO₄ (aq) —> 2K⁺ (aq) + SO₄²¯ (aq)

<h3>Cation => K⁺</h3>

From the balanced equation above,

1 mole of K₂SO₄ contains 2 moles of K⁺ (i.e cation).

Finally, we shall determine the number of mole of cation in 1.35 mole of K₂SO₄. This can be obtained as follow:

1 mole of K₂SO₄ contains 2 moles of K⁺ (i.e cation).

Therefore, 1.35 mole of K₂SO₄ will contain = 1.35 × 2 = 2.7 moles of K⁺ (i.e cation).

Hence, we can conclude that 1.35 mole of K₂SO₄ contain 2.7 moles of cation

Learn more: brainly.com/question/24707125

6 0
2 years ago
There are several different models that represent compounds. One type of model is shown.
Kipish [7]
What I’m seeing on quizlet says what you’re describing is a ball-and-stick model.
3 0
2 years ago
Read 2 more answers
What is the molecularity of this elementary step?
dybincka [34]
The correct answer is b. bimolecular
3 0
3 years ago
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The ka of hf is 6.8 x 10-4. what is the ph of a 0.35 m solution of hf?
damaskus [11]
When the reaction equation is:

HF ↔ H+   +   F-

and when the Ka expression
= concentration of products/concentration of reactions

so, Ka = [H+][F-]/[HF]

when we assume:

[H+] = [F-] = X

and [HF] = 0.35 - X

So, by substitution:

6.8 x 10^-4 = X^2 / (0.35 - X) by solving for X

∴ X = 0.015 M

∴[H+] = X = 0.015

when PH = -㏒[H+]

∴PH = -㏒0.015

        = 1.8
6 0
2 years ago
Manganese(iv) oxide reacts with aluminum to form elemental manganese and aluminum oxide: 3mno2+4al→3mn+2al2o3part awhat mass of
Oxana [17]
<span>12.4 g First, calculate the molar masses by looking up the atomic weights of all involved elements. Atomic weight manganese = 54.938044 Atomic weight oxygen = 15.999 Atomic weight aluminium = 26.981539 Molar mass MnO2 = 54.938044 + 2 * 15.999 = 86.936044 g/mol Now determine the number of moles of MnO2 we have 30.0 g / 86.936044 g/mol = 0.345081265 mol Looking at the balanced equation 3MnO2+4Al→3Mn+2Al2O3 it's obvious that for every 3 moles of MnO2, it takes 4 moles of Al. So 0.345081265 mol / 3 * 4 = 0.460108353 mol So we need 0.460108353 moles of Al to perform the reaction. Now multiply by the atomic weight of aluminum. 0.460108353 mol * 26.981539 g/mol = 12.41443146 g Finally, round to 3 significant figures, giving 12.4 g</span>
7 0
3 years ago
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