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fgiga [73]
3 years ago
5

1) If you have 2.6 moles of iron (III) oxide, how many molecules of iron (III)

Chemistry
1 answer:
Ugo [173]3 years ago
8 0

Answer:

234

Explanation:

so 3 x 3 x 26 =234

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Why atomic mass is an average vàlue​
lukranit [14]

Answer:

The atomic mass is the average number of protons and neutrons for all natural isotopes of an element. It is a decimal number.

Explanation:

Atomic Mass and Mass Number Example :

Hydrogen has three natural isotopes: 1H, 2H, and 3H. Each isotope has a different mass number.

1H has 1 proton. Its mass number is 1. 2H has 1 proton and 1 neutron. Its mass number is 2. 3H has 1 proton and 2 neutrons. Its mass number is 3. 99.98% of all hydrogen is 1H 0.018% of all hydrogen is 2H 0.002% of all hydrogen is 3H Together, they give a value of atomic mass of hydrogen equal to 1.0079 g/mol.

4 0
3 years ago
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How does changing the temperature affect the chemical reaction?
tiny-mole [99]
The correct answer is C) Raising the temperature increases reaction rate by increasing the energy of the reacting atoms/ions/molecules and increases the number of collisions. 
8 0
3 years ago
What occurs at one of the electrodes in both an electrolytic cell and a voltaic cell?
rjkz [21]
Anode- oxidization

Cathode-reduction
3 0
3 years ago
What element are usually shiny , can be bent or stretched and conduct electricity
Alik [6]

Answer:

gold and copper

Explanation:

but I think there is 1 more

8 0
3 years ago
You are given a 1.55 g mixture of calcium nitrate and calcium chloride. You dissolve this mixture in 20 mL of water and add an e
irina [24]

Answer:

13.4 (w/w)% of CaCl₂ in the mixture

Explanation:

All the Cl⁻ that comes from CaCl₂ (Calcium chloride) will be precipitate in presence of AgNO₃ as AgCl.

To solve this problem we must find the moles of AgCl = Moles of Cl⁻. As 2 moles of Cl⁻ are in 1 mole of CaCl₂ we can find the moles of CaCl₂ and its mass in order to find mass percent of calcium chloride in the original mixture.

<em>Moles AgCl - Molar mass: 143.32g/mol -:</em>

0.535g * (1mol / 143.32g) = 3.733x10⁻³ moles AgCl = Moles Cl⁻

<em>Moles CaCl₂:</em>

3.733x10⁻³ moles Cl⁻ * (1mol CaCl₂ / 2mol Cl⁻) = 1.866x10⁻³ moles CaCl₂

<em>Mass CaCl₂ -Molar mass: 110.98g/mol-:</em>

1.866x10⁻³ moles CaCl₂ * (110.98g/mol) = 0.207g of CaCl₂ in the mixture

That means mass percent of CaCl₂ is:

0.207g CaCl₂ / 1.55g * 100 =

<h3>13.4 (w/w)% of CaCl₂ in the mixture</h3>
8 0
3 years ago
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