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AURORKA [14]
3 years ago
11

What is the mole ratio of AlCl3 to AlSO4 in the above chemical reaction?

Chemistry
1 answer:
PSYCHO15rus [73]3 years ago
7 0
What reaction is it?
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Is iornIInitrate ionic or covalent
kondaur [170]

Answer:

Iron (II) nitrate is ionic compound

Explanation:

Formula:

Fe(NO₃)₂

Iron (II) nitrate is ionic compound.

Its molecular mass is 179.85 g/mol.

NO⁻₃ is anion while Fe⁺² is cation.

Iron loses its two electron which is accepted by nitrate.

Its molecular formula can be written as FeN₂O₆.

Its color is pale green.

Its melting point is 333.65 K.

It is para magnetic compound.

it is mostly present in non hydrated form.

It is also known as ferric nitrate.

It is used to form sodium amide.

Its is also used catalyst.

7 0
3 years ago
Which is true about the total mechanical energy in a closed system?
ryzh [129]
It’s between C and B
3 0
3 years ago
Read 2 more answers
A gas has a volume of 340.0 mL at 45.90 oC. What is the new temperature of the gas, in Kelvin, if the volume increased to 550.0
d1i1m1o1n [39]

Answer:

Solution for A gas has a volume of 340.0 mL at 45.90 degree celsius. What is the new temperature of the gas, in kelvin, if the volume increased to 550.0 mL.

Missing: oC. ‎| Must include: oC.

Explanation:

6 0
3 years ago
0.315 to scientific notation
irga5000 [103]

Answer:

3.15 × 10^-1

or

3.15E-1

Explanation:

7 0
3 years ago
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2Mg + O2 → 2MgO<br><br> If you are burning 5.8332 g of Mg, how many grams of MgO will this make?
LekaFEV [45]
<h3>Answer:</h3>

9.6724 g MgO

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

<u>Chemistry</u>

<u>Stoichiometry</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN - Balanced] 2Mg + O₂ → 2MgO

[Given] 5.8332 g Mg

<u>Step 2: Identify Conversions</u>

[RxN] 2 mol Mg = 2 mol MgO

Molar Mass of Mg - 24.31 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of MgO - 24.31 + 16.00 = 40.31 g/mol

<u>Step 3: Stoichiometry</u>

  1. Set up:                              \displaystyle 5.8332 \ g \ Mg(\frac{1 \ mol \ Mg}{24.31 \ g \ Mg})(\frac{2 \ mol \ MgO}{2 \ mol \ Mg})(\frac{40.31 \ g \ MgO}{1 \ mol \ MgO})
  2. Multiply/Divide:                                                                                               \displaystyle 9.67241 \ g \ MgO

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 5 sig figs.</em>

9.67241 g MgO ≈ 9.6724 g MgO

5 0
3 years ago
Read 2 more answers
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