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Mnenie [13.5K]
2 years ago
14

Write the complete and net ionic equations for the following reactions. If only the reactants are given, predict the products an

d balance the equation first.
​

Chemistry
1 answer:
11111nata11111 [884]2 years ago
3 0

Explanation:

u can put them in order crossed are spectator ions. hope this helps:)

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About how many elements make up everything on Earth?
Alex73 [517]
92 i am pretty sure


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7 0
3 years ago
Use the following equation to answer question 1-4. Make sure you balance first.
worty [1.4K]
<h3>Answer:</h3>

5.2 mol H₂O

<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>

  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN - Balanced] 6HCl + Fe₂O₃ → 2FeCl₃ + 3H₂O

[Given] 10.4 mol HCl

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

[RxN] 6 mol HCl = 3 mol H₂O

<u>Step 3: Stoichiometry</u>

  1. Set up:                             \displaystyle 10.4 \ mol \ HCl(\frac{3 \ mol \ H_2O}{6 \ mol \ HCl})
  2. Multiply/Divide:               \displaystyle 5.2 \ mol \ H_2O
4 0
3 years ago
When the fuel mixture contained in a 1.49 l tank, stored at 750 mmhg and 298 k, undergoes complete combustion, how much heat is
Ket [755]
Get to know first how many moles in the gas:n = pV/RT= (1.013*10^5*750/760) Pa *1.49*10^-3 m^3/(8.314 J/(molK)*298) n = 0.0601 moles. 
The combustion energies  are  889 kJ/mol (methane) and 2 220 kJ (propane) x = moles methane, y = moles propane 
x*889 + y*2220 = 778 x + y = 0.0601----------- x = 0.267784 moles = 0.267784*100/0.0601 = 44.6 % y = 0.243216 moles = 0.243216*100/0.0601 = 55.4 %
4 0
3 years ago
In the hydrolysis of trimyristin the reaction mixture is heated at about 75℃ for 45 minutes. what is the purpose of heating a re
Effectus [21]

The correct answer is :

the purpose of heating the mixture is to accelerate the reaction and mix the reagent.

The explanation:

Many organic reactions are slow and can take an extended period of time to achieve any noticeable effect so heating is often used to increase the rate of reaction. However, many organic compounds have low boiling points and will vaporise upon exposure to such high heat, preventing the reaction from proceeding in full.

so, heating is used. This refers to heating a solution with an attached condenser to prevent reagents from escaping

6 0
3 years ago
Read 2 more answers
if 14.0 g of aluminium reacts with excess sulfuric acid to produce 75.26 g of aluminium sulfate, what is the percent yield?
vlada-n [284]

Taking into account definition of percent yield, the percent yield for the reaction is 84.88%.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

2 Al + 3 H₂SO₄ → Al₂(SO₄)₃ + 3 H₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • Al: 2 moles
  • H₂SO₄: 3 moles
  • Al₂(SO₄)₃. 1 mole
  • H₂: 3 moles

The molar mass of the compounds is:

  • Al: 27 g/mole
  • H₂SO₄: 98 g/mole
  • Al₂(SO₄)₃: 342 g/mole
  • H₂: 2 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

  • Al: 2 moles ×27 g/mole= 54 grams
  • H₂SO₄: 3 moles ×98 g/mole= 294 grams
  • Al₂(SO₄)₃: 1 mole ×342 g/mole= 342 grams
  • H₂: 3 moles ×2 g/mole= 6 grams

<h3>Mass of aluminium sulfate formed</h3>

The following rule of three can be applied: if by reaction stoichiometry 54 grams of aluminium form 342 grams of aluminium sulfate, 14 grams of aluminium form how much mass of aluminium sulfate?

mass of aluminium sulfate=\frac{14 grams of aluminium x342 grams of aluminium sulfate}{54 grams of aluminium}

<u><em>mass of aluminium sulfate= 88.67 grams</em></u>

Then, 88.67 grams of aluminium sulfate can be produced if 14.0 g of aluminium reacts with excess sulfuric acid.

<h3>Percent yield</h3>

The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.

The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

percent yield=\frac{actual yield}{theorical yield} x100

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

<h3>Percent yield for the reaction in this case</h3>

In this case, you know:

  • actual yield= 75.26 grams
  • theorical yield= 88.67 grams

Replacing in the definition of percent yields:

percent yield=\frac{75.26 grams}{88.67 grams} x100

Solving:

<u><em>percent yield= 84.88%</em></u>

Finally, the percent yield for the reaction is 84.88%.

Learn more about

the reaction stoichiometry:

brainly.com/question/24741074

brainly.com/question/24653699

percent yield:

brainly.com/question/14408642

#SPJ1

7 0
1 year ago
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