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Eva8 [605]
2 years ago
5

How many grams of CaSO4 (Molar mass = 136 g) can be produced if 15.4 g Ca3(PO4)2 (molar mass = 310 g) completely reacts?

Chemistry
1 answer:
kykrilka [37]2 years ago
8 0
Balance Chemical equation is as follow,

                    Ca₃(PO₄)₂  + 3 H₂SO₄   →   3 CaSO₄  +  2 H₃PO₄

According to eq.

     310 g (1 mole) of Ca₃(PO₄)₂ produces  =  408.42 g (3 mole) of CaSO₄
So,
              15.4 g of Ca₃(PO₄)₂ will produce  =  X g of CaSO₄

Solving for X,
                                           X  =  (15.4 g × 408.42 g) ÷ 310 g

                                           X  =  20.28 g of CaSO₄
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Given the following unbalanced equation:
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<h3>Answer:</h3>

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<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> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

  • Moles
  • Compounds

<u>Stoichiometry</u>

  • Using Dimensional Analysis
  • Analyzing Reactions RxN
<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN - Unbalanced] Mg + O₂ → MgO

[RxN - Balanced] 2Mg + O₂ → 2MgO

[Given] 8.01 moles Mg

[Solve] moles MgO

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

[RxN] 2 mol Mg → 2 mol MgO

<u>Step 3: Stoich</u>

  1. [DA] Set up:                                                                                                       \displaystyle 8.01 \ mol \ Mg(\frac{2 \ mol \ MgO}{2 \ mol \ Mg})
  2. [DA] Multiply/Divide [Cancel out units]:                                                          \displaystyle 8.01 \ mol \ MgO
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