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stich3 [128]
3 years ago
12

Magnesium oxide does not readily decompose into magnesium and oxygen. The reaction is shown below. MgO(s) + 601.7 kJ mc017-1.jpg

Mg(s) + ½O2(g) Which factor plays the most important role in allowing this reaction to occur? temperature concentration pressure surface area Mark this and return
Chemistry
2 answers:
Sophie [7]3 years ago
7 0

Answer is: temperature.

Balanced chemical reaction: MgO(s) + heat → Mg(s) + 1/2O₂(g).

This is endothermic reaction (ΔH > 0, chemical reaction that absorbs more energy than it releases). In endothermic reactions heat is reactant.

Because magnesium oxide (MgO) is in solid state, concentration, pressure and surfuce does not play the most important role in allowing this reaction to occur.

galben [10]3 years ago
5 0
TEMPERATURE IS THE ANSWER 
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Using PV = nRT, we can calculate the moles of the sample.
874 mmHg = 116,524 Pa
n = PV/RT
n = 116,524 x 294 x 10⁻⁶ / 8.314 x (140 + 273)
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moles = mass / Mr
Mr = 0.271/9.98 x 10⁻³
Mr = 27.2
Mass of empirical formula = 14
Repeat units = 27.2 / 14 ≈ 2

Formula of substance:
C₂H₄

Combustion equation:
C₂H₄ + 3O₂ → 2CO₂ + 2H₂O

1 mole produces 2 moles of CO₂, so 3 moles will produce 6 moles CO₂
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697 g

Explanation:

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C₂H₅OH + C₃H₇COOH → C₃H₇COOC₂H₅ + H₂O

The molar ratio of C₂H₅OH to C₃H₇COOC₂H₅ is 1:1. The moles of C₃H₇COOC₂H₅ produced from 6.00 moles of C₂H₅OH are:

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