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diamong [38]
3 years ago
8

Consider the following hypothetical molecular collisions and predict which of the following will form potential products, given

the values for the energy of activation, Ea, and enthalpy of the reaction, ΔH, in combination with the molecular orientation.
Chemistry
1 answer:
Annette [7]3 years ago
7 0

Answer:

The collision theory is defined as the rate of a reaction is proportional to the rate of reactant collisions.

Explanation:

The reacting species should collide with orientation that allows contract between the atoms that will become bonds together in the product.

The collision occurs with adequate energy  to permit mutual penetration of the reacting species. The two physical factors based on the orientation and energy of collision, the following reaction with carbon monoxide with oxygen is considered.

 2CO(g) + O2(g) → 2CO2 (g)

After collision between the carbon monoxide and oxygen the reaction is

 CO(g) + O2(g) → CO2 (g) + O(g)

Based on the theories of chemical reaction the molecules collide with sufficient amount of energy an activated complex is formed.

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Consider the reaction; Mg + O2 → MgO Calculate the mass of magnesium oxide possible if 2.5 g Mg reacts with 5.0 g O2?
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Answer:

4.15g

Explanation:

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2.5/24.3 = 0.103 moles/2 = 0.0515

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0.0515 is small than 0.156, so limiting reactant is Mg

Compare the ratio of Mg with MgO

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So same moles = 0.103 moles

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