Lab: Types of Reactions

Question 1

Consider the following chemical reaction:2CH4(g) C2H2(g) + 3H2(g)Describe what is happening within the system when it is at equilibrium in terms of concentrations, reactions that occur, and reaction rates.

Revolt · Accepted Answer

The system is in dynamic equilibrium: CH4 is decomposing into C2H2 and H2 while C2H2 and H2 react to form CH4. Both reactions continue at equal rates, so the concentrations of all substances remain constant.

Question 2

Which of these did your answer include?

Revolt · Accepted Answer

The equilibrium in the system is a dynamic equilibrium.; At equilibrium, the rate of the forward reaction (CH4 decomposing into C2H2 and H2) is equal to the rate of the reverse reaction (C2H2 and H2 reacting to form CH4).; At equilibrium, the concentrations of all substances are not changing.; At equilibrium, both the forward and reverse reactions are still occurring.

Question 3

Although I2 is the stable form of iodine at low temperatures, at high temperatures the molecule can dissociate:What is the equilibrium constant expression for this system?

Revolt · Accepted Answer

K subscript e q equals StartFraction StartBracket upper I EndBracket superscript 2 over StartBracket upper I subscript 2 EndBracket EndFraction.

Question 4

In this system, the equilibrium lies to the , and the reaction favors the

Revolt · Accepted Answer

Selection 1: left; Selection 2: reactants.

Question 5

In this system, the equilibrium lies to the , and the reaction favors the

Revolt · Accepted Answer

Selection 1: left; Selection 2: reactants.

Lab: Types of Reactions Answers

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