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Question
Write a relation between ∆G and Q and define the meaning term and answer the following:
Explain the effect of increase in pressure in terms of reaction quotient Q. for the reaction: \[\ce{CO (g) + 3H2 (g) ⇌ CH4 (g) + H2O (g)}\]
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Solution
When we increase the pressure equilibrium will shift in forward direction it means Q < K.
Types of Chemical Reactions: There are 4 main types of chemical reactions. These are:
1. Combination Reactions: Combination Reactions are chemical reactions with 2 or more substances combining to form one single compound.
2. Decomposition Reactions: Decomposition Reactions are chemical reactions with one compound decomposing to produce 2 or more different substances. The digestion process of food in our body is a Decomposition reaction.
3. Displacement Reactions: Displacement reactions are reactions that involve the displacement of 1 element or group by another.
4. Double Displacement: Displacement reactions are reactions with 2 compounds that react to form 2 new compounds. In the displacement reaction, no change in oxidation state occurs.
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RELATED QUESTIONS
Write a relation between ∆G and Q and define the meaning term and answer the following:
Why a reaction proceeds forward when Q < K and no net reaction occurs when Q = K.
For a system to be in equilibrium, ΔG = 0 under conditions of constant.
For the reaction \[\ce{A(g) <=> 2B(g)}\] the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K.
[Given: R = 0.0831 L atm mol−1 K−1]
Kp for the reaction at 1000 K is:
For the reaction \[\ce{2A <=> B + C}\], Kc = 4 × 10−3. At a given time, the composition of reaction mixture is:
[A] = [B] = [C] = 2 × 10−3 M
Then, which of the following is correct?
