Consider the following reaction that is occurring inside a sealed container:

CH₄(g) + NH₃(g) <-- --> HCN(g) + 3H₂(g)

If we increase the volume of the sealed container without changing the temperature, will this affect the amounts of product and reactant in this container? If so, will the amounts of products increase or decrease? Briefly EXPLAIN!

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Reid WolffLv2

17 Dec 2019

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Answer all questions 4

Consider the following equilibrium between oxides of nitrogen

3 NO(g) NO₂(g) + N₂O(g)

(a) Use data in Appendix C to calculate ∆H° for this reaction. (b) Will the equilibrium constant for the reaction increase or decrease with increasing temperature? (c) At constant temperature, would a change in the volume of the container affect the fraction of products in the equilibrium mixture?

brownweasel195

A. Consider the following reaction where K_p = 2.20Ã10⁴ at 723 K.

2NH₃(g) N₂(g) + 3H₂(g)

If the three gases are mixed in a rigid container at 723 K so that the partial pressure of each gas is initially one atm, what will happen?

Indicate True (T) or False (F) for each of the following:

___TF 1. A reaction will occur in which NH₃(g) is consumed.
___TF 2. K_p will increase.
___TF 3. A reaction will occur in which N₂ is produced.
___TF 4. Q_p is less than K_p.
___TF 5. The reaction is at equilibrium. No further reaction will occur.

B. Consider the following reaction where K_p = 2.01 at 500 K:

PCl₃(g) + Cl₂(g) PCl₅(g)

If the three gases are mixed in a rigid container at 500 K so that the partial pressure of each gas is initially one atm, what will happen?

Indicate True (T) or False (F) for each of the following:

___TF 1. A reaction will occur in which PCl₅(g) is produced.
___TF 2. K_p will decrease.
___TF 3. A reaction will occur in which PCl₃ is produced.
___TF 4. Q is less than K.
___TF 5. The reaction is at equilibrium. No further reaction will occur.