Question
Consider the following reaction:
HCN <--> H+ + CN- delta H = 315kJ
If 1.00 mole of CN- in the form of NaCN was added to equilibrium mixture, describe the effect on [H+], [HCN], [CN-], pH, and heat.
HCN <--> H+ + CN- delta H = 315kJ
If 1.00 mole of CN- in the form of NaCN was added to equilibrium mixture, describe the effect on [H+], [HCN], [CN-], pH, and heat.
Answers
This ia Le Chatelier's Principle problem. When working with those problems I find it best to include heat as part of the equation. for dH = + it means endothermic; for dH = - it means exothermic. Therefore, I add heat to the appropriate side.
HCN + heat ==> H^+ + CN^-
Le Chatelier's Principle says that a system in equilibrium will try to undo what we do to it.
So adding CN^- to a system in equilibrium means the system will shift to the left (in order to try and use up the added CN^-). That means HCN increases, H^+ decreases, etc.
Note: The CN will increase because we have added CN^-; however, it will not be the sum of what we added and what it was originally because some of the CN is lost when it shifts to the left to form HCN.
HCN + heat ==> H^+ + CN^-
Le Chatelier's Principle says that a system in equilibrium will try to undo what we do to it.
So adding CN^- to a system in equilibrium means the system will shift to the left (in order to try and use up the added CN^-). That means HCN increases, H^+ decreases, etc.
Note: The CN will increase because we have added CN^-; however, it will not be the sum of what we added and what it was originally because some of the CN is lost when it shifts to the left to form HCN.
Related Questions
Does my work here look right?
3. One mole of an ideal gas expands adiabatically into a vacuum. C...
CH4 + 2O2 ---> CO2 + 2H2O
Delta H H2O= -285.8 kJ/mole
Delta H CO2= -393.3 kJ/mole
What is the...
Given overall reaction: P4 + 10Cl2 ---> 4PCl5 Delta H for the reaction = ?
PCl5 ----->...
Why these answers are so?
1- For this reaction 2H2 + O2 = 2H2O
a- dela H=delta Hf
b-delta Hc= del...