Which conditions ( reactant concentration , pressure , and temperature ) elevate high concentration of the underlines in these following equilibrium systems :
1) 2CO + O2 <==> 2CO2 + 167 kJ
2) Cu^+2 + 4NH3 <==> [ Cu(NH3)4 ]^+2 + 24 kJ
3) 2HI + 12.6 kJ <==> H2 + I2
4) 4HCl + O2 <==> 2H2O + 2Cl2 + 113 kJ
5) PCl5 + 88 kJ <==> PCl3 + Cl2
Here is the first one in detail (for CO2).
1) 2CO + O2 <==> 2CO2 + 167 kJ and I will rewrite the problem to more clearly show how the heat is treated. Basically the heat is made to look just like an added product (if an exothermic rxn) or a reactant (if an endothermic rxn).
1) 2CO + O2 <==> 2CO2 + heat
All of these questions are answered following Le Chatlier's Principle. That says that if we do something to a rxn it will shift so as to undo what we've done to it. Basically we are asking how CO2 is increased by
a. what change in reactant concns(increase or decrease)?
b. what changes in T(increase or decrease)?
c. what changes in pressure(increase or decrease)?
a.If we want to increase CO2 we must increase the concentration of the reactants (put in more CO or O2 or both). That will shift the equilibrium to the right producing more CO2 and more heat. (Adding either reactant makes the reaction try to use up what we've added--that's undoing what we've done-- and that decreases CO and O2 and adds heat and CO2)
b. If we decrease T the reaction will shift so as add heat and that means it will shift to the right. Heat will be added, CO2 will be increased, CO and O2 will decrease.
c. Changes in pressure for gas reactions make the reaction shift to the side with fewer mols for increase in P or to side with more mols for decrease in P. You have 3 mols gas on the left and 2 mol on the right. So increased in P will make it shift to produce more CO2 at the expense of CO and O2.
I'm sorry
the underlines are "
1) CO2
2) [ Cu(NH3)4 ]^+2
3) I2
4) 2Cl2
5) Cl2
To determine how the concentration, pressure, and temperature affect the equilibrium position in the given reactions, we need to consider a few principles from chemical equilibrium.
1) Effect of Concentration: According to Le Chatelier's principle, if the concentration of a reactant or product is increased, the equilibrium will shift in the opposite direction to alleviate the stress. Conversely, if a concentration decreases, the equilibrium will shift in the direction of the affected species.
2) Effect of Pressure: For reactions involving gases, changes in pressure can affect the equilibrium position. Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, whereas decreasing pressure will shift the equilibrium towards the side with more moles of gas.
3) Effect of Temperature: Changes in temperature can have different effects on equilibrium depending on whether the reaction is exothermic (releases heat) or endothermic (absorbs heat). Increasing temperature favors the endothermic reaction, while decreasing temperature favors the exothermic reaction.
Now, let's apply these principles to the given reactions:
1) 2CO + O2 <==> 2CO2 + 167 kJ:
- Increasing the concentration of CO or O2 would shift the equilibrium towards the product side (2CO2) to alleviate the stress.
- Increasing pressure would not have a significant effect since there are no gases involved.
- Increasing temperature would favor the exothermic reaction (forward reaction), leading to a decrease in the concentration of CO2.
2) Cu^+2 + 4NH3 <==> [ Cu(NH3)4 ]^+2 + 24 kJ:
- Increasing the concentration of Cu^+2 or NH3 would shift the equilibrium towards the product side ([ Cu(NH3)4 ]^+2) to alleviate the stress.
- Increasing pressure would not have a significant effect since there are no gases involved.
- Increasing temperature would favor the endothermic reaction (forward reaction), leading to an increase in the concentration of [ Cu(NH3)4 ]^+2.
3) 2HI + 12.6 kJ <==> H2 + I2:
- Increasing the concentration of HI would shift the equilibrium towards the product side (H2 and I2) to alleviate the stress.
- Increasing pressure would not have a significant effect since there are no gases involved.
- Increasing temperature would favor the endothermic reaction (forward reaction), leading to an increase in the concentration of H2 and I2.
4) 4HCl + O2 <==> 2H2O + 2Cl2 + 113 kJ:
- Increasing the concentration of HCl or O2 would shift the equilibrium towards the product side (H2O and Cl2) to alleviate the stress.
- Increasing pressure would not have a significant effect since there are no gases involved.
- Increasing temperature would favor the endothermic reaction (forward reaction) and lead to an increase in the concentration of H2O and Cl2.
5) PCl5 + 88 kJ <==> PCl3 + Cl2:
- Increasing the concentration of PCl5 would shift the equilibrium towards the product side (PCl3 and Cl2) to alleviate the stress.
- Increasing pressure would not have a significant effect since there are no gases involved.
- Increasing temperature would favor the endothermic reaction (forward reaction), leading to an increase in the concentration of PCl3 and Cl2.
In summary, the equilibrium position in these reactions can be influenced by changes in reactant concentration, while pressure and temperature effects depend on the presence of gases and the nature of the reaction (exothermic or endothermic).