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    What does the delta temp mean? Does it mean the forward reaction is exothermic.

    I'll take it as if it does, so if the temp increases then wouldn't the equilibrium shift towards the exothermic reaction(which is the forward reaction). So equilibrium shifts toward the left. So more products are formed, as its an exothermic reaction which reduces the temperature .
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    Hi Questioness

    You are right when you say the delta value is showing that the forward reaction is exothermic, this is because it is a negative enthalpy value. Unfortunately you have confused yourself afterwards.

    The forward reaction is exothermic which means gives out heat. If we increase the temperature of the system this will cause the equilibrium to shift to the side which would counteract this temperature increase, which would be to the left (or the reactants) because this is the ENDOTHERMIC side.

    I hope that helps

    Alex
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    (Original post by ajsullivan)
    Hi Questioness

    You are right when you say the delta value is showing that the forward reaction is exothermic, this is because it is a negative enthalpy value. Unfortunately you have confused yourself afterwards.

    The forward reaction is exothermic which means gives out heat. If we increase the temperature of the system this will cause the equilibrium to shift to the side which would counteract this temperature increase, which would be to the left (or the reactants) because this is the ENDOTHERMIC side.

    I hope that helps

    Alex
    How would the endothermic counteract and increasing temperature. Endothermic reactions give out heat so that would further increase the temperature?
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    No, your making the same mistake again. EXOthermic means give out heat, ENDOthermic means taking in heat. Read my explanation again reminding yourself off exo and endo.
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    (Original post by Questioness)
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    What does the delta temp mean? Does it mean the forward reaction is exothermic.

    I'll take it as if it does, so if the temp increases then wouldn't the equilibrium shift towards the exothermic reaction(which is the forward reaction). So equilibrium shifts toward the left. So more products are formed, as its an exothermic reaction which reduces the temperature .
    Firstly, this is an exothermic reaction. we know that because the enthalpy change for the reaction is a negative value.
    In an exothermic reaction, when temperature is increased, the equilibrium shifts to the left and more reactants are formed.
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    Le Chatelier's principle states that when the rate of equilibrium is subjected to a change, the position of the equilibrium will shift to minimise the change. Here, you have been given a negative enthalpy value, meaning that the reaction is exothermic(moving to the right). Therefore, increasing the temperature means that the molecules will move to minimise the change by absorbing energy (endothermic), which shifts to the left.
 
 
 
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