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Enthalpy Change!!! Unit 2 Chemistry
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50.0 cm^3 of 2.00M sodium hydroxide and 50.0 cm^3 of 2.00M HCl were mixed in an expanded polystyrene beaker. The temperature rose by 11.0K.
a) Calculate the delta H for the reaction.
b) How will this value compare with the accepted value for this reaction?
c) explain your answer to b.
a) Calculate the delta H for the reaction.
b) How will this value compare with the accepted value for this reaction?
c) explain your answer to b.
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#2
(Original post by Jyotii)
50.0 cm^3 of 2.00M sodium hydroxide and 50.0 cm^3 of 2.00M HCl were mixed in an expanded polystyrene beaker. The temperature rose by 11.0K.
a) Calculate the delta H for the reaction.
b) How will this value compare with the accepted value for this reaction?
c) explain your answer to b.
50.0 cm^3 of 2.00M sodium hydroxide and 50.0 cm^3 of 2.00M HCl were mixed in an expanded polystyrene beaker. The temperature rose by 11.0K.
a) Calculate the delta H for the reaction.
b) How will this value compare with the accepted value for this reaction?
c) explain your answer to b.
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(Original post by morgan8002)
What are your thoughts on the question? Do you have an ideas on how to start?
What are your thoughts on the question? Do you have an ideas on how to start?
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#4
(Original post by Jyotii)
Is delta H q=mc(delta)T
Is delta H q=mc(delta)T
This is how to work out the first part of the question, but this won't be for one mole of the reactants. You need to use this to work out the enthalpy change for one mole.
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