enthalpy change
the student added 0.0210 mol of pure anhydrous copper(II) sulphate to 25.0cm3 of deionised water in an open polystyrene cup. an exothermic reaction occurred and the temperature of the water increased by 14.0 C
Use the data to calculate the enthalpy change in kjmol-1 for this reaction of copper(II) sulphate. this is the student value for deltaH1
In this experiment you should assume that all of the heat released is used to raise the temperature of the 25.0g of water. the specific heat capacity of water is 4.18 JK-1g-1
Use the data to calculate the enthalpy change in kjmol-1 for this reaction of copper(II) sulphate. this is the student value for deltaH1
In this experiment you should assume that all of the heat released is used to raise the temperature of the 25.0g of water. the specific heat capacity of water is 4.18 JK-1g-1
Original post by alexandrad0037
the student added 0.0210 mol of pure anhydrous copper(II) sulphate to 25.0cm3 of deionised water in an open polystyrene cup. an exothermic reaction occurred and the temperature of the water increased by 14.0 C
Use the data to calculate the enthalpy change in kjmol-1 for this reaction of copper(II) sulphate. this is the student value for deltaH1
In this experiment you should assume that all of the heat released is used to raise the temperature of the 25.0g of water. the specific heat capacity of water is 4.18 JK-1g-1
Use the data to calculate the enthalpy change in kjmol-1 for this reaction of copper(II) sulphate. this is the student value for deltaH1
In this experiment you should assume that all of the heat released is used to raise the temperature of the 25.0g of water. the specific heat capacity of water is 4.18 JK-1g-1
Q = mass (25) x 4.18 x temperature change (14).
Q/1000 (convert to KJ)
Enthalpy change = Q/moles (0.021)
As temperature increased, exothermic, so add negative sign to enthalpy.
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