Determine the enthalpy change, in kJ, when 25 cm3 of 0.5 mol dm-3 hydrochloric acid reacts with 25 cm3 of 0.5 mol dm-3 sodium hydroxide. Give your answer to 2 decimal places.
The student added excess zinc powder to the cup with 50.0 cm3 of 1.0 mol dm-3 copper(II) sulfate solution in a calorimeter. The reaction equation was as follows:
Zn (s) + CuSO4 (aq) → ZnSO4 (aq) + Cu (s)
The maximum temperature rise was 22.6 oC. Using section 1 of the data booklet, determine the enthalpy of reaction, in kJ. Give your answer to 2 significant figures.
Calculate the energy change, q …………………………
Calculate the number of moles of copper(II) sulfate solution ………………
Calculate the enthalpy change of the reaction …………………
0.61 g of ethanol, C2H5OH, was burned in a spirit burner and used to heat 100 cm3 of water in a copper calorimeter. The temperature of the water rose by 40 oC.
i)
Using section 1 and 2 in the data booklet determine the energy, in joules, for this reaction.
4.00 g of powdered iron was reacted with 25.0 cm3 of 2.00 mol dm−3 copper(II) sulfate solution in an insulated beaker. Temperature was plotted against time.
Estimate the time at which the powdered iron was added to the beaker.
The student used the equation q = mcΔT to calculate the enthalpy change for the reaction that took place in the beaker. State the value that the student should use for m.