# Chemistry Lab Report- Determining the Enthalpy of Enthalpy Change, H, for a Redox Reaction (

by florianb (student)

Chemistry Lab Report- Determining the Enthalpy of Enthalpy Change, ΔH, for a Redox Reaction (DCP, CE Criterion)

Aim: The aim of this investigation is to experimentally determine the change in the enthalpy for the following redox (displacement) reaction:

Zn (s) + Zn2+(aq) ---->+ Zn2++ Cu (s)

Data Collection and Processing

Recording Raw Data:

Data Table:

Minimum temperature of trial 1: 21 °C

Maximum temperature for trial 1:59°C

Temperature difference of trial 1: 38 °C

Minimum temperature of trial 2: 21 °C

Maximum temperature for trial 2:59 °C

Temperature difference of trial 2: 38 °C

Processing Raw Data:

Average of Temperature rise (ΔT): 38°C+38°C 2 trials= 38°C

This value will be used to calculate the enthalpy change throughout this experiment.

Number of Moles (Cu + Zn2+) = Mass/Mr

Mass=Mass of CuSO4 Solution (g) (±0.05g) + Mass of Zinc Powder (g) (±0.05g)

Mass= 25.0g (±0.05g)  +4.0g (±0.05g)

Mass= 29.0g (±0.05g)

Convert to Kg: 29.0g/1000= 0.0290Kg

Mr=

Cu-1; 63.55 x 1=63.55

S-1; 32.06 x 1=32.06

O-4 16.00 x 4=64.00

Total relative mass of = 63.55 + 32.06 + 64.00

Total relative mass of ethanol= 159.61= 159.6 (to 3 significant figures)

Number of Moles (Cu + Zn2+) = 29.0g159.6= 0.182 moles

Enthalpy change (heat energy change) (ΔH) measured in kJ per mole

Mass (m) measured in (Kg)

Specific heat capacity ...