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Single displacement reaction
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Displacement Reaction
The aim of my experiment is to find out what happens to the heat of
the zinc and copper sulphate solution when one of the variables is
changed.
Key variables:
§ amount of copper sulphate solution
§ amount of zinc
I am going to investigate what happens to the temperature of the zinc
and copper sulphate solution as the amount of zinc is increased. The
equation to show this reaction is:
Zn + CuSO4 ® ZnSO4 + Cu
The enthalpy change for the reaction is:
²H = -217kJ mole ¹
This means that if 1 mole of solution is used of each substance, the
heat given off will be 217,000 Joules.
Apparatus:
§ 1 test tube
§ 20ml of copper sulphate solution for each experiment
§ Zinc
§ Rubber bung
§ Thermometer
Prediction:
I think that as the amount of zinc is increased, the temperature of
the solution will also increase. I have used the following formula to
predict some results of this experiment.
q = Q
mc
where q = temperature rise, Q = quantity of heat, m = mass of solution
(20g) and c = the specific heat capacity of water which = 4.18Jg ¹K ¹.
65g Zinc ® 217000 joules
1g Zinc ® 217000 = 3338 joules
65
Therefore for 1g of zinc:
3338 =39°c rise
20x4.18
I can now use this formula proportionately to predict results for my
investigation.
For 0.3g of zinc:
0.3 x 39 = 12°c rise
For 0.5g of zinc:
0.5 x 39 = 19.5°c rise
For 0.7g of zinc:
0.7 x 39 = 27.3°c rise
For 0.9g of zinc:
0.9 x 39 = 35.1°c rise
I have used this information in order to predict the results of the
temperature rise I expect to see as the amount of zinc is increased. I
have also used this information to plan my experiment.
Two equations were used in this experiment to determine the initial temperature of the hot water. The first equation
Tf-Ti). Next, subtract the initial temperature, 25 degrees from the final temperature, 29 degrees putting the change in temperature at 4 °C. To calculate the heat absorbed by the water in calorimeter, use the formula (q = mCΔT). Plug in 50 mL for (m), 4.184 J for (C) and 4 °C for the initial temperature (ΔT), then multiply.
Temp: Mass of evap. dish: Mass of evap dish+contents: Mass of contents: Solubility g/100cm3 water
* pH of Solution: Water has pH of 7 at 25°C. As the pH decreases,
The purpose of this lab was to calculate the specific heat of a metal cylinder
In this lab, I determined the amount of heat exchanged in four different chemical reactions only using two different compounds and water. The two compounds used were Magnesium Hydroxide and Citric Acid. Both compounds were in there solid states in powder form. Magnesium Hydroxide was mixed with water and the change in heat was measured using a thermometer. The next reaction combined citric acid and magnesium hydroxide in water. The change in heat was measured as well. For the third reaction citric acid was placed in water to measure the change in heat. In the last reaction, citric acid was combined with water. The heat exchanged was again measured. It is obvious we were studying the calorimetry of each reaction. We used a calorimeter
from the work surface, if any. Our results are set out below. Time (mins) : 0 - Height from bench (cm) -.. Temperature reached (d. c.). Water Volume (cm cubed).
on how long it takes to heat up. If we heat a large volume of water it
The purpose of performing this lab was to find the specific heat capacity of an unknown metal.
To investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powder
Specific heat capacity of aqueous solution (taken as water = 4.18 J.g-1.K-1). T = Temperature change (oK). We can thus determine the enthalpy changes of reaction 1 and reaction 2 using the mean (14) of the data obtained. Reaction 1: H = 50 x 4.18 x -2.12.
The objective of this experiment was to identify a metal based on its specific heat using calorimetry. The unknown metals specific heat was measured in two different settings, room temperature water and cold water. Using two different temperatures of water would prove that the specific heat remained constant. The heated metal was placed into the two different water temperatures during two separate trials, and then the measurements were recorded. Through the measurements taken and plugged into the equation, two specific heats were found. Taking the two specific heats and averaging them, it was then that
be yes as I will then be able to use enthalpy change of reaction to
In a 100ml beaker 30mls of water was placed the temperature of the water was recorded. 1 teaspoon of Ammonium Nitrate was added to the water and stirred until dissolved. The temperature was then recorded again. This was to see the difference between the initial temperature and the final temperature.
My aim is to see the effects of a change in temperature on the rate of