Prakhar+Dubey

(Reaction between HCL and NAOH)**
 * Chemistry Experiment 5

 Aim : Calculate the heat realeased in reaction of HCL and NAOH Things needed : beaker, dropper, thermometer and measuring cylinder,b **eam Balance, NAOH (2 mol) and HCL (2 mol) 
 * 

Procedure:
 * Record mass of a empty beaker
 * Put 25 cc of HCL in another beaker
 * Put 25 cc of NAOH in again a different beaker
 * Now measure the initial temperature of both the chemicals
 * Now take the empty beaker and add HCL and NAOH and immediatly place a thermometer
 * Measure the temperature till the experiment ends
 * Now measure the mass of beaker with the chemiacals

= = =** Chemistry Experiment 4 (Cuso4 + Zn) Aim: To find the amount of heat produce in a exothermic reaction between CuSO4 and Zn  Things required: thermometer, measuring cylinder, stop watch, beam balance, beaker, dropper, zinc and copper sulphate. Procedure: Take Cuso4 in beaker and measure the starting temperature.Take zinc granules and crush them with mortar and pestle. Now add Cuso4 and Zn and immediately start the stop clock. Then measure the temp. at 30s interval and **** calculate the amount of heat given by formula heat **=
 * mass of reagent x specific heat x defference in temperature / number of moles.****

Chemistry Experiment 3 **

(Reaction Between Calcium Carbonate and Hydro Chloric Acid)
** Aim: **To find the difference in time to reach the emission of carbon dioxide gase till 100000 pps with different masses of calcium carbonate. Prediction: **The more we put calcium carbonate in constant HCl it take more less time to emit 100000 pps carbon dioxide. Observation: ** Taking masses of calcium carbonate 0.5 g 1 g 1.5 g2 g 2.5 g and 50 cm3 of HCl
 * Things Required: **Beam Balance, Data Logos with carbon dioxide sensor, Laptop, Beaker, Spatula and measuring cylinder.
 * Reagent Required:**Calcium carbonate and HCl Acid (1 mol)
 * Procedure:**
 * Install Data logos software in your laptop.
 * measure the different masses of calcium carbonate and record it, atleast take 3
 * Then take 50 cm3 of HCl and in a beaker.
 * Prepare the data logos with a carbon dioxide sensor and connect it to laptop.
 * Put the HCl in CO2 sensor beaker.
 * Put calcium carbonate in that beaker.
 * Than immediately put CO2 sensor in that beaker and immediately start collect in your laptop in data logos software.
 * Graph will be plotted on your laptop.
 * Then use different mass of calcium carbonate with 50 cm3 of HCl, so different graph will be plotted, repeat this at least 3 times with different masses.
 * 

Chemistry Experiment 2

(Endothermic Reaction between Sodium Bicarbonate and Citric Acid)
** Aim: **__To find the difference in temperature, when different molarity of Citric acid was added to Sodium Bicarbonate.__ Prediction: **<span style="-webkit-text-decorations-in-effect: none; color: #000000; display: inline; font-family: Arial,Helvetica,sans-serif; font-size: 13px; font-weight: normal; line-height: 20px; text-align: left;">__As it’s endothermic reaction so, it absorb the heat, therefore the more we use the molarity of Citric acid, the more the temperature goes down.__
 * Things Required: **<span style="-webkit-text-decorations-in-effect: none; color: #000000; display: inline; font-family: Arial,Helvetica,sans-serif; font-size: 13px; font-weight: normal; line-height: 20px; text-align: left;">__Beam Balance, Data Logos with temperature sensor, Laptop, Beaker, Spatula and Water.__
 * Reagent Required:**<span style="-webkit-text-decorations-in-effect: none; color: #000000; display: inline; font-family: Arial,Helvetica,sans-serif; font-size: 13px; font-weight: normal; line-height: 20px; text-align: left;">__Sodium Bicarbonate and Citric Acid__


 * Procedure:**
 * <span style="color: #000000; display: block; font-family: Arial,Helvetica,sans-serif; text-align: left;">Install Data logos software in your laptop.
 * <span style="color: #000000; display: block; font-family: Arial,Helvetica,sans-serif; text-align: left;">Prepare different molarity of citric acid using different mass of it and 100 cm3 of water. At least take 5 different molarity.
 * Then take 60 cm3 of a molarity in beaker.
 * Prepare the data logos with a temperature sensor and connect it to laptop.
 * Put the temperature sensor in beaker.
 * Then in your laptop, in data logos software start collect.
 * After 2 or 3 sec put 5 gm of sodium bicarbonate in a beaker.
 * Graph will be plotted on your laptop.
 * <span style="color: #000000; display: block; font-family: Arial,Helvetica,sans-serif; text-align: left;">Then use different molarity different graph will be plotted, repeat this at least 5 times with different molarity

__**Chemistry Exp 1**__

<span style="font-family: 'Times New Roman',Times,serif; font-size: 18pt;"> ** AIM ** : To observe the endothermic reaction between sodium bicarbonate and citric acid.

** THINGS REQUIRED ** : Beakers, disposable cup, digital weight balance, citric acid, sodium bicarbonate, measuring cylinder, data logger and computer.

** PROCEDURE: ** Take 2.1, 4.2, 6.3, 8.4 and 10.5 grams of citric acid and mix them with 100cc of water to make different solutions of different molarities.

Take sodium bicarbonate and make five pouches of it containing 5 grams of NAHCO3 in each of it.

Correctly assemble the data logger and prepare it for the experiment.

Take 0.1 molarity of solution and pour the 5gram of sodium bicarbonate in the solution and quickly place the data logger and press collect.

Repeat the above statement with other molarities solution in a particular time period and notice the changes in graph obtained on the screen.

**Observation:** When the reaction started between the citric acid and sodium bi carbonate effervescence was observed and since it was an endothermic reaction heat was lost.


 * Conclusion: ** At higher concentrations of citric acid more heat is lost which can be seen in the graph.


 * Precautions: ** While weighing the citric acid powder, use only a piece of paper as the base.


 * mass of citric acid / g ||  || volume on water/cc ||   || concentration / mol ||


 * 2.1 ||  || 100 ||   || 0.1 ||


 * 4.2 ||  || 100 ||   || 0 .2 ||


 * 6.3 ||  || 100 ||   || 0.3 ||


 * 8.4 ||  || 100 ||   || 0.4 ||


 * 10.5 ||  || 100 ||   || 0.5 ||