• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

Investigation of Enthalpy Change When Mg is added to HCl

Extracts from this document...

Introduction

ï»¿Investigation of Enthalpy Change When Mg is added to HCl Defining the Problem and Selecting Variables Research Question: How is the enthalpy change of the reaction between Mg and HCl affected when different amounts of Mg are added to a constant amount of HCl? Variables: Independent: Mg Dependent: Temperature Control: HCl Controlling Variables I will use three different masses of Mg: 0.02g ± 0.001g, 0.03g ± 0.001g, 0.04g ± 0.001g I will measure the temperature using a colorimeter made from a foam cup, a lid, and a thermometer I will keep HCl at a constant volume of 10mL of 1M HCl Procedure: Step 1: Measure out 10mL of 1M HCl Step 2: Pour HCl into foam cup and place lid on cup Step 3: Measure the initial temperature and record data Step 4: Add in 0.02g of Mg into cup and measure the finial temperature Step 5: Calculate change in temperature by ...read more.

Middle

10°C ± 0.1°C 9°C ± 0.1°C 7°C ± 0.1°C 13°C ± 0.1°C 11°C ± 0.1°C 11°C ± 0.1°C 16°C ± 0.1°C 15°C ± 0.1°C 17°C ± 0.1°C Calculations: When a sample of Mg dissolves in 10mL HCl, the temp increases. The following are the ΔH of the 9 trials: Equation: q=mcΔT Trial 1 0.02g ± .001g Mg 1. (10mL)(4.184)(10°C)= 418.4 Qw= = -0.4184 0.02g Mg (= 0.0008 -0.4184/0.0008= -523 kJ/mol 1. (10mL)(4.184)(9°C)=376.56 Qw== -0.37656 0.02g Mg (= 0.0008 -0.37656/0.0008= -470.7 kJ/mol 1. (10mL)(4.184)(7°C)= 292.88 Qw== -0.29288 0.02g Mg (= 0.0008 -0.29288/0.0008= -366.1 kJ/mol Average of trial 1 is 453.27 kJ/mol Trail 2 0.03g ± .001g Mg 1. (10mL)(4.184)(13°C)=543.92 Qw== -0.54392 0.03g Mg (= 0.0012 -0.54392/0.0012= -453.3 kJ/mol 1. (10mL)(4.184)(11°C)=460.21 Qw== -0.46021 0.03g Mg (= 0.0012 -0.46021/0.0012= -383.5 kJ/mol 1. (10mL)(4.184)(11°C)=460.21 Qw== -0.46021 0.03g Mg (= 0.0012 -0.46021/0.0012= -383.5 kJ/mol Average of Trial 2 is 406.77 kJ/mol Trail 3 0.04g ± .001g Mg 1. ...read more.

Conclusion

Now the answer to the question -How is the enthalpy change of the reaction between Mg and HCl affected when different amounts of Mg are added to a constant amount of HCl? - Is there is an effect to the enthalpy change when different amounts of Mg are added but it is irregular and the change in the enthalpy isn?t steady in its rise or decline. The experiment was done using different foam cups and a calorimeter and the amount of time that the chemicals temperatures were recorded were different. If I was to improve this experiment I would use the same kind of foam cups and lids for each trial and I would also measure the temperature for each chemical under a specific time limit which would be the same for each trial. Investigation of Enthalpy Change When Mg is added to HCl Kerolin Francois Lab Report IB Chemistry Period 4 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

Related International Baccalaureate Chemistry essays

1. Hesss Law Lab, use Hesss law to find the enthalpy change of combustion of ...

They are listed as under: Improvements: � It is extremely important to minimize the heat loss from the system to the surrounding during the experiment. We should have an advanced isolated system which will be able to prevent any heat loss to the surroundings.

2. Thermodynamics: Enthalpy of Neutralization and Calorimetry

heat of neutralization with the formula q neutralization cal = (m �?T � s)Solution + (Heat Capacity � ?T)calorimeter Results The data presented below is relevant to Trial 1 of the experiment. These calculations also include uncertainty and the propagation thereof.

1.  Vitamin C in Fruit Juices

10.0 mg x mg 33.78mL = 12.61mL 10.0 mg x mg x mg = 12.61mL 33.78ml = 3.73mg/10.0ml = 0.373mg/ml DISCUSSION: Analysis Results show that, in experimental conditions, all fruit juices contained more than the amount of vitamin C stated on the juice box per serve.

2. Enthalpy Change Design Lab (6/6)How does changing the initial temperature (19C, 25C, 35C, and ...

or HCl(aq) is negligible itself - even more so considering the dilute concentration being used in the investigation. Another component of measuring the molar enthalpy change of a neutralization reaction is the change from the initial temperature of the reactants, to the final temperature of the resulting solution.

1. Group 4

This is because during a collision all the energy of the impact went directly to the vehicle and onto the passengers. In 1967, the Mercedes Heckflosse was the first mass production car in the world to feature "crumple zones" and a safety cage.

2. Titration of Na2CO3.xH2O with HCl

Where the no. of moles = concentration (mol dm-3) � Volume (dm3) (Let C2 be the concentration of Na2CO3) Therefore, [0.1 mol dm-3 � (0.0248 � 0.0001) dm3] � [C2 � (0.025 � 0.00005) dm3] = 2 � 1 C2 = [0.1 � (0.0248 � 0.0001)] � [2 � (0.025 � 0.00005)] C2 = (0.00248 � 0.40%)

1. The aim of this experiment is to examine the enthalpy of combustion of the ...

the sequence of exothermic chemical reactions between a fuel and an oxidant accompanied by the production of heat and conversion of chemical specie ) of a primary alcohol increases . This means that as the number of carbon- carbon bonds increase, with the increase in the carbon chain length, more

2. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

This means that the heat produced if all 0.05g would be Mg would be greater than that recorded and therefore, the value of Q (heat produced by 0.05g of Mg) is understated. To overcome this common oxide problem, the strip should be sanded off of its oxide coating using a sand paper. • Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to
improve your own work 