The Efficiency of Heating Using a Flame Thermodynamics II Contents Introduction 2 Observations 2 Time/Temperature readings 2 Time/Temperature Plot 3 Calculations and Results 3 1) Enthalpy change of gas burned over the duration of the test 3 2) Heat transfer to the water in the kettle (Qw) 4 3) Heat transfer to the water which evaporates from the kettle (Qev) 4 4) Heat transfer to the kettle from initial to final state (Qk) 4 Find‚ as a fraction of 1‚ the values
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specific heat (4.18 J for water)‚ g - grams of water and ΔT - change of the temperature; division by 1000 shows that the data is calculated in kJ. Also the number was divided by the amount of moles used in each trial (which is shown in the table above). The final amount of ∆H sol/mol of CuSO4 was calculated by finding the average of all 5 trials‚ which is 11.4 kJ/mol (±7‚91%). Experiment was done according to the equation below: 1) CuSO4-5H2O ----> CuSO4 (aq) + 5H2O The equation represents the
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Fuels Investigation Aim: To find out which fuel gives out the most energy. Planning We will be using 6 different fuels to heat up 100ml of water‚ and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes‚ and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula: Mass of water x 4.2 (water’s specific
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Chapter 1 Introduction and Basic Concepts 1-1 Thermodynamics and Energy Application Areas of Thermodynamics 1-2 Importance of Dimensions and Units Some SI and English Units Dimensional Homogeneity Unity Conversion Ratios 1-3 Systems and Control Volumes 1-4 Properties of a System Continuum 1-5 Density and Specific Gravity 1-6 State and Equilibrium The State Postulate 1-7 Processes and Cycles The Steady-Flow Process 1-8 Temperature and the Zeroth Law of Thermodynamics Temperature Scales The International
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CHAPTER 10 Liquids and Solids 1. Order the intermolecular forces (dipole-dipole‚ London dispersion‚ ionic‚ and hydrogen-bonding) from weakest to strongest . a) dipole-dipole‚ London dispersion‚ ionic‚ and hydrogen-bonding b) London dispersion‚ dipole-dipole‚ hydrogen-bonding‚ and ionic c) hydrogen-bonding‚ dipole-dipole‚ London dispersion‚ and ionic d) dipole-dipole‚ ionic‚ London dispersion‚ and hydrogen-bonding e) London dispersion‚ ionic‚ dipole-dipole‚ and hydrogen-bonding Ans: b 2. Hydrogen
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the enthalpy changes accompanying different neutralization reactions will be measured. It is because the number of moles of water formed varies according to the acid and alkali used‚ it is the convention to measure enthalpy change of neutralization in kJ mol-1 when 1 mole of water is formed. We will use a simple calorimeter to determine the enthalpy change of neutralization for the pairs of acid and base given. Apparatus and Materials: 1.0mol dm-3 sodium hydroxide solution‚ 1.0 mol dm-3 hydrochloric
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just plain play her--even someone as fine as her (ex) man KJ. And she knows how to survive the streets of Compton. The girl’s got it going on. What she doesn’t know is how to play the game at South Bay High‚ aka Drama High‚ a white school in Los Angeles where the kids keep looking at Jayd like she’s going to steal one of their rides. And that’s just the beginning of the drama that’s about to play out. After a summer of bliss kicking it with KJ‚ Jayd returns to South Bay High for what she hopes will
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of the forward reaction? A B C D decreasing the size of the catalyst pieces increasing the pressure increasing the temperature removing the ammonia as it is formed 3 The equation for a reaction is shown. H2(g) + 1 2 O2(g) → H2O(l) ; ∆H = x kJ mol–1 Which pair of descriptions is fully correct for this reaction? type(s) of enthalpy change A B C D 4 formation only formation only combustion‚ formation combustion‚ formation value
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Investigation Investigate the amount of heat evolved when magnesium reacts with dilute acids. Planning What I am going to do I am going to find out how much heat is given out when magnesium reacts with a variety of dilute acids. In order to make comparisons between the acids‚ I shall use my results to work out how much heat would be given out if 1 mole of magnesium reacted with an excess of each acid. The acids I shall use are hydrochloric acid‚ sulphuric acid‚ nitric acid and ethanoic acid
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The mixture will contain (A) He‚ Ne gases; Ar+‚ Kr+‚ Xe+ ions (B) He+‚ Ne+ ions; Ar‚ Kr‚ Xe gases (C) He+‚ Ne+‚ Ar+‚ Kr+‚ Xe+ gases (D) He+‚ Ne+‚ Ar+ ions and Kr‚ Xe gases (5) If EA1 and EA2 for oxygen atom are -142 kJ mol-1 and 844 kJ mol-1. The energy released to form 2 O + 2 e ( 2 O - will be (A) 986 (B) 702 (C) 284 (D) 1688 (6) Dipole moment of K+Cl- is 3.336 x 10-29 cm and it is 80 ionic in nature. The inter ionic distance between K+ and Cl-
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