atoms has more variations in how it can vibrate than a molecule with fewer atoms. This means more ways to distribute energy- or greater energy dispersal at any given temperature and larger entropy. A2. ΔGo for reaction A is -50 kJ mol-1. ΔGo for reaction B is -75 kJ mol-1. Which reaction is faster? How do you know? Nothing can be said about the rates of these two reactions. G is a state function and does not depend on the reaction rate. A3. Why are condensed phases such as solids and pure
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solutions is 25.3ºC. Calculate the qsol using equation 1 (qsol = grams of solution x specific heat of solution x ΔT). Answer in kJ. q = mCΔT q = (50.09)(4.18J/g ºC)(3.9ºC) 0.82kJ 5. What is the qrnx ? -qsol = qrnx -0.82 kJ 6. If the reaction described in #4 used 0.15 moles of B‚ calculate ΔHrxn by dividing kJ by moles. ΔHrxn = -0.82 kJ / 0.15 mol ΔHrxn = -5.5 kJ/mol IV. Procedures Measure 50.0 mL of a 2.0 M HCl solution in a graduated cylinder prior to transferring to the calorimeter
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Calorimetry: Enthalpy of Neutralization Introduction: The purpose of this lab experiment was to determine the molar concentration of the unknown HCl by using a coffee cup calorimeter. A coffee cup calorimeter is made of Styrofoam cups with a thermometer that is placed from the top and into the calorimeter to measure the temperature as the reaction happens. The Styrofoam cup used for the calorimeter creates an isolated system as it acts as a heat insulator between the cup and the surrounding
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Experiment 9 Aim A. To investigate the existence of hydrogen bonds between ethanol molecules. B. To measure the strength of hydrogen bond formed between ethanol molecules C. To investigate the formation of hydrogen bonds between molecules of ethyl ethanoate and trichloromethane. D. To measure the strength of hydrogen bond formed between molecules of ethyl ethanoate and trichloromethane. Procedure A. 1. 10 cm3 of ethanol was added into an insulated 50 cm3 beaker by
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Background As a child I would always place myself in the overweight category. I generally found it very difficult to eat real food I would always find myself snacking away on junk food when I was hungry. I recognized I had a problem with my weight at the age of 16. At the age of 14 I was actively participating in sporting activities and played rugby league for several years. It was my years of playing league that made me distinguish that maybe I was doing something wrong; that is the reason I
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Experiment 1: Calorimetry Nadya Patrica E. Sauza‚ Jelica D. Estacio Institute of Chemistry‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines Results and Discussion Eight Styrofoam ball calorimeters were calibrated. Five milliliters of 1M hydrochloric acid (HCl) was reacted with 10 ml of 1M sodium hydroxide (NaOH) in each calorimeter. The temperature before and after the reaction were recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature
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Practice Exam Chapter 8 I have put the questions we may not get to for this exam at the end of the practice exam) 1. How many lone pairs of electrons are assigned to the sulfur atom in H2S? a) 0 b) 1 c) 2 d) 3 e) 4 2. Which of the following is a correct Lewis structure for nitrous acid‚ HNO2? 3. The central atom in PH3 is surrounded by a) three single bonds and no lone pairs of electrons. b) three single bonds and one lone pair of electrons. c) three single bonds and two lone
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OBJECTIVE The main purpose of this experiment is:- i. To demonstrate the working principles of industrial heat exchangers ii. To investigate the efficiency of the heat exchanger in parallel and counter flow arrangements 1.0 INTRODUCTION A heat exchanger is equipment in which heat exchange takes place between 2 fluids that enter and exit at different temperatures. The main function of heat exchanger is to either remove heat from a hot fluid or to add heat to the cold fluid. The direction
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SCH 4U1 FINAL EXAM REVIEW ATOMIC STRUCTURE AND MOLECULAR ARCHITECTURE 1. Describe the wave mechanical model of the atom. 2. Write the ground state electron configuration for Br. 3. Explain why the first ionization energy for Ne is significantly greater than Na. 4. Distinguish between ionization energy and electronegativity. 5. How does VSEPR Theory account for the fact that the bond angle in H2O is less than NH3? 6. Which of the following molecules are polar? Include diagrams
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The Increasing Enthalpy of Combustion Rates for Pentanol Isomers EEI Report Draft - JEREMY SAJU 11B Fuels are the main energy source of the modern world. The topic of this extended experimental investigation is to explore combustion rates of alcohols‚ specifically pentanol and it’s relationship with varying structural isomers. A fuel is defined as a material that stores potential energy that‚ when released‚ can be used as heat energy (Chemguide‚ 2003). The balanced combustion equation for pentanol
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