A student modeled the exothermic synthesis reaction that occurs when solid iron and liquid sulfur chemically react to produce solid iron (ii) sulfide. The chemical reaction and the student's model are shown below. The student's model is incorrect. Identify two things in the model that need to be corrected. Explain why they are wrong and how the student needs to correct them. Fe (s) + S (1) → FeS (s) Before After Fe S Fe Potential Energy: Kinetic Energy: Potential Energy: Kinetic Energy: System Surroundings System Surroundings System Surroundings System Surroundings

A student modeled the exothermic synthesis reaction that occurs when solid iron and liquid sulfur chemically react to produce solid iron (ii) sulfide. The chemical reaction and the student's model are shown below. The student's model is incorrect. Identify two things in the model that need to be corrected. Explain why they are wrong and how the student needs to correct them. Fe (s) + S (1) → FeS (s) Before After Fe S Fe Potential Energy: Kinetic Energy: Potential Energy: Kinetic Energy: System Surroundings System Surroundings System Surroundings System Surroundings

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Constants | Periodic Table Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: Part B AHm = En,AH: (products)- E n,AH (reactants) For the reaction given in Part A. how much heat is absorbed when 3.50 mol of A reacts? where n represents the stoichiometric coefficients. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) Value Units Submit Previous Answers X Incorrect; Try Again; 29 attempts remaining Provide Feedback Pearson O 1:35 21
Try Again Row 3: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 7.000 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 15.00 °C to 53.26 °C over a time of 12.3 minutes. Next, 5.420 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 74.42 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or…
Consider these reactions, where M represents a generic metal. 2 M(s) + 6 HCI(aq)→ 2 MCl,(aq) + 3 H, (g) AĦ1 = -918.0 kJ 1. HCI(g) → HCI(aq) AH = -74.8 kJ H2(g) + Cl,(g) → 2 HCI(g) AH3 = -1845.0 kJ 3. MCI3(s) –→ MCl,(aq) AHA -380.0 kJ 4. Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl,(g) → 2 MCI,(s) 2.
A student is asked to identify an unknown piece of metal. The metal has a mass of 12.34 g. It is placed in a boiling water bath and brought up to 99.98 oC. A coffee-cup calorimeter is set up with 103.25 mL of water (density = 1.00 g/mL and specific heat = 4.184 J/g.oC) at a room temperature of 21.30 oC. The metal is removed from the boiling water and placed in the calorimeter. A final temperature is recorded as 22.32 oC. Find the specific heatcapacity of the unknown metal. (Assume there is no heat loss)
Rachel West Section 017 A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as ie reaction proceeds. Is this reaction endorhermic or exothermic? Describe if heat energy is lost or gained Trom the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the cemperature of the surrounding solution increase or decrease as a result of this chemical process?
When sulfuric acid is poured on sugar the volume expands, it turns black and gets very hot. Which of the following best describes this reaction? endothermic exothermic decomposition synthesis
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22. Statement A: The system loses 726 J to the surroundings as heat. The enthalpy change for the system is positive. Statement B: The system absorbs 178 J to the surroundings as heat. According to sign conventions heat is negative. Which of the following conclusions is correct about statements A and B? Group of answer choices Statement A is incorrect, Statement B is correct. Both statements are correct. Both statements are incorrect. Statement A is correct, Statement B is incorrect.
A chemist burned a sample of coal in a bomb calorimeter. Her results are below. Calorimeter's Heat Capacity 7.264 kJ/°C Mass of Coal Initial Temperature Final Temperature 0.100 g 22.07°C 25.37°C The sample of coal that the chemist placed in the bomb was dry but when she finished the test there was a small amount of water in the bomb. Where did this water come from and how does it affect her result? The water came from the water surrounding the bomb so her measured heat of combustion is for a closed system. The water was a product of combustion so her measured heat of combustion is for an open system. The water came from the water surrounding the bomb so her measured heat of combustion is for an open system. The water was a product of combustion so her measured heat of combustion is for a closed system.
A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt? How many moles of the unknown salt were used in the reaction ? _______ J?
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.