Calorimetry Group Proposal v2.2

Gaseous water (H20) and solid magnesium oxide (MgO) are formed by the decomposition of solid magnesium hydroxide (Mg(OH),). Write a balanced chemical equation for this reaction. O-a Co S ? X 201 McGrawHl Educaion Al Rights Continue MacBook Pro

Peisalla lamacron Nar. ,202 Date Name Section galauvinstenos Pre-Laboratory Assignment 1. Read an authoritative source for a discussion of preparing and interpreting a graph, especially the extrapolation of a curve. 2. A student determined the calorimeter constant of the calorimeter, using the procedure described in this module. The student added 50.00 mL of cold water to 50.00 mL of heated, distilled water in a Styrofoam cup. The initial temperature of the cold water was 21.00 °C and of the hot water, 29.15 °C. The maximum temperature of the mixture was found to be 24.81 °C. Assume the density of water is 1.00 g mL¯1 and the specific heat is 4.184 J g¯K gniwollot bns of toh bine botollon ot ssb om (1) Determine the AT for the hot water and the cold water. mit At cold water = 24.8I- 21,00 = 3.81°COn आनी AT hot = 24.81- 29.15 = - 4.34°C 60.ES 2.0 0LES 8. 0.1 0.0 If 0.8 28.5S Calculate N 0.4 08.TT gabxim 02 4.34°C hot water 81 answer cold water 381°C dogesn boximnu sdt to anuiSTeqmad mom…

Anna was asked to identify and explain if the equation CO2 (1)-CO2 (g) was an endothermic or exothermic reaction. However she got it wrong. What is her error and what should the answer have been? Anna's statement : The equation is an endothermic reaction because the energy is released from gaseous CO2 to the surroundings to become liquid CO2 causing the molecules to slow down. earch a inse # % & 3 4 7 8 9 E R Y P D G H J L V BN M alt

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…

ORT SHEET Heat of Neutralization EXPERIMENT elemsboomfchg lom 12 A. Heat Capacity of Calorimeter 1. Temp. of calorimeter and water before mixing 2. Temp. of warm water °C 22.0 39,0 30.3 3. Maximum temp. determined from your curve °C 4. Heat lost by warm water (temp decrease x °C 50.0 g x 4.184 J/K-g) = 02), 5. Heat gained by cooler water (temp. increase x 50.0 g x 4.184 J/K-g) = 30,3 22.0)x 13626J s0.0gmpi S0.0gy 6. Heat gained by the calorimeter [(4) – (5)] = 7. Heat capacity of calorimeter: heat gained by the calorimeter temperature increase J/K 3. Heat of Neutralization of HCl-NaOH 22.2 22.2. °C . Temp. of calorimeter and NaOH Temp. of HCI AT determined from your curve after adding HC1 °C to the NaOH Heat gained by solution (temperature increase x ON 100 g x 4.184 J/K-g) = 9977.8J %3D Heat gained by calorimeter (temperature increase x heat capacity of calorimeter) = J %3D Total joules released by reaction [(3) + (4)] = Tight O 2018 Pearson Education, Inc.

Write the chemical formulas for the products formed when each of the following hydrocarbons undergoes complete combustion. For each part, there are two answers.  Input one chemical formula in each blank.  Order doesn't matter. Do NOT include equation coefficients, ONLY the two products When typing a compound formula, use an underscore "_" to depict a subscript for example for K2CO3 you would type K_2CO_3 a)  C2H4         b)  C7H8

In part 1 of this lab, you will be calculating A-H by conducting constant-pressure calorimetry measurements. One of the final steps in this calculation is obtaining A,H by taking the q value (with respect to the system) and dividing by n. What number of moles (n) will you be using in the above formula? Select one: O Number of moles of magnesium, since Mg is in the balanced chemical equation and is a part of the system O Number of moles of water

education.wiley.com + 00 D2L Topic 4 (Chapter 3 and 12) Online Home... W NWP Assessment Builder UI Application W NWP Assessment Player UI Application C Question 17 Of 50 -/1 = View Policies Cur... b Similar Questions | bartleby E Topic 3 (Chapter 3 and 12) Online Homework Assignment Question 15 of 50 0/1 E View Policies Show Attempt History Current Attempt in Progress Incorrect. Write a balanced equation for the formation reaction of each of the following substances: (a) K3PO4(s) (b) acetic acid, CH3CO2H(I) (c) trimethylamine, (CH3)3N(g) (d) bauxite, Al203(s) eTextbook and Media Save for Later Attempts: 1 of 3 used Submit Answer

= 14 15 16 17 18 19 20 21 22 23 24 25 26 thermometer A 52.3 g sample of quartz is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The quartz sample starts off alo insulated container at 90.2 °C and the temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 29.6 °C. The pressure remains constant at 1 atm. water Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to 2 significant digits. sample a calorimeter J ?

Course Home Course Home Syllabus Scores Pearson eText Document Sharing User Settings Course Tools 76°F Mostly sunny X Qbartebly - Search b My Questions | bartleby x + https://openvellum.ecollege.com/course.html?courseld=17044720&OpenVellumHMAC=02ab23286d132bee2c1ff7fb0c33c5f5#10001 Problem 12.50 Part A Zinc sulfide, ZnS, crystallizes in a face-centered cubic unit cell where the cations occupy one of the two types of tetrahedral holes. How many Zn²+ ions touch each S2-ion? Express your answer as an integer. ΨΕ ΑΣΦ S Zn > Submit Request Answer Part B How many S2 ions touch each Zn²+ ion? Express your answer as an integer. IVE ΑΣΦ Request Answer Submit < Return to Assignment Provide Feedback Pearson ? ions ? ions A o 7 of 7 Review | Constants | Periodic Table 5:39 PM 5/31/2022 E

Answer in 2 sig figs, thank you!

PERFORMANCE TASK 4.4 (CHEMICAL EQUATION) MELC: Apply the principles of conservation of mass to chemical reactions. (S10MT-IVe-g-23) GO REACT! DIRECTIONS: 1. Write the symbols to complete chemical equation inside the box. 2. Balance the chemical equations by writing its coefficient on the space provided beside the box. 3. Determine the type of reaction in each item. A. Chemical Reactions: 1. Magnesium combines with chlorine gas to produce magnesium chloride. Mg + Type of Reaction: 2. Sodium reacts with copper sulfate and forms sodium sulfate and copper. 2 Na + C² 99 → Na₂SO4 Type of Reaction: 3. Mercury (11) oxide, a red solid, decomposes when heated to produce mercury and oxygen gas. HgO 2 + Type of Reaction: 4. Lead(II) nitrate and potassium iodide give lead(11) iodide and potassium nitrate. Pb(NO3)2 + Pbl₂ +2 Type of Reaction: gas and water 5. Ethane reacts with oxygen gas produces carbon dioxide C₂H6 + CO₂ +6 Type of Reaction: 6. The reaction of hydrochloric acid, with magnesium…

Pre-Laboratory Assignment 1. Sam performed a reaction in lab where he mixed a dilute solution of hydrochloric acid into a dilute solution of sodium hydroxide. The temperature of the mixed solution rose immediately from 20.0°C to 30.0 °C. Was the reaction Sam performed in the lab exothermic or endothermic? What evidence (observation) for this reaction supports your inference? 2. Define Hess's Law. 3. Predict the target reaction which can be obtained by adding step 1 and 2 shown below. Also calculate the heat of reaction of the target reaction, which can be obtained by AH" from step 1 and 2. Step 1 2 Hy(g) + N>(g) N,H,(g) AH = 95.4 Step 2 NgH,(g) + Ha(g) 2 NH3(g) AH" =-187.6 kJ kJ 81

Make a scatter plot of temperature vs time (x-axis). Then determine the initial temp of the water inside the calorimeter, the final temperature of the water and the calorimeter and indicate the time of mixing on the plot.

17

please answer

Acetic acid and ethanol react to form ethyl acetate and water, like this: HCH,CO,(aq)+C,H,OH(aq) → C,H,CO,CH,(aq)+H,O() Imagine 231. mmol of HCH3CO₂ are added to a flask containing a mixture of HCH³CO₂, C₂H²OH, C₂H²CO₂CH3 and H₂O at equilibrium, and then answer the following questions. What is the rate of the forward reaction before any HCH3CO₂ has been added to the flask? What is the rate of the forward reaction just after the HCH3CO₂ has been added to the flask? What is the rate of the forward reaction when the system has again reached equilibrium? How much more HCH3CO2 is in the flask when the system has again reached equilibrium? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater…

Please refer to the attached photo. Thank youuu

Please help

Нурothesis Theory Law Answer Bank Scientists, after many experiments, An untested explanation. An explanation that has been A doctor thinks, but has explain how the temperature of a gas tested and verified. not verified, why a patient depends on the energy of its molecules. has stomach pain. A description that predicts what happens, but does not explain how.

be Maps O GASES Understanding how average molecular kinetic energy scales wi... Lindsay Five samples of neon gas are described in the table below. Rank the samples in order of increasing average kinetic energy of the atoms in them. That is, select "1" next to the sample in which the neon atoms have the lowest average kinetic energy. Select "2" next to the sample in which the neon atoms have the next lowest average kinetic energy, and so on. sample average kinetic energy of atoms in sample amount pressure temperature 2.4 mol 1.3 atm - 73. °C (Choose one 2,2 mol 2.5 atm -61. °C |(Choose one) v

I Review | Constants | Periodic Table Open the activity depicting Hess's Law. Part B N: (g) + 0: (g) 2NOg) AH is an Extensive Property + N: ) +0:() → NO(g) AH Changes sign when a Click on the process is reversed screen when you started and its derivative demonstrate that the reaction enthalpy, AH, changes sign when a process is reversed. button within the activity and analyze the relationship between the two reactions that are displayed. The reaction that was on the AH Canges sign when a process is reversed 2NO(g) → N:(gì + 0: (g) Consider the reaction Hess Law of Constant icat Sumnation + N: (g) +0: (g) – d NQ +0:() B's) + 302(g)—B>0ҙ(s), дн — -1270KJ When two reactions are added together. the individual reaction enthalpies are summed. Notice that equal quantities of the same species, on both sides of the reaction arrow, cancel. → NO: g What will AH be for the reaction if it is reversed? + N: (g) + O: (g → NO: (g) Express your answer with appropriate units. • View Available Hint(s) µA…