Ashley Hensley_05_Enthalpy_PostLab_Spr24

Esc ||| = OTHERMOCHEMISTRY A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). Calculating heat of reaction from bomb calorimetry data First, a 5.000 g tablet of benzoic acid (C6H,CO₂H) 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 16.00 °C to 38.96 °C over a time of 9.2 minutes. 2 4. Next, 5.730 g of acetaldehyde (C₂H₂O) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 42.19 °C. 84°F Sunny Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: FI Explanation Is this reaction exothermic, endothermic, or neither? 4- F₂ Check 2C₂H4O(g) + 50₂(g) 4CO₂(g) + 4H₂O(g) Be sure any of your answers that are…

calculate the specific heat and the molar capacity, C of the metal (part 3). thank you!

Ma Nit ← → C esc 2 1 Ho Ph Ph app.101edu.co Week 4 Lab 3....docx 1 30 F1 Q NaCl(s) Determine the enthalpy of reaction for HCI(g) + NaNO₂(s) → HNO₂(1) + - 2NaCl(s) + H₂O(l) → 2HCI(g) + Na₂O(s) AH = -507.1 kJ/mol 2 NO(g) + NO₂(g) + Na₂O(s) → 2NaNO₂(s) AH° = -427.0 kJ/mol 2 NO(g) + NO₂(g) →→ N₂O(g) + O₂(g) AH° = -43.01 kJ/mol 2HNO₂(1)→ N₂O(g) + O₂(g) + H₂O(1) AH° = +34.02 kJ/mol 2 2 Ho F2 W # 3 X 00 80 F3 G wh $ 4 000 000 F4 wh tar W Hy Gwh (3. ill MA C % C 45 F5 Question 20 of 28 6 MacBook Air & 7 CHAP Gwr Gw G ch ch | D F7 * CO 8 DII F8 9 DD F9 1 4 7 0 +/- F10

Enthalpy of Combustion (AH): 1. An alcohol is burned, and the heat is transferred to a large calorimeter that contains 3.0 kg of water. This combustion used up 0.285 moles of the alcohol and the temperature of the water to rose by 36.00°C. What is the enthalpy of combustion (AHC) of this alcohol in kJ/mol? (Remember that 1 kg = 1000 g) 2. When 1.20 g of hexane (C6H₁4) are burned, the temperature of 250.0 g of water is raised by 56.0°C. What is the enthalpy of combustion (AHC) of hexane in kJ/mol? 3. Use the following experimental data to determine the enthalpy of combustion of propanol (C3H₂OH) in kJ/mol Mass of water = 200.00 g Initial water temperature = 18.2°C Final water temperature = 38.6°C Initial mass of alcohol lamp = 185.51 g Final mass of alcohol lamp = 184.56 g subtract for massof stuff Know kJofq + mass of stuff 4. A 2.50 g sample of sucrose (C12H22011) was burned in excess oxygen in a bomb calorimeter that was surrou by 2,190 g of water. The temperature of the water…

Yoshida, Dylan H-Outle X MBS Direct: Criminal Justice X B Dropbox Folders - 2020 FALLX + → C D 101 Chem101 G How much heat (in kJ) is absor app.101edu.co Apps MBS Direct: Crimin... Registrar Home MBS Direct: 40 Shor... G History of Criminol.. Criminologist Job D.. www.criminology.c... notedwastaken - T... Question 5 of 6 How many moles of KCIO, must be reacted according to the following balanced chemical reaction to transfer -34.2 kJ of heat? 2 KCIO:(s) - 2 KCI(s) + O:(g) AH = -89.4 kJ %3D STARTING AMOUNT ANSWER RESET ADD FACTOR *( ) -34.2 122.55 0.383 2 0.765 6.022 x 1023 1000 -89.4 0.001 3060 1 1530 74.55 32.00 mol KCIOS g KCIOS kJ mol KCI g KCI mol Oz Type here to search hp

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tml?ClassID=543616615# Calculate the enthalpy, in kJ/mol, for the combustion of the hydrocarbon from the data from the previous steps. 9cal = 6191.78 J n= 0.0019243682 mol AH = [ ? ] kJ/mol Enter either a + or - sign AND the magnitude. Give your answer to three significant figures. AH (kJ/mol) Enter

The combustion of one cubic foot of natural gas produces 1000. kJ of heat. Assume a 57% efficiency and determine how many cubic feet of natural gas must be burned to raise the temperature of 46 gallons of water in a hot water tank from 12.7°C to 90.0°C. Note: 1 gal = 3.79 L. (See the table.)

Part 1. Data Table mass of empty Styrofoam cup and lid mass of cup, lid and cool water temperature of cool water specific heat of water temperature of hot water mass of cup, lid and water mixture observed final temperature of mixture 11.355g 36-2439 4.184 Golfc 3. Percentage error of experiment. 88-0039 4760 Calculations (Carry out to the proper number of significant digits.) 1. Masses of hot water and cold water used. 2. Calculated final temperature of mixture. (Do not use your observed final temperature of mixture.)

my previous answer was -2.16*10^-3.

Per x M Inb x 31799#/7231799/2/0 ted 13 out of 16 16 P11 Essentials of General, Organic, and Biochemistry Denise Guinn THIRD EDITION The table lists the specific heat values for brick, ethanol, and wood. Specific Heats of Substances Substance Brick Ethanol Wood heat added: P S per: X 20 effe x CDC He: X JA 6 Specific Heat 0.20 0.58 0.10 B 10 X 4 gºC Calculate the amount of heat, in calories, that must be added to warm 96.8 g of brick from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. W 4 Calculate the amount of heat, in calories, that must be added to warm 96.8 g of ethanol from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. ○바 8 No X 9 EC eth X 0 Sm X 00 39 HR MIN SEC 0/R Sm x Resources + presented by Macmillan Learning G ا ا ا 200 L Next Qu cal 40 1