F2▼Part AFor a process at constant pressure, 12,400 calories of heat are absorbed. This quantity of heat is equivalent to5.19 x 104 J.O2.96 x 103 J.O 1.92 x 10-5 J.O 1.24 x 104 J.Submit Request AnswerProvide Feedback#3сSearch or type URL88888888&67$4%►5Course HomeMacBook Pro*9

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F 2 ▼ Part A For a process at constant pressure, 12,400 calories of heat are absorbed. This quantity of heat is equivalent to 5.19 x 104 J. O2.96 × 103 J. O 1.92 × 10-5 J. 1.24 x 104 J. Submit Request Answer Provide Feedback # 3 с $ 4 Search or type URL 8888888 & 6 7 % 5 ▸ Course Home MacBook Pro A 9

F 2 ▼ Part A For a process at constant pressure, 12,400 calories of heat are absorbed. This quantity of heat is equivalent to 5.19 x 104 J. O2.96 × 103 J. O 1.92 × 10-5 J. 1.24 x 104 J. Submit Request Answer Provide Feedback # 3 с $ 4 Search or type URL 8888888 & 6 7 % 5 ▸ Course Home MacBook Pro A 9

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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1.Given reactions A - C, determine the the change in enthalpy (kJ) for the reaction between C(s) + H2(g). Do not type units into your answer. C(graphite) + 2 H2(g) ⟶⟶ CH4(g) Δ?=?ΔH=? A. C(graphite) + O2(g) ⟶⟶ CO2(g) Δ?=−393.51??ΔH=−393.51kJB. H2(g) + 1/2 O2(g) ⟶⟶ H2O(l) Δ?=−285.83??ΔH=−285.83kJC. CO2(g) + 2 H2O(l) ⟶⟶ CH4(g) + 2 O2(g) Δ?=890.30??ΔH=890.30kJ 2. Based on your answer to the previous problem, determine the value of q (kJ) if 5.08 grams of methane (CH4) gas is produced from graphite and hydrogen gas. Do not type units into your answer.
+Tools - 4 of 7 - + & 8C 11. When 0.10 moles of butane, CAH10, are combusted in a bomb calorimeter, the temperature of the system increases by 8.5°C. If the system has a heat capacity of 34 kJ/°C, what is the heat of combustion of butane in kJ/mol CaH10? Que Bomb Calorimeter Thermometer Water Bomb Reaction A AHcomb = -290 kJ/mol C4H10 B AHcomb = -2900 kJ/mol CaH10 Question C AHcomb = 290 kJ/mol CaH10 O A D AHcomb = 2900 k)/mol CAH10 Activate Go to Settin C2021lluminate EducationT Inc. e DELL F6 a F7 F8 F9 F12 Insert FS F10 Esc F11 PriScr F1 F2 F3 F4 %23 %24 13 4 10 Tab E R OP Lock S K C Alt Alt つ
s_engine.html?ClassID=824851601# The calorimeter begins at the same temperature as the water, 22.0 °C and warms to the same temperature as the water, 62.7 °C. The heat capacity of the calorimeter is 9.3 J/°C. What is the heat change for the calorimeter? ¶Cal = [?]J %3D Enter either a + or - sign AND the magnitude. q,cal (J) Enter
Try Again Your answer is incorrect. Using the table of standard formation enthalpies that you'll find under the ALEKS Data tab, calculate the reaction enthalpy of this reaction under standard conditions: 2 C₂H6(g)+70₂(g) →4 CO₂(g) + 6H₂O(1) Round your answer to the nearest kJ. -3119 kJ x10 X 5
a system does 596 kJ of work and loses 276 kJ of heat to the surroundings. What is the change in internal energy, E, of the system? Not that the internal energy is symbolized as U in some sources. E= _______ kJ
Help with number 3 please
1) PCI3(1) + Cl2(g) - PCI5(g) Jse equations (2) and (3) to calculate AHrxn of equation (1): 2) P4(s) + 6Cl2(g)→ 4PCI3(1) AH =-1280 kJ 3) P4(s) + 10C12(g) → 4PCI5(g) AH =-1774 kJ
Use the data to answer only Reaction A.
Pls answer number 1 thank you.
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A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 6.10 kg of water at 27.1 °C. During the reaction 116. kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18 J-g¹K¹. Round your answer to 3 significant digits. [1] °C 0.0 X