3.DETAILSPREVIOUS ANSWERSMY NOTESASK YOUR„A.27.3 g.sample of ethylene glycol, a car radiator coolant, loses 695 J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5°C (c of ethylene glycol = 2.42 J/g•K)?Yöur response differs from the correct answer by more than 10%. Double check your calculations.°CSubmit Answer

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Answered: DETAILS PREVIOUS ANSWERS MY NOTES ASK…

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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For the combustion of methane(CH4) CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H = -882 kJ/mol If 250.0 g of CH4 is burned , what is the energy change? ( Answer in Kj. Answers in scientific notation are entered such as 1.234 e4 )
Methane, CH4, reacts with oxygen to produce carbon dioxide, water, and heat. CH4(g) + 202(g) CO2(g) + 2H20(1) AH= -890.3 kJ --- -- What is the value of AH if 5.00 g of CH4 is combusted? Select one: O a. -445 kJ O b. -157 kJ O C. -277 kJ O d. -714 kJ
BE’s are: C=O 799, C–H 413, O–H 467, O–O 498, H–H 432 kJ/mol CO2(g) + 4H2(g) → CH4(g) + 2H2O(g) ΔHrxn° = ___ kJ (from ΔHf°s) ΔHrxn°(BE) = ___ kJ (from BEs) = (2x799+432-4x413-4x467) CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ΔHrxn° = ___ kJ (from ΔHf°s) ΔHrxn°(BE) = ___ kJ (from BEs) ...Calculate ΔHrxn°s from both!
Hi, hope you're doing great. I just need help with these 2 questions. Thank you.
For the following reaction, what mass, in g, of ammonia is required to produce 375.0 kJ of heat? 4 NH3 (g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) - 906 kJ/ mol ΔΗ Your Answer: Answer units
What is the calorimeter constant (J/°C)if qice = 7269.11J, volume of water = 100.0 mL, initial temperature = 25°C, final temperature = 16°C, and Cp of water = 4.184 J/g°C? O 1226 O 808 O 389 O 418
A piece of metal weighing 146.7 g was heated from 32.0 °C to 56.2 °C. If the amount of heat needed was 1363.3 J, calculate the specific heat of the metal. What is the identity of the metal? 20 Specific Heats of Selected Metals Smetal, J/g-°C Metal 0.901 Smetal, J/g-°C 0.449 Metal Al Fe Cu 0.384 Ni 0.444 Si 0.711 Sn 0.226 Zn 0.389 Mn 1.02
The specific heat of a certain type of cooking oil is 1.75 J/ (g.°C). How much heat energy is needed to raise the temperature of 2.71 kg of this oil from 23 °C to 191 °C? 796.7 q = J Incorrect
A coffee-cup calorimeter contains 50 mL of water with an initial temperature of 24.8°C. An unknown sample with a mass of 1.972 grams was placed inside making the water temperature rise up to 25.5°C. The initial temperature of the metal was 98.3°C. (Water: density = 1g/mL ; specific heat = 4.184 J/g-°C). 2. What is the specific heat (in Jlg-°C) of the unknown sample? (round off final answer to 2 decimal places) 1.02
Can you explain this with an explaination please?
TUMU Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) AH = -184.6 kJ Reaction 2: 20F 2(g) → O₂(g) + 2 F₂ (g) Reaction 3: N₂(g) +202(g) →→→ 2NO₂(g) Use Reaction 1. Answer: AH = -49.4 kJ Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,152.0 kJ of energy is released from the system. Round to the nearest whole number. g AH = +66.4 kJ
When 3.0 grams of H2 is reacted with excess C at constant pressure, the reaction forms CH4 and releases 58.6 kJ of heat. C(s) + 2 H2(g) --> CH4(g) What is the enthalpy of the reaction in kJ/mol of CH4? Enter your answer numerically and in terms of kJ/mol.

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