hx/7231799#/7231799/2/0mpleted 13 out of 16.3 of 16JPer: X M Inb xPRFheat added:2 O Etheat added:heat added:ا الگCalculate 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 nochanges in state occur during this change in temperature.26per xTCalculate 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 nochanges in state occur during this change in temperature.GJAeffe X CDC He: XCalculate the amount of heat, in calories, that must be added to warm 96.8 g of wood from 21.3 °C to 42.4 °C. Assume nochanges in state occur during this change in temperature.62YHUJ10 X81GA B9KNo XNowOeth X0Sm x Sm x +0/D00 39HR MIN SECРResourcesLLIFinDENextcalcalcalPEAL40 Per x M Inb x31799#/7231799/2/0ted 13 out of 1616P11Essentials of General, Organic, and BiochemistryDenise GuinnTHIRD EDITIONThe table lists the specific heat values for brick, ethanol, and wood.Specific Heats of SubstancesSubstanceBrickEthanolWoodheat added:PSper: X20effe x CDC He: XJA6Specific Heat0.200.580.10B10 X4gºCCalculate 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 nochanges in state occur during this change in temperature.W4Calculate 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 nochanges in state occur during this change in temperature.○바8No X9ECeth X0Sm X00 39HR MIN SEC0/RSm xResources+presented by Macmillan LearningGا ا ا200LNext Qucal401

Answered: Image /qna-images/answer/ed835e22-6b5a-4730-b545-df3fca343a0c.jpg

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. heat added: 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. heat added: Calculate the amount of heat, in calories, that must be added to warm 96.8 g of wood from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. cal cal

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. heat added: 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. heat added: Calculate the amount of heat, in calories, that must be added to warm 96.8 g of wood from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. cal cal

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.94PAE

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Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 C in a calorimeter, the temperature increases to 25.2 C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat in joules produced.
9.63 Reactions of hydrocarhons are often studied in the petroleum industry. One example is 2C3H8(g)C6H6(l)+5H2(g) , with H = 698 kJ. If 35 L of propane at 25C and 0.97 atm is to be reacted, how much heat must he supplied?
9.102 A runner generates 418 kJ of energy per kilometer from the cellular oxidation of food. The runner's body must dissipate this heat or the body will overheat. Suppose that sweat evaporation is the only important cooling mechanism. If you estimate the enthalpy of evaporation of water as 44 kJ/mol and assume that sweat can he treated as water, describe how you would estimate the volume of sweat that would have to be evaporated if the runner runs a 10-km race.
In earlier times, ethyl ether was commonly used as an anesthetic. It is, however, highly flammable. When five milliliters of ethyl ether, C4H10O(l)(d=0.714g/mL), are burned in a bomb calorimeter, the temperature rises from 23.5C to 39.7C. The calorimeter contains 1.200 kg of water and has a heat capacity of 5.32 kJ/C. (a) What is qH2o? (b) What is qcal? (c) What is q for the combustion of 5.00 mL of ethyl ether? (d) What is q for the combustion of one mole of ethyl ether?
9.100 Two baking sheets are made of different metals. You purchase both and bake a dozen cookies on each sheet at the same time in your oven. You observe that after 9 minutes, the cookies on one sheet are slightly burned on the bottom, whereas those on the other sheet are fine. (You are curious and you vary the conditions so you know the result is not caused by the oven.) (a) How can you use this observation to infer something about the specific heat of the materials in the baking sheets? (b) What is themathematical reasoning (equation) that you need to support your conclusion?
9.57 The heat of combustion of butane is —2877 kJ/mol. Use this value to find the heat of formation of butane. (You may also need to use additional thermochemical data found in Appendix E.)
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9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?
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9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.