Question 9 of 16.#3EDсCcmillan LearningEssentials of General, Organic, and BiochemistryDenise GuinnTHIRD EDITIONThe table lists the specific heat values for brick, ethanol, and wood.Specific Heats of SubstancesSubstanceBrickEthanolWood4Calculate the amount of heat, in calories, that must be added to warm 77.9 g of brick from 20.8 °C to 55.1 °C. Assume nochanges in state occur during this change in temperature.heat added:$Calculate the amount of heat, in calories, that must be added to warm 77.9 g of ethanol from 20.8 °C to 55.1 °C. Assume nochanges in state occur during this change in temperature.RFV%513TG Search or type URLGSpecific Heat0.200.580.10^6BMacBook ProYHtv&7NUJ9* 008M+-(9K<O<H1)OO➡Ppresented by Macmillan LearningV●:U{+ "121=?11Ical}1 Question 9 of 16#3EDсCCalculate the amount of heat, in calories, that must be added to warm 77.9 g of ethanol from 20.8 °C to 55.1 °C. Assume noo changes in state occur during this change in temperature.Macmillan Learningheat added:Calculate the amount of heat, in calories, that must be added to warm 77.9 g of wood from 20.8 °C to 55.1 °C. Assume nochanges in state occur during this change in temperature.heat added:4Which substance requires the greatest input of heat energy?ethanolbrickO woodRFV%513G Search or type URLTG^6BMacBook ProYHtv&7NUJ* 008M+I(9KO<H**)- OLAPV.II{لال[1 +=?O111-calcal}1

Heat is calculated by using the formula q=ms∆T q=heat m=mass of substance s=specific heat of that…

C Macmillan Learn The table lists the specific heat values for brick, ethanol, and wood. Specific Heats of Substances Substance Brick Ethanol Wood heat added: Calculate the amount of heat, in calories, that must be added to warm 77.9 g of brick from 20.8 °C to 55.1 °C. Assume no changes in state occur during this change in temperature. Specific Heat 0.20 0.58 0.10 D Calculate the amount of heat, in calories, that must be added to warm 77.9 g of ethanol from 20.8 °C to 55.1 °C. Assume no changes in state occur during this change in temperature. NOV 13 cal gºC MacBook Pro G Search or type URL #tv ♫ S Tall A cal

C Macmillan Learn The table lists the specific heat values for brick, ethanol, and wood. Specific Heats of Substances Substance Brick Ethanol Wood heat added: Calculate the amount of heat, in calories, that must be added to warm 77.9 g of brick from 20.8 °C to 55.1 °C. Assume no changes in state occur during this change in temperature. Specific Heat 0.20 0.58 0.10 D Calculate the amount of heat, in calories, that must be added to warm 77.9 g of ethanol from 20.8 °C to 55.1 °C. Assume no changes in state occur during this change in temperature. NOV 13 cal gºC MacBook Pro G Search or type URL #tv ♫ S Tall A cal

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

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When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
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.
9.68 What are some features of petroleum that make it such an attractive fuel?
Dissolving 6.00 g CaCl2 in 300 mL of water causes the temperature of the solution to increase by 3.43 C. Assume that the specific heat of the solution is 4.18 J/g K and its mass is 306 g. (a) Calculate the enthalpy change when the CaCl2 dissolves. Is the process exothermic or endothermic? (b) Determine H on a molar basis for CaCl2(s)H2OCa2+(aq)+2Cl(aq)
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.
A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 19.6C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, the specific heat of all solutions is the same as that of water, and volumes are additive.
Use the same fat described in Question 27. (a) Write a thermochemical equation for the metabolism of fat. (b) A dieter reduces his food intake by 425 nutritional calories a day (1 nutritional calorie=1000calories). How many kJ can he lose in one day? (c) How many pounds of fat are lost in one week with this diet?
9.29 In which case is heat added to the system: (a) E=43J , w=40J ; or (b) E=31J , w=34J ?
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?
On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm (STP) evolves 75.65 kJ of heat. If the gas is a mixture of ethane (C2H6) and propane (C3H8), what is the mole fraction of ethane in the mixture?
9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?