Please see the activity sheet below for the context and question. Thank you ExperimentDerermin arion Of The Calorimeter consrontbiven: Masug100g oF KCrerser up 1(room temp.)L RTTemp: = 20°2009 Of wcHer1ver up 7Temp I: 60°C(hot tep.)Final temp: 46.67°Cspecific nect = 4. 184 J/g°C9norM2 Speipic HecH • (TF - TI)= (200g)(4. 184JIYT )( *v.69°C - 60°)= - 111 54. 544 J,* Mi• Spei pic HeCT • ( TF - T)-C10og) (4. 1840/0°C) (46.6607°C-20°C)%3D=11158. 728JCean : -(9er + 9 not)RThOTQue stion : whCr will be Theinitial temperaure ponthis Formulca? will I codthe Two initicH temp. ( C60°C & 20 °C):(Jince the 2 vegUp was nixed toyetner).(TP - ti)466.67°C

Given that, M1=100g of waterT1=200CM2=200g of waterT2=600CFinal temperature, Tf=46.670CSpecific…

* Experiment Derermin arion Of The Calorimeter constont Given: Masua = 100g oF KCrer ver up 1 (room temp. LV RT Temp2 * 20° 2009 Of wCHer 1 ver up ? Temp i : 66°C (hot tep.) Final temp= 46.67°C SpeUFし heCt - 4. 184 J/9°C 9 nor Mz°Speipic HeCH • (TF - TI (200g)C4. 184J/yʻt )( 46.69°C - 60°) = - 111 54. 544 J, ( TF - Ti) -(1oog) (4. 1840 la°C) ( 4.07°C - 10°C) : Mi•Spei pic HeaT • = 11 158. 7 28J -(1er + 9nor) Ccar ミ hot Que ution initial temperaure pon this formulce? will I cod the wo initici temp. (G0°C& 20 °C): (Sike the 2 seuP was : WHCT will be The (TP - Ti) 46.67°C ヘxed ogether).

* Experiment Derermin arion Of The Calorimeter constont Given: Masua = 100g oF KCrer ver up 1 (room temp. LV RT Temp2 * 20° 2009 Of wCHer 1 ver up ? Temp i : 66°C (hot tep.) Final temp= 46.67°C SpeUFし heCt - 4. 184 J/9°C 9 nor Mz°Speipic HeCH • (TF - TI (200g)C4. 184J/yʻt )( 46.69°C - 60°) = - 111 54. 544 J, ( TF - Ti) -(1oog) (4. 1840 la°C) ( 4.07°C - 10°C) : Mi•Spei pic HeaT • = 11 158. 7 28J -(1er + 9nor) Ccar ミ hot Que ution initial temperaure pon this formulce? will I cod the wo initici temp. (G0°C& 20 °C): (Sike the 2 seuP was : WHCT will be The (TP - Ti) 46.67°C ヘxed ogether).

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 72QAP: On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm...

See similar textbooks

Similar questions

In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/Cg, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
Isomers are molecules with the same elemental composition but a different atomic arrangement. Three isomers with the formula C4H8 are shown in the models below. The enthalpy of combustion (cH) of each isomer, determined using a calorimeter, is as follows: (a) Draw an energy level diagram relating the energy content of the three isomers to the energy content of the combustion products, CO2(g) and H2O(). (b) Use the cH data in part (a), along with the enthalpies of formation of CO2(g) and H2O() from Appendix L, to calculate the enthalpy of formation for each of the isomers. (c) Draw an energy level diagram that relates the enthalpies of formation of the three isomers to the energy of the elements in their standard states. (d) What is the enthalpy change for the conversion of cis-2-butene to trans-2-butene?
If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is CT- = 56.990.1202T J/mol.K, how much heat is needed?
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
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.
A cubic piece of uranium metal (specific heat capacity = 0.117 J/C g) at 200.0C is dropped into 1.00 L deuterium oxide ("heavy water;" specific heat capacity = 4.21 I J/C g) at 25.5C. The final temperature of the uranium and deuterium oxide mixture is 28.5C. Given the densities of uranium (19.05 g/cm3) and deuterium oxide (1.11 g/mL). what is the edge length of the cube of uranium?
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.
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?
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?
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?
Acetylene (C2H2) and butane (C4H10) are gaseous fuels with enthalpies of combustion of 49.9 kJ/g and 49.5 kJ/g. respectively. Compare the energy available from the combustion of a given volume of acetylene to the combustion energy from the same volume of butane at the same temperature and pressure.