[Review Topics][References]Use the References to access important values if needed for this question.The following information is given for antimony at 1atm:Tb = 1440.00°CTm = 631.00°CSpecific heat solid = 0.2090 J/g °CSpecific heat liquid = 0.2590 J/g °CSubmit AnswerAHvap (1440.00°C) = 1.605 x 10³ J/gAH fus (631.00°C) = 161.1 J/gA 39:60 g sample of liquid antimony at 726.00°C is poured into a mold and allowed to cool to 22.00°C. How many kJ of energyare released in this process?(Report the answer as a positive number.)Energy =KJRetry Entire Group 8 more group attempts remaining99+PreviousNextSave and

Given , □Hfus = 161.1 J/g Mass (m) = 39.60 g Heat = m.c.□T 726° c ---> 631 °c <---> 631 °c…

owing information is given for antimony at 1atm: 140.00°C 31.00°C heat solid = 0.2090 J/g °C heat liquid = 0.2590 J/g °C = g sample of liquid antimony at 726.00°C is poured into a mold and allowed to cool to 22.00°C. How many kJ of energy ased in this process? the answer as a positive number.) kJ nswer AHvap (1440.00°C) = 1.605 x 10³ J/g AHfus (631.00°C) = 161.1 J/g Retry Entire Group 8 more group attempts remaining # 99+ for this questi W Previous Next Save and

owing information is given for antimony at 1atm: 140.00°C 31.00°C heat solid = 0.2090 J/g °C heat liquid = 0.2590 J/g °C = g sample of liquid antimony at 726.00°C is poured into a mold and allowed to cool to 22.00°C. How many kJ of energy ased in this process? the answer as a positive number.) kJ nswer AHvap (1440.00°C) = 1.605 x 10³ J/g AHfus (631.00°C) = 161.1 J/g Retry Entire Group 8 more group attempts remaining # 99+ for this questi W Previous Next Save and

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 143IP: A cubic piece of uranium metal (specific heat capacity = 0.117 J/C g) at 200.0C is dropped into...

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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?
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.
Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?
Sublimation of 1.0 g of dry ice. CO2(s), forms 0.36 L of CO2(g) (at 78 C and 1.01 105 Pa). The expanding gas can do work on the surroundings (Figure 5.8). Calculate the amount of work done on the surroundings.
A 244-g amount of coffee in an open plastic cup cools from 80.0C to 20.0C. Assuming no loss of mass and a heat capacity of liquid water, determine w, q, U, and H for the process. The densities of water are dH2O, 80.0C = 0.9718g/cm3 and dH2O, 20.0C =0.9982 g/cm3.
hat difference is necessary for heat to flow between two systems? Can you think of an exception to your answer?
Heat lost by nickel = Heat gained by waterQNi = Qw m×CNi×(TNi – Tf) = mw×Cw×(Tf – Tw)275 g×0.444 Jg K×373-Tf=100 g×4.184 Jg K×Tf-295122.1×373-Tf=418.4×Tf-295373-Tf=3.4267×Tf-2953.4267 Tf-1010.8763 = 373-Tfsolve for Tf mathematicallyTf=312.62 K This part is very confusing.
he density of liquid oxygen at its boiling point is 1.14 kg/L , and its heat of vaporization is 213 kJ/kg .How much energy in joules would be absorbed by 3.0 L of liquid oxygen as it vaporized?Express your answer to two significant figures and include the appropriate units.
To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of the material was supplied with 35.548 J of heat causing the temperature of the material to rise from 297.05 K to 461.4 K. What is the specific heat of this material? Report your answer in units of J/(ºC · g) to 4 sig figs, but do NOT include units in your answer.
Chemistry 1. A pool of lava exhibits Group of answer choices nuclear energy thermal energy potential energy due to position potential energy due to composition 2. Determine the heat required to raise the temperature of a gold nugget (mass = 376 g) that starts at 25.0 oC and is heated to 125 oC. The specific heat capacity of gold is 0.128 J/g°C. Use correct units and amount of sig.figs. 4.81kJ/mol 4812.8J 4812.8kJ 4.8128J 4.81kJ A 4.682 g sample of phenol (C6H5OH, molar mass = 94.11 g/mol) was combusted in a bomb calorimeter with a heat capacity of 4.845 kJ/°C. If the temperature rose from 26.81°C to 56.95°C, determine the value of ΔH°comb for phenol. Use correct units and amount of sig.figs. 7265J/mol 2935.kJ -688.8kJ/mol 2935.225kJ -3051kJ/mol -2935kJ/mol Use the ΔH°f information provided to calculate ΔH° in kJ/molC2H6 for the reaction IS IT ENDOTHERMIC OR EXOTHERMIC? 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2Og) ΔH°f (kJ/mol) 49.10 0 -393.5 -241.8…
A 59.7 g piece of metal originally at 100C was placed in 60.0 g of water initially at 22.0 C. The final temperatture of both after some time is 28.5 C. Determine the specific heat of the metal.
When, a volume of 200 cm3of Lithium hydroxide solution of concentration 1.00 mol/dm3and 200 cm3of Hydrochloric acid of concentration 100 mol/dm3 were mixed together in acalorimeter the reaction was investigated to be exothermic. Based on the information given above in question one (1), calculated the enthalpychange per mol of water produced, if the heat capacity of the calorimeter was 76 J/Kand the temperature rise was 5.25 K. (State any assumptions made)