Canvas Question 24 Gold has a melting point Of 1338 K with AH°fus = 12.7 kJ/mol and boils at 3080 K with AH°vap = 310 kJ/mol. Given the specific-heat capacities (in J/g K) of Au(s), Au(I), and Au(g) are 0.131, 0.149, and 0.0632, respectively, how much heat (J) is requires to convert 2.15 g Au(s) at 1000 K to liquid at 1500K? 160. J Å 12.8 J O 81.1 J O 285 J Question 25 Which is the oxidizing agent in the reaction below? Cr₂O72- + 6 S₂032 + 14 H+ 2 Cr³+ + 3 S4062 +7 H₂O 0₂²- MacBook Pro ( 9 P

Canvas Question 24 Gold has a melting point Of 1338 K with AH°fus = 12.7 kJ/mol and boils at 3080 K with AH°vap = 310 kJ/mol. Given the specific-heat capacities (in J/g K) of Au(s), Au(I), and Au(g) are 0.131, 0.149, and 0.0632, respectively, how much heat (J) is requires to convert 2.15 g Au(s) at 1000 K to liquid at 1500K? 160. J Å 12.8 J O 81.1 J O 285 J Question 25 Which is the oxidizing agent in the reaction below? Cr₂O72- + 6 S₂032 + 14 H+ 2 Cr³+ + 3 S4062 +7 H₂O 0₂²- MacBook Pro ( 9 P

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 31QAP: A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at...

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A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)
9.95 How much heat is required to convert 250 g of water from liquid at 23°C: into steam at 107°C? (The necessary heat capacities and enthalpy changes can be found in the chapter or online.)
It has been determined that the body can generate 5500 kJ of energy during one hour of strenuous exercise. Perspiration is the bodys mechanism for eliminating this heat. What mass of water would have to be evaporated through perspiration to rid the body of the heat generated during 2 hours of exercise? (The heat of vaporization of water is 40.6 kJ/mol.)
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.
After the sinking of RMS Titanic, US operated the International Ice patrolwith the purpose of monitoring the presence and movements of icebergsin the Atlantic and Arctic oceans. Once, they observed a unique tabulariceberg in a form of a rectangle (250 km x 50 km x 300 m). How manyyears would it take to melt the iceberg solely by heat from the sun if theice absorbs a mean of 98 J/m2-s, 12.5 hrs per day? Note: the exposed area for heating is 250 km x 50 km and the density is 920 kg/m3.
An ice cube with a mass of 20 g at -20 °C (typical freezertemperature) is dropped into a cup that holds 500 mL ofhot water, initially at 83 °C. What is the final temperaturein the cup? The density of liquid water is 1.00 g/mL; thespecific heat capacity of ice is 2.03 J/g-C; the specific heatcapacity of liquid water is 4.184 J/g-C; the enthalpy offusion of water is 6.01 kJ/mol.
5. The literature value for the heat of fusion of ice is 6.02 kJ/mole. What is the percent error for the experimentally determined heat of fusion?
How much heat must be removed from a 90.5 g sample of benzene (M = 78.11 g mol-1) to cool the sample from 305 K to 215 K? The following physical data may be useful.ΔfusH = 9.8 kJ mol-1ΔvapH = 30.8 kJ mol-1Cs(l) = 1.73 J g-1 K-1Cs(s) = 1.51 J g-1 K-1Cs(g) = 82.4 J g-1 K-1 Tm = 279.0 KTb = 353.3 K Note: The word 'removed' in the question already accounts for the negative sign involved in the heat transfer. Express your answer to three significant figures.
Theheat of fusion for titaniumis 390.6J/g. How much heat energy is required to melt 541.28g of titaniumat its melting point.(Show all work.)
Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 791.0 g sample of acetone sitting in the lab has a temperature of 21.7°C. How much heat would be involved in lowering the temperature of the acetone to -200.0°C? (answer in Joules)
Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 523.70 g sample of acetone gas has a temperature of 56.0°C. How much heat is involved in converting it to a solid that has a temperature of -94.0°C? (Answer in Joules)
The heat of vaporization for 1.0 mole of water at 100.°C and 1.0 atm is 40.55 kJ/mol. Calculate DS for the process H2O(l) -> H2O(g) at 100.°C.