43) The temperature of a substance is a measure of its particles' A) Jentropy B) enthalpy C) average potential energy D) average kinetic energy 44) The molecules of which substance have the highestaverage kinetic energy? DC=°C A) He(g) at ODC C) N2(g) at 60DC D) CO2(g) at 20DC B) HCI(g) at 40DC 45) In which beaker would the particles have the highest average kinetic energy? A) C) 10 milliliters 0.1 M HCI at 20°C 50 milliliters 0.1 M HCI at 10°C D) B) 200 milliliters 0.1 M HCI at 30°C 400 milliliters 0.1 M HCI at 15°C A)

43) The temperature of a substance is a measure of its particles' A) Jentropy B) enthalpy C) average potential energy D) average kinetic energy 44) The molecules of which substance have the highestaverage kinetic energy? DC=°C A) He(g) at ODC C) N2(g) at 60DC D) CO2(g) at 20DC B) HCI(g) at 40DC 45) In which beaker would the particles have the highest average kinetic energy? A) C) 10 milliliters 0.1 M HCI at 20°C 50 milliliters 0.1 M HCI at 10°C D) B) 200 milliliters 0.1 M HCI at 30°C 400 milliliters 0.1 M HCI at 15°C A)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.101PAE

See similar textbooks

Similar questions

For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7kJ: a.What quantity of heat is required to produce 1 mole of mercury by this reaction? b.What quantity of heat is required to produce 1 mole of oxygen gas by this reaction? c.What quantity of heat would be released in the following reaction as written? 2Hg(l) + O2(g) 2HgO(s)
How much heat is produced by combustion of 125 g of methanol under standard state conditions?
When steam condenses to liquid water, 2.26 kJ of heat is released per gram. The heat from 168 g of steam is used to heat a room containing 6.44 104 g of air (20 ft 12 ft 8 ft). The specific heat of air at normal pressure is 1.015 J/(gC). What is the change in air temperature, assuming the heat from the steam is all absorbed by air?
9.21 Which type of energy heat or work, is valued more by society? What evidence supports your judgment?
Oxygen was first prepared by Joseph Priestley (1733-1804) by heating HgO. Use data in Appendix L to estimate the temperature required to decompose HgO(s) into Hg() and O2(g).
The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?
What is a driving force? Name two common and important driving forces, and give an example of each. What is entropy? Although the total energy of the universe is constant, is the entropy of the universe constant? What is a spontaneous process?
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)
How much will the temperature of a cup (180 g) of coffee at 95 C be reduced when a 45 g silver spoon (specific heat 0.24 J/g C) at 25 C is placed in the coffee and the two are allowed to reach the same temperature? Assume that the coffee has the same density and specific heat as water.
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.
What quantity of heat energy would have to be applied to a 25.1 -g block of iron in order to raise the temperature of the iron sample by 17.5 °C? (See Table 10.1.)