Calculating Kinetic Energy worksheet (back) 9. At standard temperature (0°C), a carbon dioxide molecule travels at a speed of159.5 m/s. Find the kinetic energy of a carbon dioxide molecule. Substitute intothe formula and verify the final units are in J. (Gas speed is to 4 SF, butcompute KE to 3 SF).10. Summarize the results from problems 6. through 9. in the table below.MolarMass(g/mol)Temperature(°C)Prob.#6.7.8.9.GasFormulaSpeed(m/s)4 SFΚΕ(J)3 SF11. What appears to be the relationship between the temperature and the kineticenergy of gas particles?12. At a constant temperature, as the mass of gas particles increases, the speed(increases/decreases/stays the same)? [Circle the correct choice.]13. Calculate the KE for propane gas at 20 °C moving at 175 m/s. (3 SF) Would theKE for butane gas be, (smaller/larger/same)? [Circle correct choice.] Would itbe moving (faster/slower/same) as propane? [Circle correct choice.]14. Both carbon dioxide and propane have the same molar mass of 44 g/mol. Whydoes the carbon dioxide KE from problem 9. differ from the propane KE ofquestion 13.?15. Using the KE from the problem 13. calculate the actual speed of the butanemolecule at 20 °C. (All to 3 SF) Was your prediction about the speed ofpropane vs. butane from question # 13. correct?

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9. At standard temperature (0°C), a carbon dioxide molecule travels at a speed of 159.5 m/s. Find the kinetic energy of a carbon dioxide molecule. Substitute into the formula and verify the final units are in J. (Gas speed is to 4 SF, but compute KE to 3 SF).

9. At standard temperature (0°C), a carbon dioxide molecule travels at a speed of 159.5 m/s. Find the kinetic energy of a carbon dioxide molecule. Substitute into the formula and verify the final units are in J. (Gas speed is to 4 SF, but compute KE to 3 SF).

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Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)
You heat 1.000 quart of water from 25.0C to its normal boiling point by burning a quantity of methane gas, CH4. What volume of methane at 23.0C and 745 mmHg would you require to heat this quantity of water, assuming that the methane is completely burned? The products are liquid water and gaseous carbon dioxide.
When two cotton plugs. one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white 1111g of NH4Cl forms where gaseous NH3 and gaseous HC1 first come into contact. NH3(g)+HCl(g)NH4Cl(s) At approximately what distance from the ammonia moistened plug does this occur? (Hint: Calculate the rates of diffusion for both NH3 and HCI, and find out how much faster NH3 diffuses than HCI.)
Evaluate (U/V)T for an ideal gas. Use the expression from Example 4.11. Does your answer make sense?
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?
What will be the final temperature of a mixture made from equal masses of the following: water at 25.0C, ethanol at 35.5C, and iron at 95C?
Explain why Gf of O2 (g) is zero.
Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40. cm3. If the combustion of this mixture releases 950. J of energy, to what volume will the gases expand against a constant pressure of 650. torr if all the energy of combustion is converted into work to push back the piston?
Difference between the system and the surroundings. Give examples of both.
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.
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.
Consider the reaction between methane and oxygen producing carbon dioxide and water. Suppose that the reaction is carried out in a furnace used to heat a house. If q=890kJ and w=+5kJ, what is E? H at 25C?

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