You are the human resources manager for a famous retailer and are trying to convince the president of the company to change the structure of employee compensation. Currently, the company’s retail sales staff is paid a flat hourly wage of $20 per hour for each eight-hour shift worked. You propose a new pay structure whereby each salesperson in a store would be compensated $10 per hour, plus 1 percent of that store’s daily profits. Assume that, when run efficiently, each store’s maximum daily profits are $25,000. Outline the arguments that support your proposed plan.

Water gas, a mixture of carbon monoxide and hydrogen, is produced by treating carbon (in the form of coke or coal) with steam at high temperatures. (See Study Question 83.) C(s) + H2O(g) CO(g) + H2(g) Not all of the carbon available is converted to water gas since some is burned to provide the heat for the endothermic reaction of carbon and water. What mass of carbon must be burned (to CO2 gas) to provide the energy to convert 1.00 kg of carbon to water gas?

Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.

Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.

Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2(aq) and NaBr(aq) are mixed. Pb(NO3)2(aq) + 2 NaBr(aq) PbBr2(s) + 2 NaNO3(aq) rH = ? To measure the enthalpy change, 200. mL. of 0.75 M Pb(NO3)2(aq) and 200. mL of 1.5 M NaBr(aq) are mixed in a coffee-cup calorimeter. The temperature of the mixture rises by 2.44 C. Calculate the enthalpy change for the precipitation of PbBr2(s), in kJ/mol. (Assume the density of the solution is 1.0 g/mL., and its specific heat capacity is 4.2 J/g K.)

The equation for the fermentation of glucose to alcohol and carbon dioxide is: C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is 67 kJ. Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?

list at least three quantities that must be conserved in chemical reactions.

Imagine that you were the chief engineer for NASA's Apollo 13 mission to the moon. The air filter which they had been using is fully saturated and no longer works. The astronauts are running out of oxygen and need to get rid of the excess carbon dioxide. You remember that the astronauts have a container of 14.5 kg of sodium hydroxide on the ship. As a chemical engineer, you know that sodium hydroxide can be used to remove carbon dioxide from the air by producing sodium carbonate and dihydrogen monoxide. How many liters of carbon dioxide are cleaned by the amount of sodium hydroxide given in the problem? The astronauts have 3 days left before they land on earth. You know that there are 4 astronauts, and each astronaut emits roughly 700 grams of carbon dioxide (CO2) each day. • How many liters of CO2 are produced by the astronauts? • Is there enough NaOH for the astronauts to survive the rest of their trip? If the astronaut survived the trip, how much NaOH was left over? If the astronaut…

A student is preparing a solution of sucrose (C12H22O11) at a specific concentration. They are doing this by weighing out sucrose on a scale, placing it in a volumetric flask, dissolving it in water, and then diluting it up to the mark on the volumetric flask with water. How would the experimental (actual) molar concentration for C12H22O11 differ from the calculated concentration (higher, lower, or the same) given the following scenarios? Explain. (Hint: Compare the calculated concentrations to experimental concentrations). c) When preparing the diluted solution, a student used the pipet bulb to blow out the last few drops in the pipet into the solution.