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Octane (C8H18(l)) is a key component of gasoline. How much energy (enthalpy) in kJ is released from the combustion of one mole of octane? How much energy is released from the combustion of one gram of octane?
A basketball is inflated to a pressure of 1.50 atm in a 20.0C garage. What is the pressure of the basketball outside where the temperature is -5.00C.
Determine the percent yield for this reaction as N2(g) + 3 H2(g) ? 2 NH3(g)
Calculate the [Zn2+] in a solution of ZnC2O4 held at a pH of 3.00. Remember C2O4^2- is a weak base so you must consider other equilibria. (Ksp(ZnC2O4)=7.5X10^-9, Kb1=1.8X10^-10, Kb2=1.8X10^-13).
Determine the molarity of the NaOH(sodium hydroxide) solution. In an acid-base titration, 22.13 mL of a sodium hydroxide solution are required to neutralize 24.65 mL of the potassium hydrogen phthalate solution?
Calculate the entropy change that occurs when 3.5 moles of an ideal gas expands from 1.75 L at 20 degress Celsius to 8.46 L at .54 atm.
A 20.00 mL sample of 0.1026 M HCl was titrated with NaOH solution. The initial buret reading was 0.25 mL, and the final reading was 18.78 mL.
A 12-liter tank contains helium gas pressurized to 160atm . What size tank would be needed to contain this same amount of helium at atmospheric pressure (1atm )?
In this experiment a hot metal block at 100oC is added to cold water in a calorimeter. The heat lost by the metal block equals the heat gained by the water and the two end up at the same temperature.
Calculate the cumulative acid equivalents per square meter that were deposited in the watershed over the entire period 1880-1950.
Assume that the H2O2 solution has a density of 1.0g/cm3. What would the mass of 35cm3 of the H2O2 solution be?
A 65 L sample of dry air cools from 133°C to -16°C while the pressure is maintained at 2.85 atm. What is the final volume?
Dehydrohalogenation Prepare styrene (C6H5CH=CH2) by dehydrohalogenation of either 1-bromo-2-phenylethane or 1-bromo-1phenylethane using KOH in ethanol.
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