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Why does cyclopentadiene dimerize so easily and rapidly to dicyclopentadiene? Please explain your answer.
Relate entropy and reaction spontaneity, Gibbs free energy and reaction spontaneity, and Gibbs free energy and the equilibrium constant of a reaction.
Calculate the heat of dissolution (q) of urea using the following formula: q = -s m? Where is the heat capacity assume the heat capacity.
What volume of dry carbon dioxide, measured at 25 C and 785 mm Hg, will result from the complete combustion of 2.50 g of pentane?
Use the values of ?Hof given below to calculate (in kJ) ?Horxn for the following reaction
Suppose that the enthalpy of some substance over a large temperature range can be expressed as a function of the temperature.
A real gas is found to have a molar volume that is 90% of the molar volume of an ideal gas at 298K and 3 atm pressure.
A sample of N2 gas occupies 2.40 L at 20oC. If the gas is in a container that can contract or expand at constant pressure, at what temperature.
Discuss the idea that the standard of living in society might be measured in units of kJ/person available in that society.
The density of octane is 0.7025 g/cm and the density of ethanol is 0.7893 g/cm . If burning octane in an automobile is 20% efficient (i.e., 20% of the energy.
What is the value of ? G when [H+]= 1.5 x 10^-8 M, [CH3NH3+]= [H+]= 1.5 x 10^-8 M, [CH3NH3+]= 5.5 x 10^-4 M, and [CH3NH2]= 0.120 M?
A quantity of 7.480g of an organic compound is dissolved in water to make 300.0 mL of solution.
Compare the amount of cooling experienced by an individual who drinks 400mL of water (0 degrees C) with the amount of cooling experienced.
Calculate the standard reaction enthalpy, entropy and free energy at 298K for the following reactions:
Two fuels available for automobile uses are ethanol (C2H5OH) and gasoline (assume it to be octane, C8H18).
An ideal gas described by T(initial)=300K,P(initial)=1 bar and V(i)=10 L is heated at constant volume until P=10 bar.
For all three of the equilibria in problem #1 predict (1) how Ke is affected by an decrease in temperature, (2) predict how the equilibrium will shift.
Given the thermodynamic data in the table below, calculate the equilibrium constant for the reaction:
Calculate the molar enthalpy (in kJ/mol NaOH) for the solution process NaOH(s)>>Na+(aq)+OH-(aq) .
Using the equilbrium expression (from above) calculate What the OH- (aq) ion concentration in an ammonia solution with an equilibrium concentration.
Water is often used as a heat sink because of its high specific heat. Explain what this means and give examples where this is used.
Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20oC to convert it to liquid water at 60.0oC.
If 0.15 mol each of CO2, H2, CO, and H2O (all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K.
Define chemical potential, equilibrium Constants Kp and Kc. Also derive Kc and Kp mathematically and show the relationship between them.
What is the standard free energy change for the following reaction at 25°C