Use standard enthalpies of formation from appendix
Formation of SO3 from the air pollutant SO2 is a key step in the formation of acid rain, according to the following reaction. Use standard enthalpies of formation from Appendix L to calculate the enthalpy change for the reaction.
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In the reaction A → products, [A] is found to be 0.490 M at t=72.0 s and 0.474 M at t=82.6 s. What is the average rate of the reaction during this time interval (in Ms^-1)?
Compare the pH values in the dilution experiment for the strong acid(HCL) and the weak acid(ACETIC ACID). Do the pH values increase at the same rate across the wells?
Calculate the formal concentration of a sodium acetate solution prepared by diluting 45.0 mL of a solution containing 25.0 ppm sodium acetate (NaC2H3O2) to a total of 0.500 liters of solution.
In a test on the vaporization of water into air in a wetted-wall column, the following data were obtained: Tube diameter= 1.46 cm. Calculate the rate of mass transfer of water in air.
The most common source of copper (rm Cu) is the mineral chalcopyrite (rm CuFeS_2). How many kilograms of chalcopyrite must be mined to obtain 200. g of pure rm Cu?
In a reaction 82.00 g of sodium reacts with 74.00g of ferric oxide to form sodium oxide and iron metal. calculate the mass of solid iron produced.
How many grams of sodium lactate must be added to a 1.00L solution of .400M lactic acid to make a buffer with a pH of 3.7 ?
What is the charge on magnesium iodide? What does the charge on the magnesium ion have to do with the number of valence electrons that an atom of magnesium has?
When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?
A student placed 12.0 g of glucose (rm C_6H_{12}O_6) in a volumetric flask, added enough water to dissolve the glucose by swirling, then carefully added additional water until the 100.-rm mL mark on the neck of the flask was reached.
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