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when copper(II) hydroxide is heated it dehydrates, losing one molecule of water and forming copper(II) oxide.
calculate the concentration in mol/L and mg/L of a solution prepared by adding 4.00 mL of a 8.26 x 10^-4M stock solution of Allura Red to a 100.00 mL volumetric flask and then filling to the mark with DI water.
Draw a structure for a compound that meets the following description: A compound C3H5N with an IR absorption at 2215 cm-1 but none at 3300 cm-1
A lungful of air (500 mL) contains 4.1% CO2 by volume. How many grams of KO2(s) is needed to remove the CO2 from a lungful of air at STP according to the following reaction?
Consider the following reaction: 2A + B → 3C + D If 63.0 mol A and 42.0 mol B react to form 54.0 mol C. What is the percent yield of this reaction.
Assuming that the pressure and amount of a gas sample remain constant, what will be the final volume of a 3 .84 L sample of a gas originally at 160 0C when heated to 280 0C
calculate the difference between the Gibbs free energy and Helmholtz free energy for this reaction at normal temperatures and pressures.
what is the term for a substance that is capable of either accept or donate a proton in as which base reaction?
Calculate the number of moles in each of the following: a) 85.2 g of Ni, b) 144 g of K, c) 6.4 g of H2O, d) 308 g of BaSO4, e) 252.8 g of fructose C6H12O6
how many kilojoules of energy are needed to convert 100 g ice at 10.0C to water at 20.0C? (the specific heat of ice at 10C is 2.01)
A mixture of CO(g) and O2 (g) in a 1 L container at 1000 K has a total pressure of 2.2 atm. After some time the total pressure falls to 1.9 atm as the result of the formation of the CO2(g). Find the mass in grams of the CO2 gas.
Cobalt was used as an internal standard to analyze a sample of titanium with atomic absorption spectroscopy. A mixture was prepared by combining a 5.50 mL Ti solution of unknown concentration with 2.00 mL of a 13.4 g/mL solution of Co
How would the addition of sodium chloride affect the hydrated cobalt(II) ion equilibrium? Explain using Le Chatelier's principle
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