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Calculate the partial pressure of oxygen in the air at 100 kPa if nitrogen has a partial pressure of 82 kPa and carbon dioxide and water combined have a partial pressure of 0.77 kPa.
You have 10.00L of a 0.350M KCl solution, but you need a solution that is 0.450M. What volume of water, in L, would you evaporate from the solution
A solution is prepared by dissolving 49.3 g of of KBr in enough water to form 473 mkof solution. calculate the mass % in the soulutionif the density is 1.12 g/mL
the solubility product for a sparingly soluble transition metalsalt m2x equals 3.80e-19. the formation constant for
During the course of an experiment, 10.0 mL of water is added to 25.0 mL of aqueous 0.120 M NaCl. What is the concentration of NaCl in the resulting solution
the permangenate ion and determine the standard reduction potential for the reaction.
Exists in an otherwise nonpolar molecule. Occurs because the electrons in a bond move about the orbital and at any moment may not be distributed exactly between the two bonding atoms, even when the atoms are identical.
The cylinder diameter is 2 inches and the depth of the water in the cylinder is 4 inches. Determine the concentration of salt in solution, showing your answer in the units specified.
The liquid vaporizes quickly to gaseous nitrogen (which has a density of 1.15 g/mL at room temperature and atmospheric pressure) when the liquid is removed from the tank.
Determine the mass of ice that has melted. Assume that the heat capacity of the cup can be ignored. It takes 334 J to melt 1.00 g of ice at 0 c.
How many moles of carbon dioxide are produced when 19.3 mole of propane gas is burned in excess oxygen? C3H8(g) +5O2(g)=3CO2(g) + 4H2O(l).
Making plastic drinking bottles for bottled water requires about 58 million barrels of oils per year (2007). In 2007, 300 million people averaged 114 L of bottled water per person. The average cost of 0.6 L was $1.00. The average charge for tap wa..
The substances, NaCl, Na2CO3, MgSO4, and NH4Cl used for test solutions, are all soluble ionic compounds. For each substance indicate the ions present in its respective test solution.
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