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The volume of a 15.6% (by mass) solution is 79.2 mL. The density of the solution is 1.480 g/mL. What is the mass of the solution?
What volume of oxygen is required to burn completely 401 cm3 (centimeters cubed) of butane, C4H10 (All substances are gases measured at the same temperature and pressure.)
would the equilibrium constant for the formation of Cu(OH)2 (s) be greater or lesser than the equilibrium constant for the formation of Cu(NH3)4^2+ (aq)? Please explain your reasoning.
Calculate the decomposition for this process at constant pressure and 25o C: CaCO3(s) = CaO(s) + CO2 look up the standard enthalpy formation of the reactant and product
After filtering, washing, drying, and weighing, the AgBr is found to weigh 0.609 g. What is the mass percent bromide in the metal salt?
What is the mole fraction of benzene in the vapor above the solution described in part (a)
What are the consequences of removing some of the phase transfer catalyst along with the hot reaction mixture after refluxing
Calculate the pH of 1.00 L of the buffer 1.00 M CH3COONa/1.00 M CH3COOH before and after the addition of (a) 0.080 mol NaOH, (b) 0.12 mol HCl. (Assume that there is no change in volume.)
The molal freezing point constant for water is 1.86 C/m. At what temperature will a mixture of 2.00 g of CaCl2(MM: 110.98g/mol) and 25.00 g of water freeze
For each pair of substances below, which one will have the higher molar entropy. Justify each choice with a brief explanation. Which substance has greater molar entropy. Why is its entropy greater
its freezing point depression constant is 8.37*C per molal. Use your corrected average temperature (5.0*C) to find the molality of the water in the alcohol. Find the percent water in the alcohol.
Calculate the mole fraction of each component in resulting mixture after oxidation assuming that H2O is present as a gas.
a solution of ammonia and water contains 1.10times1025 water molecules and 5.00times1024 ammonia molecules. how many
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