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What is the molarity of aqueous silver nitrate if 50.00 mL of AgNO3 reacts with 25.0 mL of 0.100 M K2CrO4?
How much heat is required to convert 27.0 grams of ethanol at 28 degrees celcius to the vapor phase at 78 degrees celcius?
Estimate the value of the equilibrium constant at 610K for each of the following reactions. Delta Hf and S for BrCl is 14.6 kj/mol and 240.0 J/mol*K , respectively. Br2(g)+ Cl2(g) --> 2BrCl(g)
The excess I3- was titrated with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass percent of arsenic trichloride in the original sample?
Find the empirical formulas for compounds with the following compositions: a. 8.74% magnesium, 91.26% iodine b. 36.86% nitrogen, 63.14% oxygen
When 0.450kJ of heat is added to the gas, it expands and does 219J of work on the surroundings. What is the value of \Delta H for this process? Answer in units of kJ
Density and Identity, The mass of 5.00 mL carbon tetrachloride is 7.97g. What is the density of the carbon tetrachloride?
how many grams of lead (II) chloride is produced when 13.87 g lead (II) nitrate combines with hydrochloric acid to produce lead (II) chloride and nitric acid?
Compute the thermal-equilibrium values of hole and electron concentrations while Considering a homogeneous gallium arsenide semiconductor at the given temperature of T = 300 K with Nd = 1016 cm-3 and Na = 0?
A certain reaction releases 10.1 kJ at constant volume and at constant pressure releases 8.4 kJ. What is the (delta)U for the reaction?
A sample of nitrogen has a volume of 630 mL at a temperature of 49 degC. Assuming that the pressure is constant, what will be the volume when the temperature is 348.6 degC.
72.0 mL of a 1.40 M solution is diluted to a volume of 278 mL. A 139-mL portion of that solution is diluted using 161 mL of water. What is the final concentration.
How many grams of solute are present in each of the following aqueous solutions?
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