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Aqueous potassium iodide reacts with aqueous copper(II) nitrate to form a mixture of solid copper(I) iodide, solid iodine, and aqueous potassium nitrate. What volume of a 0.2089 M solution of aqueous potassium iodide will contain enough potassium iodide to react exactly with the copper(II) nitrate in 43.88 mL of a 0.3842 M solution of aqueous copper(II) nitrate?
Determine the molarity of Ni in the 20.0 mL solution. Determine the mass in grams of Ni in the original sample. Determine the weight percent of Ni in the sample.
Given that the standard free energy of formation of MCl2(s) and MO2(s) are, respectively, -311.5 and -286.5 kJ/mol at 25o C. What is the standard change in free energy (kJ) for the following reaction
nitric acid is usually purchased in concentrated form with a 70.3% HNO3 concentration by mass and a density of 1.14% g/ml. How much of the concentrated stock solution in milliliters should you use to make 2.5L of 0.500 M HNO3.
Keq is 1.60 at 933 K for this reaction. H2(g) + CO2(g) H2O(g) + CO(g) Calculate the equilibrium concentration of hydrogen when [CO2] = 0.290 mol/L, [H2O] = 0.250 mol/L, and [CO] = 0.210 mol/L.
Calculate the molality of a solution that contains 51.2 g of naphthalene, C10H8, in 500. mL of carbon tetrachloride. The density of CCl4 is 1.60 g/mL.
assuming no heat loss, and that the specific heat (capacity) of water is 4.184 J/g*K, what is the heat capacity of the copper in J/K?
The mass percent of sulfur in the product is Blank 1 % (2 dec places). The mass percent of oxygen in the product is Blank 2 % (2 dec places).
What is the pH of an 85 mL solution containing .215 M NaHCO3 and .203 M Na2CO3?
A buffer is made using 45.0 mL of 0.750 M HC3H5O2 and 55.0 mL of 0.700 M NaC3H5O2.What volume of 0.10 M NaOH must be added to change the pH of the original buffer solution by 2.5%? Ka for this acid is 1.3 x 10
At constant pressure, 660 mL of nitrogen at 37°C are changed to 725 mL What is the new temperature of this gas?
What is the value of x in the formula for the hydrate? (hint: remember that x represents the ratio of moles of H2O to moles of hydrate compound, and that moles of hydrate compound equals the moles of anhydrous compound)
Final temperature after urea dissolves in water, What is the final temperature of the solution in kJ? The density of water is 4.18 J/g·°C. What is the final temperature in °F? F = °C x 1.8 + 32 (Round your answer to one decimal place)
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