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A 1.45 g sample of an iron ore is dissolved in an acid and the iron is obtained as Fe+2 (ag). To titrate the solution, 21.6 mL of 0.102 M KMnO4 (aq) is required. The Fe+2 solution reacts with MnO4- as follows: 5Fe+2 (aq) + MnO-4 (aq) + 8H+ (aq) --------> 5Fe+3 (aq) + Mn+2 (aq) 4H2O (l) What is the percent of iron in the ore?.
a second reaction has a standard Gibbs free energy of -55 kJ/mol. What is the ratio of their equilibrium constants at 300 K?
Important information about Organic Chemistry, The most reasonable formula for a compound demonstrating M+ =101 with a minor M+1 peak is
If 138 mL of wet H2 is collected over water at 24°C and a barometric pressure of 748 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr at 24°C.)
The concentration of N2O4 at equilibrium was 0.0750 M. Calculate Kc for the reaction, according to the above equation.
Suppose that you have 175 mL of a buffer that is 0.300 M in both benzoic acid (C6H5COOH) and its conjugate base (C6H5COO%u2013). Calculate the maximum volume of 0.250 M HCl
A mixture of CO(g) and O2 (g) in a 1.0-L container at 1.0x10^3 Kelvin has a total pressure of 2.2 atm. After some time the total pressure falls to 1.9 atm as the result of formation of CO2. Find the mass (in grams) of CO2 that forms.
The acid ionization constant of Fe(H2O)62+(aq) is 3E-6. Compute the pH of a 0.2 M aqueous solution of Fe(NO3)2. 5. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.31. The solubility product of magnesium hydroxide is 1.2E-11
The normal boiling point of the liquid is 425 K. Liquid, X, and Y are all in equilibrium at 342 K and 1800 bar. Tc = 571K, Pc= 46 bar
A 100 g sample of an unknown liquid absorbs 2000 J of heat energy, raising the liquid's temperature from 50 ?C to 70 ?C .What is the speci?c heat capacity of this liquid.
if you use a one liter bottle of oil in your engine determine how much heat is produced in kcal the density of motor
determine how many moles of cation are produced when 6.46 grams of nh4cl is dissolved?nbspcompute the difference in the
its ground state absorbs 2.50 times as much energy as the minimum required for it to escape from the atom. Calculate the deBroglie wavelength of the emitted electron
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