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A reaction mixture of 4.00 mL of 0.00200 M SCN and 5.00 mL of 0.00200 M Fe^3+ is diluted to 10.00 mL with 0.1 M HNO3 to form the blood-red FeNCS^2+ complex. The equilibrium molar concentration of the FeNCS^2+ determined from a calibration curve, is 1.5 x 10^-4 mol/L. Calculate, in sequence each of the following quantities in the aqueous solution to determine the equilibrium constant for the reaction. Fe^3+(aq) + SCN-(aq)<-------->FeNCS2+(aq) a. moles of FeNCS^2+ that form in reacting equilibrium b. moles of Fe3+ that react to form the FeNCS^2+ at equilibrium c. moles of SCN- that react to form the FeNCS^2+ at equilibrium d. moles of Fe^3+ initially placed in the reaction system e. moles of SCN- initially placed in the reaction system f. moles of Fe^3+ (unreacted) at equilibrium EQUATION: mol Fe^3+ equilibrium = mol Fe^3+ initial - mol Fe^3+ reacted g. moles of SCN- (unreacted) at equilibrium EQUATION: mol SCN- equilibrium = mol SCN- initial - mol SCN- reacted h. molar concentration of Fe^3+ (unreacted) at equilibrium i. molar concentration of SCN- (unreacted) at equilibrium j. molar concentration of FeNCS^2+ at equilibrium k. Kc= ([FeNCS^2+]) / ([Fe^3+][SCN-])
TCE is added to the aqueous phase so that initally it has an aqueous phase concentration of 100 ppb. After the system equilibrates, what will be the concentration of TCE in the aqueous phase
If 40.0 g of Cu is placed into 100.0 g of H20 at a temperature of 20.0*C and if the temperature of the water rises to 23.0*C, what was the temperature of the Cu
Draw the structure of camphor and show which C-C bond must be broken to form the unwanted by-product
When aluminum is produced by electrolysis we get 5.68 tons of aluminum and 5.04 tons of oxygen. What is the empirical formula of the compound that is being electrolyzed
When an ionic solid is added into a solvent, you can see that the ionic solid dissociates into its respective cations and anions. The solvent molecules immediately cluster around the ions.
Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5. 10-3, Ka2 = 8. 10-8, and Ka3 = 6. 10-10. Calculate [H + ], [OH ? ], [H3AsO4], [H2AsO4? ], [HAsO42- ], and [AsO43- ] in a 0.62 M arsenic acid solution.
Polyglutamic acid, a polypeptide containing only glutamic acid residues, spontaneously coils into an a-helix at pH 1 but not at pH 7.
Problem- In the experiment of establishing the relative reactivity of Halogens and Halide Ions a student performed the following two tests on an unknown solution containing one halide ion.
calculate the change in entropy that occurs when 18.53 g of ice at -10.7°C is placed in 54.05 g of water at 100.0°C in a perfectly insulated vessel.
When a 0.369 g sample was studied by combustion analysis, 0.662 g of CO2 and 0.0897 g of H2O formed. How many moles of each of the following were in the original sample? C: ? H: ? Cl: ? What is the molecular formula?
The radioactive Co-60 isotope is used in nuclear medicine to treat certain types of cancer. Calculate the wavelength and frequency of an emitted gamma particle having the energy of 1.29 x 10^11 J.
A gas mixture with a total pressure of 765 contains each of the following gases at the indicated partial pressures: , 118 ; , 229 ; and , 187 . The mixture also contains helium gas. What is the partial pressure of helium gas.
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