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When iron metal is added to a solution of a silver salt, the iron goes into solution and the silver precipitates out according to the following:
Fe(s) + AgNO3(aq) yields Ag(s) + Fe(NO3)2(aq)
What mass of Fe(s) is required to remove all the silver from 2.00L of .650M AgNO3? This is a redox reaction. write the oxidation half-reaction. what is the oxidation agent?
4.00 mol CO2 is placed in a 6.00 L container at a temperature where 12.3% of it decomposes. What is the value of Kc for the following at this temperature
If aluminum is diffused into a thick slice of silicon with no previous aluminum in it at a temperature of 1100?C for 8 hours, what is the depth below the surface at which the concentration is 1016 atoms/cm3 if the surface concentration is maintain..
Yet the stock bottle clearly reads 0.0020 M. Why? Similarly, why is the initial concentration of iron (III) ion 0.10 M when the stock bottle contained 0.20 M iron (III) nitrate?
Calculate the concentrations of all species in a 0.100 M H3PO4 solution given the following Ka: 7.5 X 10^-3 for H3PO4^- 6.2 X 10^-8 for H2PO4^- and 4.8 X 10^-13 HPO4^2
A certain second-order reaction (B-> Products) has a rate constant of 1.80×10^-3 M^-1xs^-1 at 27C and an initial half-life of 216 s . What is the concentration of the reactant B after one half-life?Express the molar concentration numerically.
A student is asked to determine the formula of a hydrate of colbalt (II) chloride. The mass of the empty clean, dry crucible and cover, after heating is 22.446 g. A sample of 0.324 g of cobalt chloride is added to the crucible.
A Breathalyzer instrument contains two ampules, each of which contains 0.75 mg K2Cr2O7 dissolved in 3 mL of 9 mol L?1 H2SO4(aq). One of the ampules is used as reference. When a person exhales into the tube of the Breathalyzer, the breath is direct..
A 2.00 g sample of silver (Ag) was heated with excess sulfur (S) to produce 2.30 g of a "silver sulfide". Calculate the empirical formula of this sulfide, AgxSy, where x and y are the smallest whole-number moles of Ag and S, respectively. (remembe..
A gaseous reaction occurs at a constant pressure of 50. atm and releases 74.2kj of heat. Before the reaction, the volume of the system was 8.00L After the reaction, the volume of the system was 2.80L
A 2.0-liter sample of H2(g) at 1.00 atm, an 8.0-liter sample of N2(g) at 3.00 atm and a 4.0-liter sample of Kr(g) at 0.50 atm are transferred to a 10.0-liter container at the same temperature. Calculate the partial pressure of each gas and the tot..
Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume of concentrated sulfuric acid required to prepare 2.80 L of 0.275 M H2SO4 solution.
Calculate the pressure and temperature at which 1.0 mol of H2O, HCl, and C6H6 corresponds to the same states as 1.0 mol of CH4 at 2.00 atm and 298
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