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Consider the reaction of sulfur dioxide and water, which is represented by the following equation: 2SO2(g) + 2H2O(g) ® 2H2S(g) + 3O2(g) How many moles of electrons are transferred according to the equation that is written?
need to dissolve CaCl2 in water to make a mixture that is 31.0% calcium chloride by mass. If the total mass of the mixture is 405.5 g, what masses of CaCl2 and water should be used?
If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.519 grams of iron and 21.0 mL of 0.590M copper(II) sulfate react to form as much product as possible, how many millimoles (mmol) of the non-limiting reactant will remain unuse..
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=∞.
How many moles of CF4 can be produced when 5.00 mol C react with 8.00 mol F2?
The equilibrium constant for this reaction at 1400K is 4.7. A mixture of reactants and products at 1400K contains 0.035 M H2O, 0.050 M CH4, 0.15 M CO, and 0.20 M H2
Compute the work done when 55.0 grams of tin mixes in excess acid at the pressure of 1.00 atm and at a temperature of 24°C.
Bombardment of boron-10 with a neutron produces a hydrogen-1 atom and another nuclide. What is this nuclide
The normal boiling point for acetone is 56.5°C. At an elevation of 5300 ft the atmospheric pressure is 630. torr.
Compare a refrigerator set at four degree celcius and a freezer set at minus twenty degree celsius, both of which are operating in the room at the temperature of eighteen degree celsius.
Assume that the pH is low enough that CH3COOH is not dissociated at all and that the activity of water equals 1 just like for pure liquid water (after all, the solution is quite dilute). HINT: This problem requies you to keep and extra large numbe..
When the following equation is balanced using the smallest possible integers, what is the exponent of H2O in the reaction quotient expression
where C is a constant.The following table gives the equilibrium constant (Kp) at various temperatures for the reaction of nitrogen monoxide with oxygen gas that produces nitrogen dioxide
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