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A quantity of HI was sealed in a tube, heated to 425C, and held at this temperature until equilibrium is reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 moles/liter. Calculate the equilibrium concentration of H2 (and I2 ). For the reaction H2 (g) + I2 (g) 2HI(g), Kc = 54.6 at 425C.
How much water must be added to 488 mL of 0.223 M HCl to produce a 0.134 M solution?
Determine mass of water is contained in 2.8 Litres of the vapor in this solution at 55 degree celcius temperature express your answer in grams
Calculate the maximum numbers of moles and grams of iodic acid (HIO3) that can form when 635g of iodine trichloride reacts with 118.5g of water.
What volume of oxygen, in ml, would be produced at STP (0 degrees C and 1.00atom) by the decomposition of 3.428g of sodium chlorate, according to 2NaClO3(s) -> 2NaCl(s) + 3O2(g)
Calculate the mass percent of a solution that is prepared by adding 40.0 g of rm NaOH to 408 g of {rm H_2O}.
What are the concentrations of each of the ions in a saturated solution of PbBr2, given the Ksp of PbBr2 is 2.1 x 10^-6?
An Ionic Compound has the formula M4(NO3)2(PO4)2. What is the net charge on the metal ion M in this Compound.
I am given the 10 ml of .200M Fe(NO3)3 and .25 ml of .00200 KSCN and 14.75 ml of .500 M of HNO3. How do I figure out the initial concentration of FE3+ and SCN-.
The mass percent of a three component gas sample is 58.0% C2H4O2, 14.6% NH3 and 27.4% CH2O. Calculate the partial pressure (atm) of CH2O if the total pressure of the sample is 0.340 atm.
calculate the pH of a solution that is prepared by mixing 75ml of 0.20 M (NH4)2SO4
Compute pH and [OH-] for each of the following solutions. (a) 8.1×10-2M Na2CO3, (b) 0.15M NaCN
The 9.163 g their air Air Cs equals 1005J/KG c in an inflated balloon is warmed over a toaster and increases in temperature by 11°C the balloon expands against one atmospheric pressure and changes volume for one liter to two liters
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