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If 1.0 atm H2S (g) are added to a 1.0 L flask containing an excess of I2 (s), what will be the equilibrium pressure of HI?
H2S (g) + I2 (s) --> <-- 2HI (g) + S (s) Kp = 1.34 * 10^-7
AgBr is the light-sensitive compound in most photographic films. Assume, when film is exposed, that the light energy absorbed dissociates the molecule into atoms.
Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.
Calculate the mass of HONH2 required to dissolve in enough water to make 250.0 ml of solution having a pHof 10.00 (Kb=1.1*10 (-8).
A mixture of twenty five grams of potassium nitrate(KNO3) and two grams of CuSO4*5H20 with 11.5 grams of water at 100 degree celcius temperature, 15 g ramsof water are mixed.
3 isotopes of argon occur in nature. Ar-36, Ar-38, and Ar-40. The abundance of each are as follow: 0.34%, 0.07%, and 99.59%.
The concentration of Mg2+ in seawater is 0.052 M. At what pH will 92% of the Mg2 be precipitated as the hydroxide salt? [Ksp for Mg(OH)2 = 8.9* 10-12.]
For each of the following equilibria, use Le Chatelier's principle to predict the direction of reaction when the volume is increased.
Determine the partial pressure. Calculate the total pressure and volume in liters at STP of Nitrogen, Helium and Neon mixture.
Calculate the molarity of each of the following solutions. (a) 29.0 g of ethanol (C2H5OH) in 545 mL of solution
Consider the gas-phase reaction A + 2B 2C + D. Starting with 1.0 mole of A and 1.0 mole of B in 2.0 liter container, the reaction proceeds to equilibrium at T = 103C with 8.6 × 10-2 moles of C now present.
If 2.45 g of N2H4 reacts and produces 0.650 L of N2, at 295 K and 1.00 atm, what is the percent yield of the reaction?
The boling point of water in city a is 94 degrees celcius and in city b it is 97 degrees celcius. which is at the higher elevation.
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