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At 700 K, the equilibrium constant, Kc, for the reaction H2 + I2 2 HI is 49.0. How many moles of H2 would have to be added to 1.00 mole of I2 in a 10.0-L flask to get a 90.0% yield
How many grams of ammonium sulfate can be produced in 30 mol of H2SO4 react with excess NH3 according to the equation 2NH3(aq)+H2SO4(aq)-->(NH4)2SO4(aq)?
BaSO4 is listed as insoluble. Actually, BaSO4 is highly soluble, Ksp=1.1e-10. What is the solubility, in mg/l?
Calculate the heat energy released when 29.0 g of liquid mercury at 25.00 C is converted to solid mercury at its melting point
What external pressures have moved mainstream medicine to accept alternative therapies? Have any alternative therapies been proven to work as well as standard treatments? Support your answer with information from the reading materials and/or inter..
Calculate the molar mass of the uknown compound. The boiling point elevation constant for water is0.52°C/m
It takes 580. J of energy to raise the temperature of 124.5 g mercury from 20.0°C to 53.5°C. Calculate the specific heat capacity and the molar heat capacity of mercury.
A 51 kg person drinks 400. g of milk, which has a "caloric" value of approximately 3.0 kJ/g. If only 15% of the energy in milk is converted to mechanical work, how high (in meters) can the person climb based on this energy intake?
A titration of 200.0 mL of 1.00 M H2A was done with 1.28 M NaOH. For the diprotic acid H2A, ka1 = 2.5 x 10^-5 and ka2 = 3.1 x 10^-9.
Then the potential of the mercury cathode was adjusted to -1.80 V vs. SCE, and the quantity of electricity passed during this second electrolysis was 64.17 cou- lombs. Calculate the weight percentages of CCl4 and CHCl3 in the original sample.
Compute the enthalpy change for this reaction per mole of this substance and dissolves via the reaction and the temperature of the solution rises to twenty eight degree celsius.
What is temperature of boiling water in Denver (in?C) at an elevation of 6000 ft ? 2000 m given that atmospheric pressure at that altitude is about 0.8 atm?
Find the mass of urea (CH4N2O) needed to prepare 50.8 g of a solution in water in which the mole fraction of urea is 7.55×10?2.
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