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Concentration of a SpeciesOne mole of NOCl gas is added to a 4.0L container. The NOCl undergoes slight decomposition to form NO gas and Cl2 gas. If the equilibrium constant, Kc, for the reaction is 2.0x 10-10 at 25'C, calculate the concentration of all the species at equilibrium at this temp.
A. Epinephrine, C9H13NO3, has a concentration of 10-10 M in circulating blood. Calculate the diameter of a round swimming pool with a water depth of 2.0 M that would be needed to dissolve 1.0 g (about a teaspoon) of epinephrine.
What is the molarity of a solution prepared by dissolving 10.5 grams of NaF in enough water to produce 750 mL of solution
Calculate the molarity of 736 mL of a solution that contains 153 g of sucrose C12H22O11.
A 4.10 g nugget of pure gold absorbed 287 J of heat. The initial temperature was 24.0°C. What was the final temperature?
Determine the theatrical yield if 1.56 grams of hydrogen is permitted to combines with 9.70 grams of nitrogen producing 1.43 grams of ammonia?
If ΔH = -60.0kJ and ΔS = -0.200kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
Predict the order for increasing binding energies of the C(1s) electron for the following compounds giving your reasoning.
Compute the mass of H 2 O formed when 22 grams of propane are burnt if 4.4grams of propane are burnt in excess O2 7.2g of H 2 O are formed.
If delta H for the reaction is -851.5 kJ/mol at 25'C, calculate the standard free energy change, delta G for the reaction at 25'C. Calculate the temperature at which the reaction changes from spontaneous to non-spontaneous.
At 100 degrees C, the vapor pressure of water, methanol, and ethanol are 760, 2625, and 1694 torr, respectively. Which counpound has the highest normal boiling point.
A 29.0-g sample of ice at -11.0°C is mixed with 113.0 g of water at 71.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
How many grams of diphenyl (C 12H10) must be dissolved in 655 g of benzene to lower the freezing point by 3 .20ºC.
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