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The pH of a sample of rain is found to be 3.2. Calculate the percentage of HSO4- that is ionized in this sample, given that the acid dissociation constant for the second stage of ionization of H2SO4 is 1.2E-2.
Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9.30 10-8 at 700°C. 2 H2S(g) 2 H2(g) + S2(g) If 0.33 mol H2S is placed in a 4.7 L container
The rate law for a hypothetical reaction is rate=k[A]2 When the concentration is 0.10 moles/liter, the rate is 2.7 * 10-5 moles/liter second. What is the value of k?
Cannot be determined from the information provided. 9. Starting with the initial concentrations provided in the question above, what will be the equilibrium concentration of CO2? a) 1.6 M b) 1.8 M c) 2.0 M d) 2.2 M 10. What is KC for this process ..
Analysis shows that there are 1.8 moles of H2, 7.45e-05 moles of S2, and 7.2 moles of H2S present in a 50.8 L flask at equilibrium. Calculate the equilibrium constant Kc for the reaction.
a 365.0g sample of water,contains 23mg Au. How much gold is present in the sample in parts per million?
A hypothetical element Z has two stable isotopes: Z-46 = 46.046 u 64.08% Z-51 = 50.826 u 35.92% What is the average atom weight of the element?
A bag of potato chips contains 595 ml of air at 25.0 degrees celsius and a pressure of 775 mm Hg.Assuming the bag does not break, what will be its volume at the top of a mountain where the pressure is 424 mm Hg and the temperature is 10.0 degrees ..
Calculate the activation energy of this reaction in kJ/mol At what temperature would the half-life be 12.0 min?
How many moles of oxygen are consumed in burning 1.60 moles of benzene, C6H6?
a solution of .64g adrenaline in 36.0 g of CCl4 elevates the boiling point by .49 degrees C. What is the molar mass of adrenaline.
Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. Heat capacity of H2O(s) 37.7 J/(mol X K) Heat capacity of H2O(l) 75.3 J/(mol X K) Enthalpy of fusion H2O 6.01 KJ/m..
A 9.0×10-2 M solution of a monoprotic acid has a percent dissociation of 0.60%. Determine the acid ionization constant Ka for the acid.
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