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Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl : Zn(s) + 2HCl(aq) = ZnCl2 (aq) + H2 (g). How many grams of zinc would you start with if you wanted to prepare 5.45L of H2 at 388mm Hg and 29.5C?
A 4.07 L sample of H2O(g) reacts at a temperature of 375°C and a pressure of 679 mm Hg. How many grams of NH3 can be produced?
when 50.0 gram of metal at 75.0 C is added to 100 grams of water at 15.0 C the temperature of the water rises to 18.3 C. Assume that no heat is lost to the surroundings. What is the specific heat of this metal
Which state in each of the following pairs has the higher entropy per mole of substance. 1. Ice at - 40 degrees C or ice at 0 degrees C 2. N2 at STP or N2 at 0 degrees C and 10 atm 3. N2 at STP or N2 at 0 degrees C in a volume of 50 L 4.
The latent heat of vaporization of water is 577 J/kg. If a person's body needs to lose 345 J of energy through sweating, how many kilograms of water in the form of sweat must be evaporated.
Calculate the pH of a 0.40 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.
A a student started with a mixture weighing 1.356 gm. The student recovered 1.543 g . Assuming that all calculations were done correctly what was the most likely source of error in the experiment
If 7.1 g of butanoic acid, C4H8O2, is dissolved in enough water to make 1.0 L of solution, what is the resulting pH? A table with Ka values can be found here.
Suppose a black-body chamber is constructed from 55.8 g (one mole) of iron and heated to 500 K. Classical theory and the observations of Dulong and Petit indicate that the total energy of vibration of iron atoms is 3RT per mole.
Find the pH and the concentration of each of the species of lysine in a solution of .010M lysine monohydrochloride (lysine-HCl)
For the diprotic weak acid H2A, Ka1 = 3.2 × 10-5 and Ka2 = 7.9 × 10-7. What is the pH of a 0.0400 M solution of H2A? What are the equilibrium concentrations of H2A and A2- in this solution
The equilibrium constant kp for the following reaction is found to be 4.31 *10^-4 at 375 degrees C. N2(g)+3H2(g) 2NH3(g) Calculate the partial pressures of all species when equilibrium is reached.
Which of the following buffers will have the lowest pH?
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