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The standard free energy of activation of a reaction A is 76.8 kJ mol%u20131 (18.4 kcal mol%u20131) at 298 K. Reaction B is one million times faster than reaction A at the same temperature. The products of each reaction are 10.0 kJ mol%u20131 (2.39 kcal mol%u20131) more stable than the reactants.
(a) What is the standard free energy of activation of reaction B?
(c) What is the standard free energy of activation of the reverse of reaction B?
Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide (H2O2)to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?
How much heat (in kJ ) is required to warm 13.0 of ice, initially at -13.0, to steam at 114.0? The heat capacity of ice is 2.09 and that of steam is 2.01
Compound A is optically active and has the molecular formula C5H10O. On catalytic hydrogenation (addition of hydrogen) of A, Compound B is obtained
how many grams of water are consumed if 4.0 g of hydrogen gas and 32.0 g of oxygen are produced
When power was turned off to a 30.0 gal. water heater, the temperature of the water dropped from 75.0°C to 22.5°C. How much heat was lost to the surroundings? (1 gal = 3.785 L) Assume the density of water is 1.00 g/mL.
Write a chemical equation for the formation of methionyl glycine from the constituent amino acids.
a solid,is thought to be either zinc or lead(2)nitrate.how are we going to determine the identity of the solid?
Calculate the molecular weight of the unknown acid.
At a particular temperature, Kp = 0.25 atm for the reaction N2O4(g) 2NO2(g) a. A flask containing only N2O4 at an initial pressure of 4.5 atm
To see the affect on W when n > N/2, calculate W for N = 20 and n = 9 and 11. Is the result at all surprising? Why? Can you explain why you get this result? What other choices of n would give similar results?
If 5.68 g of Cu was added to 3.18 g of S8, How much copper (I) sulfide would be produced?
Aluminum nitrate and ammonium chloride react to form aluminum chloride, nitrogen, and water. what mass of aluminum chloride is present after 74.7 g of aluminum nitrate and 56.8 g ammonium chloride have reacted completely.
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