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The equilibrium constant, Kp, for the following reactions is 11.5 at 300oC when the amounts of reactant and products are given in atmospheres. At equilibrium, the partial pressure of PCl5 is 0.53 atm at this temperature. What is the partial pressure of chlorine gas once equilibrium has been established?
If you were to dissolve 15.0 mg of the antibiotic in 546 mg cyclohexane, at what temperature would you expect this solution to boil
How many total calories do you consume from these three organic substances when you eat 1 candy bar 3 times a day?
What is the pH at the equivalence point when 100.00 mL of a 0.200 M solution of acetic acid (CH3COOH) is titrated with 0.10 M NaOH to its end point?
A first order reaction has a half-life of 1.34 x 10^-3 hours. If the initial concentration of the reactant is 8.00M, what is its concentration after 4 half-lives?
A phase change occurs at 298 K and deltaS system - -13.5 J/K. What is the change in the entropy of the surroundings?
What alkene (including cis and trans isomers) would be produced by the dehydration of the following alcohols. Where possible, predict the relative amounts of each product according to Zaitsev's rule.
What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V2O5 with 40.0 g of calcium based on the following chemical reaction?
delta H = -174 kcal/mol (-728 KJ/ mol) methanol for the process. How many kilocalories are released by burning 2.00mol of methanol? 3- How many kilojoules are released by burning 55g of methanol?
Why is the density of an ethanol/water mixture dependant on temperature? and how would the density of the ethanol/water change IF the temperature was increased and decreased
Can someone please explain how to do this problem? I asked before but the past answers didn't really help A rectangular storage container with an open top is to have a volume of 50 cubic meters. The length of its base is twice the width.
If a second order reaction is found to have a rate constant k equal to 1.57E3 M-1s-1. Utilize the appropriate integrated rate law to find out the half-life of the reaction.
In a particular experiment, 2.25 g of NH3 and 3.75 g of O2 are placed in a container and allowed to react. How many grams of NO will have been formed when all of the limiting reactant has been consumed.
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