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What is the reaction order with respect to each reagent for the following reaction? Then write the rate law equation.
2A + 2B + C --> D + 3E
Exp Initial [A] Initial [B] Initial [C] Initial Rate (mol/Lsec)1 0.024 0.085 0.032 6.0 x 10-62 0.096 0.085 0.032 9.6 x 10-53 0.024 0.034 0.080 1.5 x 10-54 0.012 0.170 0.032 1.5 x 10-6
The second equivalence point was reached after 35.75mL of 0.1005 M hydrochloric acid was added to a 50.00 mL solution containing your sodium carbonate unknown., calculate the pH of the solution at the second equivalence point
NO is produced in the atmosphere at moderately low partial pressure by high temperature combustion. What is its fate as cooling occurs? To help address the question, calculate the equilibrium constant at 298 K and 1300 K for each reaction
Draw the Lewis structure for each including formal charges and describe in paragraph format how you went about solving the problem and making sure the answer was correct.
What is the mass percent, expressed to the proper number of significant figures, for each metal in the original metal mixture? Define all variables, show units, and show algebraic steps to your the answers.
How many equivalents of electrons were delivered to the unknown soln? What is the normality of the unknown solution?
A zero-order reaction has a constant rate of 3.50×10-4 M/rm s. If after 65.0 seconds the concentration has dropped to 1.00×10-2 M, what was the initial concentration?
Exactly 5.02 grams of an unknown gas was sealed in a 3.0 L flask at 37.0oC and a pressure of 1.25 atm. Which one of the following is most likely to be the unknown
Show your calculations for the pH when 0.00 mL, 4.00 mL, 6.00 mL, 12.00 mL (equivalence point), and 16.00 mL of 0.10 M HCl have been aded to an initial
Liquid carbon disulfide burns in oxygen to form carbon dioxide and sulfur dioxide gases. Calculate the number of oxygen molecules it would take to consume 500 molecules of carbon disulfide
in the resonance form caused by the delocalization of the immediately adjacent Nitrogen's lone pairs, there is a pi bond.
The total mass of pure metals produced = 0.4684 grams. compute the mass percent of CuCl2, and AgNO3, FeCl3 in the original mixture.
below, 8.34 atm each of H2 and Br2 were placed into a 1.00 L flask and allowed to react: H2(g) + Br2(g) 2 HBr(g) Given that Kc = 86.7, calculate the equilibrium pressure of Br2.
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