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For the reaction PCl5 <=> PCl3 + Cl2, Kc= 33.7. Calculate the reaction quotient Q to determine which direction the reaction will shift toward when 0.00650 M PCl5, 1.04 M PCl3 and 0.0500 M Cl2 are mixed together in a 1.0 L flask?
what would the coefficent of Al(NO3)3 be in the balanced equation?
Calculate the final concentration of solute when 25.0 mL of 3.0 M of carbose solution and 37.0 mL of 2.5 M carbose solution are mixed
If you drop 25 g warm nails initial temp 65.4 into coffee cup calorimeter that contains 100.0 g water at 20 degrees Celsius, what will the temperature be.
The first steps in the radioactive decay of 257 Uuh involves the rapid and successive emission of 2 alpha particles. [Note: Uuh is the symbol for ununhexium, which is element number 116.]
Why is the angular momentum of some nuclei and molecules observable. How is it observed? What are some typical results.
Calculate how many moles and grams of aluminum chloride can be made from 2.70 g of aluminum and 4.05 of chlorine. find the mass of aluminum chloride 2Al(s)+3Cl3(g)---2Alcl3(s).
A flask contains 400 ml of .05 M phosphate buffer that has a ph of 7.2. What volume of .05 M NaOH should be added to increae the ph to 8.2? (please show all steps in math as best as possible)
a sample of hfrac12o with a mass of 46.0 grams has a temperature of -58.0 agravec. how many joules of energy are
What concentration of the salt NaC2H3O2 must be added to shift the equilibrium toward the reactants so that the [H3O+] concentration is reduced to pH = 5.5
the slopes corresponding to standard Beer's Law plots were as follows: ?IA = 0.072 ?IB = 0.306 ?IIA = 0.760 ?IIB = 0.036 Using this data, calculate the ratio between the relative concentrations of MR- and HMR in this solution.
Calculate ?G° for the reaction of ammonia with fluorine. 2NH3(g) + 5F2(g) ? N2F4(g) + 6HF(g) Substance: NH3(g) F2(g) N2F4(g) HF(g) ?G° f (kJ/mol): -16.4 0 79.9 -275.4 179.1 kJ -179.1 kJ 1539.7 kJ -1539.7 kJ None of these choices is correct.
Assuming that the specific heat of water is 4.18 J/(g · °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene.
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