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A student measures k for a certain blue dye to be 24.16 M^-1 at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.118 at 560 nm?
If 4.00 mL of vinegar needs 41.5 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.80 qt sample of this vinegar?
Verify the first equality in R (beta(delta e)^2e^Beta(delta e)/[e^Beta(delta e)-1]^2 using the chain rule, and then verify the second equality in the same bolded equation by evaluating the derivative with respect to Beta
The following osmotic pressures were observed for bovine serum albumin (BSA) in 0.15 M NaCl at 273 K. Calculate the molar mass of BSA.
determine the volume of .450m napo4 is needed to precipitate all the leadii ions from 190.0ml of .550m leadii
Ionization energy is the energy required to remove an electron from an atom in the gas phase. The ionization energy of lead is 715.0 kJ/mol.
At high temperature, ammonia reduces copper(II) oxide to the free metal: 2NH3(g) + 6CuO(s) => N2(g) + 3Cu2O(s) + 3H2O(g) Step 2: 2NH3(g) + 3Cu2O(s) => N2(g) + 6Cu(s) + 3H2O(g)
Calculate the mass of HONH2 required to dissolve in enough water to make 250 ml of solution having a ph of 10.00 kb 1.1 x 10-8
Now if your lab partner needed 7.030 x 1019 molecules of Sodium cyanide (NaCN), how many milligrams would you need to weigh out?
Given the information below calculate ?H°rxn for: C2H4(g) + 6F2(g) => 2CF4 + 4HF(g). H2(g) + F2(g) => 2HF(g) ?H° = -537 kJ C(s) + 2F2(g) => CF4(g) ?°H = -680 kJ 2C(s) + 2H2(g) => C2H4(g)
write the net ionic equation, a solution of tin II chloride is added to a solution of iron III sulfate
For the following reaction: 2A + B + C --> 3P If the rate of disappearance of A ((delta)A/(delta)t) is -0.77 mol/(L s), what is the rate of appearance of P in mol/(L s)?
The standard free energy for the neutralization of HCl with NaOH at 25 degrees celsius is -79.9KJ/mol. Calculate the equilibrium constant for the reaction.
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