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A 0.00062G sample of benzene (C6H6) is dissolved in 200.0 mL of water. The solution gives an absorbance of 0.102 at 227nm using a 1.0 cm cell. A separate water sample containing benzene gives an absorbance of 0.0844 at 227nm in a 1.0 cm cell. What is the concentration of benzene in the water sample?
According to the data, what is the value of delta H for the reaction.
When pure carbon burns in air, 10.0 kg of carbon react with the oxygen in the air to form 36.7 kg of carbon dioxide. Calculate the percentage of oxygen contained in carbon dioxide.
A particular gaseous hydrocarbon that is 82.7% C and 17.3% H bymass has a density of 2.33g/L at 23oC and 746 mmHg. What is the molecular formula of this hydrocarbon?
comment on the situation in this case. is the positive charge of hydronium ion on the least electronegativity atom? is this reasonable? is there a choice?
Calculate Q,W and delta U for the conversion of 1 mole of liquid water to steam at T = 100C and P = 1 atm. The heat of vaporization of water is 9720 cal/mol.
A 1.0 ounce piece of chocolate contains 15mg of caffeine, and a 6.0 ounce cup of regular coffee contains 105mg of caffeine. How much chocolate would you have to consume to get as much caffeine as you would from 2.0 cups of coffee.
Use line notation to represent the electrochemical cells for each of the following overall redox reactions. Part A: Ni2+(aq)+Mg(s) Ni(s)+Mg2+(aq)
the students product is contaminated with 5% o a constitutional isomer. give the approximate expected melting point of the students product
A rock contain 3.2 grams of a radioactive isotope, uranium-235, . Determine what was the original amount of uranium-235 in the rock If the rock has undergone 2.75 half lives, and how old is the rock?
What is stray light. How does it affect the performance of the spectrometer? Can one minimize it in the design of a spectrometer.
Choose the answer which lists ionic compounds NaCl, MgS, KCl, and K2S in order of increasing lattice energy (smallest lattice energy listed first).
Then use the estimate to calculate the heat of formation of ethanol from the heats of formation (in KJ/mol) of CO2: -?394, and H2O: -?242.
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