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A 2.56 g sample of anthracene C14H10, was burned to heat an aluminum calorimeter (mass=948g). Explain the calorimeter contained 1.50 L of water with an initial temperature of 20.5 C as well as a final temperature of 34.3'C
a) Compute the molar heat of combustion of anthracene.
b) Suppose the actual value for ?H= -7150 kJ/ mol, what is the percentage error?
3, 4-dimethoxyacetophenone was my unknown ketone as well as when I reacted it with 2,4 DNPH the solution became a red color indicitating that it was a conjugated ketone.
25 mL of 0.100 M AgNO3 are mixed with 35 mL of 0.0500 M K2CrO4. (a) Calculate the concentrations of each species at equilibrium.
Calculate the concentration of each substance when mixing 40.0 mL of 0.1 M CH3COOH and 10.0 mL of 0.1 M CH3COONa
Fe 2+(aq) + 6CN- (aq) -->/
If 120 grams of Al reacts with 601 grams of Fe(III)Oxygen what is the mass of aluminum oxide formed in grams
what concentration of oxygen would be needed to maintain equilibrium in a system where NO and NO2 are known to be at equal concentrations
What kinetic energy must the electrons have in order to resolve a protein molecule that is 3.80 nm in diameter? Take the mass of an electron to be 9.11× 10-31 kg.
Based on the amounts of reagents specified in this experiment, calculate the theorectical yield of asprin (180g/mol) in terms of moles and grams.
If something goes wrong, all of the cyanide could end up in the air of the lab, calculate the minimum size of the lab to keep the concentration of hydrogen cyanide in the lab below 5% of the lethal dose.
An 95.4-mL sample of wet O2 is collected over water at 21.3 degrees celcius at a barometric pressure of 741mmHg (vapor pressure of water at 21.3 degrees celcius = 19mmHg).
Suppose that a certain biologically important reaction is quite slow at physiological temperature (37*C ) in the absence of a catalyst.
sulfur dioxide is an unwelcome result of burning soft coal in power plants. Some of the sulfur dioxide ends up as sulfuric acid ( H2SO4) in acid rain.
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