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Compute the work that must be done against the atmosphere for the expansion of the gaseous products in the combustion of 1.00 mol C6H6 (l) at 25 degrees Celsius and 1.00 bar.
A solid mixture weighing 5 gm consists of lead nitrate as well as sodium nitrate was heated below 600o C until weight of residue was constant. If the loss in weight is 28%, discover the amount of lead nitrate and sodium nitrate in mixture.
During the isomerization of trans-1,2-dibenzoylethylene C16H12O2 using 95% Ethanol C2H6O , and UV light irradiation. What is the overall equation for this reaction. What is the product
Calculate approximately the heat released when you are given a chemical equation as 2-methyl-1-propene CH 3 ) 2 C CH 2 reacts
metal a was determined to be 95extracted into methylene chloride with dethizone at ph6 when equal volumes of aqueous
How many moles of chloride were present in the unknown. d. What mass of cholride was present in the unknown? e. What was the mass percentage of cholride present int the original sample
Calculate the molar concentration of OH - ions in an 1.18 M solution of a weak base, hydrazine, N2H4. (Kb = 4.0 10-6). What is the pH of this solution
Consider the bonding in the subsequent using valence bond theory. For which would dish be the smallest
what is the chemical formula of a homonuclear diatomic ga if it has a pressure of 1.40 atm and a density of 1.82 gl at
if a microwave oven took75 seconds to heat 1.00 cups of water from 15.8 to95.9oc how many photons per minute does the
The electron in the n = 5 level of a hydrogen atom emits a photon with a wavelength of 1280 nm. To what energy level does the electron move?
What is ozone and how it works as a protective molecule for our environment? What are the effects of CFCs on the ozone layer.
An ethylene glycol solution contains 21.2 g of ethylene glycol in 85.4 ml of water. Compute the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water)
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