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a gas is placed in a storage tank at a pressure of 20.0 atm at 20.3 degrees celsius. as a safety device, there is a small metal plug in the tank made of alloy that melts at 125 degrees celsius. if the tank is heated, what is the maximum pressure that will be attained in the tank before the plug will melt and release gas?
Hydrogen sulfide () is a common and troublesome pollutant in industrial wastewaters. One way to remove is to treat the water with chlorine, in which case the following reaction occurs:
consider the gaseous reaction at 347 celsius N2+3H2-->2NH3 if 2.00 mole of N2 and 3.00 mole of H2 react, which of the two reactants is the limiting reagent.
1.00 mole of pure NOCl and .907 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of Cl2(g).
Half-life equation for first-order reactions: where is the half-life in seconds , and is the rate constant in inverse seconds . Part A What is the half-life of a first-order reaction with a rate constant
Hydrogen was cooled from 150 c to 50 c. It's new volume is 75 ml. What was the original volume?
During a tritration, 34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H2SO4 solution. What was the concentration of the original sulfuric acid solution?
Acid chlorides are used as electrophiles in the Friedel-Crafts reaction to prepare aromatic ketones. The reaction involves the transfer of an aromatic hydrocarbon with an acyl chloride in the presence of a lewis acid
The white precipitate obtained when cold HCl was added to an unknown solution was completely insoluble in both hot water and NH4OH
A student determines the mass of a bone to be 23.3751g. A 50 mL graduated cylinder contains 30.3 mL of water. When the bone is placed in the water-filled cylinder,
What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V2O5 with 40.0 g of calcium based on the following chemical reaction?
what mass of oxalic acid dihydrate, H2C2O4 + 2H2O is required to prepare 280.0 ml of a 1.51 M solution of oxalic acid
A solution of ethanol (C2H5OH) in water is prepared by dissolving 65.8 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution.
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