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Determine the volume, in mL, of 2.00 M HC2H3O2 required to prepare each of the following solutions: 0.20 M acetic acid, and 0.020 M acetic acid.
The barometric air pressure that day was 733 mm Hg. What is the pressure of the vapor inside the flask (in atmospheres) after the vapor had cooled and the students opened the flask momentarily?
Determine what mass of sulphuric acid would be needed to mix with 0.75 mol of sodium hydroxide(NaOH)?
what is the molar mass of a nonpolar molecular compound if 5.52 grams dissolved in 36.0 grams of benzene begins to
an aqueous solution contains 4.20 nh3 ammonia by mass. the density of the aqueous ammonia is 0.979 gml. what is the
A chemical engineer studying the properties of fuels placed 1.500 g of a hydrocarbon in the bomb of a calorimeter and filled it with O2 gas. The bomb was immersed in 2.500 L of water and the reaction initiated.
Alfred bought a new graduated cylinder for his chemistry class. It holds 416 milliliters of liquid. If the cylinder has a radius of 4 cm, then how tall is the cylinder?
that forms when gaseous nitrogen dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous nitric acid. Write a balanced chemical equation for this reaction.
The following set of reactions can be used to produce nitric acid, HNO3. Calculate the mass of nitric acid produced from the reaction of 15.5 kg of nitrogen gas with excess hydrogen gas. Each reaction in turn has an excess of the second reactant a..
How much heat energy, in kilojoules, is required to convert 61.0 g of ice at -18.0 C to water at 25.0 C ?
a) What is the mo;ar mass of the gas b) If the unknown gas is composed of 2.78 g of carbon and the rest is hydrogen, what is its molecular formula
Calculate the volume in liters of 88.2 lb of CCl4 (density = 0.00160 kg/cm3; 1 lb = 454 g). A. 64.0 L B. 40.0 L C. 28.0 L D. 25.0 L
Predict the physical state of ammonia at -95 degrees C (mp =-77degrees C, Bp =-33 degrees C) and normal atmospheric pressure.
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