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Consider an ideal gas which is allowed to expand slowly under constant temperature conditions. Derive an expression for the heat change for such a process, explaining any key stages in the derivation.
A 350.0 mL sample of oxygen gas was collected over water at a temperature of 25.0ºC and 740.0 mm Hg. How many moles of gas were there in this sample if the vapor pressure of water at 25.0ºC is 23.8 mm Hg?
how many grams of NH3 will be produced? Which reactant remains in excess, and in what mass?
If a bottle of nail polish remover contains 181 g of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL
The problem: CaCO3 can be roasted to produce CaO and CO2. This reaction is carried out in a flash connected to an open-end mercury manometer when the atmospheric pressure is 754 torr.
If a sample containing 2.01 mL of nitroglycerine (density = 1.592 g/mL) is detonated, how many total moles of gas are produced?
Explain how the calculated percent NaHCO3 and Na2CO3 by mass would be affected if the initial mixture were wet with water.
when 0.273-gm of Mg is reacted at high temperatures with N2 to produce 0.378-gm of a solid, MgxNy. Calculate the empirical formula of the product.
A 335 mL container holds 0.146 g of Ne and an unknown amount of Ar at 35°C and a total pressure of 628 mmHg. Calculate the moles of Ar present.
7.5g of ammonia at STP is heated to a temperature of 25C and simultaneously compressed to a volume of 8.0L. Calculate the new pressure of the gas.
When maleic acid is heated to about 100C it forms maleic anhydride, however fumaric acid requires a much higher temperature (250-300C) before it dehydrates
or the reaction H2(g)+CO2(g) H2O(g)+CO2(g) at 700C, Kc=.534. Calculate the number of moles of H2 that are present at equilibrium
Calculate the concentrations of Fe3+ and SCN- in the reaction mixture in part I when you add 10.00 mL of 0.200 M Fe3+ to 1.00 mL of 2.0 x 10-3 M SCN- and make up the total volume to 50.00 mL? What is the concentration of FeSCN2+?
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