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If 35.0 mL of NO2 gas is completely converted to N2O4 gas under the same conditions, what volume will the N2O4 occupy?
50.0 mL of a 1.70 M solution is diluted to a volume of 248 mL. A 124-mL portion of that solution is diluted using 185 mL of water. What is the final concentration
Consider a liquid with a vapor pressure of 320. torr at 20.0 degrees C and a vapor pressure of 540. torr at 50.0 degress C. What is the normal boiling point of this liquid?
Draw a bromide that would undergo dehydrobromination (elimination of HBr) under basic conditions to give the compound whose name is below.
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water vapor? Express your answer with the appropriate units.
Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 25.0 L.
Using the technique of the previous problem ?E was found to be -2,000.00 kJ/mol at 298 K for an unknown liquid hydrocarbon. In another experiment it was determined that for each mole of hydrocarbon
If it were possible to obtain 100% yield, when the temperature was returned to the origenal value what would be the partial pressure of each gas be?
Describe how you could make 5 ml of 2 M potassium hydroxide solution if you have potassium hydroxide pellets available?
You prepared a 0.250 M solution by diluting 8.45(+-0.04)mL of 28.0(+-0.5)mL wt.%NH3 (density=0.899(+-0.003)g/mL up to 500.0(+-0.2)mL. Find the uncertainty in 0.250 M.
What is the pH at the equivalence point when 30.0 mL of 0.20 M HCl are titrated with 0.45 M NaOH at T = 298 K? Kw = 1.00 x 10-14.
Calculate the expected pH of the buffer after the addition of 1.0 mL of 1 M HCl. Remember that you are using 50 ml of the buffer so be sure to calculate the number of moles of acetic acid
what is the pH of a solution obtained by adding 3.50g of HBr to 435mL of a 0.639M solution of HNO3?
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