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burning 480 cm3 of propane measured at r.t.p,caused the temperture of 250 cm3 of water to increase by 42.5 celsius. calculate the heat of combustion of propane.
if 5.0 of nitrogen at 12 degree Celsius and 1.30 atm pressure reacts with the same volume of hydrogen at the same temperature and pressure, what volume of ammonia is obtained at that temperature and pressure?
A gas sample was collected over water at 25.3 degrees Celsius, The total pressure is determined to be 0.97 atm. What is the partial pressure of the gas that was collected?
What is the role of sodium sulfite? How does it work? Please use an equation to explain this. Why was the work-up step so important in this experiment? What can be found in the top layer, and the bottom layer in the extraction step?
When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2
12.0 moles of gas are in a 8.00 L tank at 23.2 C. Calculate the difference in pressure between methane and an ideal gas under these conditions.
when a mixture of these two gases are compressed to a smaller volume, which way does the reaction shift to? the reaction is originally at 588 kelvins and has an equilibrium constant of "k"=0.0180
Calculate the following values for a 0.0150 M solution of NaH2A. and Calculate the following values for a 0.0150 M solution of Na2HA.
Find the concentration of Pb2 in 0.0010 M KI saturated with PbI2. Include activity coefficients in your solubility-product expression. The Ksp of PbI2 is 9.8× 10-9. Hint from sapling below: Including activity coefficients, the solubility-product e..
If solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is 2021 kPa?
How much heat energy, in kilojoules, is required to convert 65.0g of ice at 18.0 degrees celcius to water at 25.0 degrees celcius.
Determine the molarity of a solution made by dissolving 20.0 g of NaOH in sufficient water to yield 436 mL of solution.
An experiment requires 42.0 g of ethylene glycol, a liquid whose density is 1.114 g/mL. Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylinder.
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