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The Henry's Law constant for CO2 gas in H2O = 0.031 mol/L-atm at the temperature of 25 degree celsius. compute the solubility of CO2 in H2O at 25 oC in moles/L if the partial pressure of CO2 in the headspace water sample is 1.56 atm.
A gas occupies 5.38 L when the temperature is 45.0oC and at 1.00 atm of pressure. What temperature change (in K) will be needed to change the volume to 6.30 L at constant pressure
The products of the fusion are carbon-13 and a proton. a) Write a nuclear reaction for this process. b) How much energy is released when 1.00 g of B-10 is fused with alpha particles?
A cell composed of a platinum indicator electrode and a silver-silver chloride reference electrode in a solution containing both Fe2 and Fe3 has a cell voltage of 0.731 V.
why is it important to allow the flask and contents to cool to room temperature before weighing
What is the volume occupied by 0.265 mol of helium gas at a pressure of 1.32 atm and a temperature of 302 K.
the partial pressure of oxygen in air at sea level is 0.21 atm. using the data in table 13.2, together with henry's law, calculate the molar concentration of oxygen, in the surface water of a mountain lake saturated with air at 20 degrees celcius ..
Which of the acids in question #3 would be the best choice to create a buffer with pH = 7.35? If you had 250.0 mL of a 0.20 M solution of the acid, what mass of the corresponding sodium salt of the conjugate base would be required to make the buff..
draw the structures for all the products obtained from the Diels - alders reaction of 2 methyl 1,3 butadiene and propene
Write an equation to show how H2PO3- can act as a base with HS- acting as an acid. Then show H2PO3- can act as an acid with HS- acting as a base.
Determine the enthalpy change for the reaction. 2NO2 (g) -> 2NO(g) + O2(g) These are the given equations: NO + O3 -> NO2 + 02 DeltaH = -198.9 kJ / mol O3 -> (3/2)O2 DeltaH = -142.3 kJ/mol
2 nas 2 h2ol 2 naohaq h2gthe hydrogen gas generated is collected over water at 25.0degc. the volume of the gas is 535
When 24 mL of a 175 mL stock solution containing 1.6 M BaF2 is diluted to 70 mL, what is the concentration of Ba2+ in the new solution?
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