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Problem- A weather balloon with a volume of 200.0 L is launched at 20oC and 1.06 atm. The balloon rises to an altitude of 20,000 meters, where the pressure is 63 torr and the temperature is -63oC? What is the new volume of the balloon at that altitude?
State your answer by means of significant figures.
What is the solubility of CaF2 in a solution that has an equilibrium concnetration of 0.01 M EDTA ^ 4- (aq)? Ksp (CaF2) = 3.9 x 10^-11 and Kf for [Ca(EDTA)]2- = 5.0 x 10^10
The concentration of sugar (glucose, C6H12O6) in human blood ranges from about 80 mg/100 mL before meals to 120 mg/100 mL after eating.
how many times faster will the reaction occur at 43circ rm c than at 0 circ rm c? how many times faster will the
question you fill a 500 ml container with 100 ml of water and shut the lid. the water is at 25 degrees celcius. how
The equilibrium molar concentration of the FeNCS^2+ determined from a calibration curve, is 1.5 x 10^-4 mol/L. Calculate, in sequence each of the following quantities in the aqueous solution to determine the equilibrium constant for the reaction.
a solution of .64g adrenaline in 36.0 g of CCl4 elevates the boiling point by .49 degrees C. What is the molar mass of adrenaline.
Explain how is the pKa of a phenol different than an aliphatic alcohol. Can a phenol be deprotonated by 3 M NaOH, can aphenol be deprotonated by NaHCO3
What is the balanced equation for the saponification of glyceryl trioloeate and sodium hydroxide
a mixture consists of 35% He(g) and 65% N2(g) by mass. If it exerts a total pressure of 2.15 atm, what is the partial pressure of helium
Assume that you started with only 1.80 g of sodium benzoate. Assuming that the reaction proceeds to form benzoic acid, what would your theoretical yield be? use two decimal places
Rates increase with increasing concentration of reactants because there are more collisions between reactant molecules. At higher temperatures, a larger fraction of molecules have enough energy to get over the activation energy barrier.
In combustion studies of the use of H2 as an alternative fuel, HO is sometimes formed in flames by the reaction, H(g) + 1/2 O2(g) HO(g)
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