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The mole fractions of CO2 and O2 in the atmosphere have been estimated to be 4.2 x 10-5 and 0.2, respectively. Given the Henry's law constants of 1,600 and 43,000 atm, respectively, calculate the ratio of CO2:O2 in both the atmosphere and in the ocean.
The electron in the He+ ion is excited to the n = 2 principal state. What is the energy of the electron now?
A 21.10 g sample of liquid ethanol is initially at -36.90 oC. If the sample is heated at constant pressure (P = 1 atm.), how much kJ of energy are needed to raise the temperature of the sample to 100.60 oC.
Using the intermolecular bonding between H2O moleculesin it's two condensed phases (solid ice versus liquid water), explain the observed phenomenon that
In the lower troposphere, ozone is one of the components of photochemical smog. It is generated in air when nitrogen dioxide, formed by the oxidation of nitrogen monoxide from car exhaust, reacts by the following mechanism.
If 158 mL of wet H2 is collected over water at 24C and a barometric pressure of 737 torr, how many grams of Zn have been consumed?
In 0.04 M NaOH at 20*C, the decomposition of H2O2 and O2 is first order. If the half-life is 654 minutes, what would be the concentration after 100.00 minutes of a solution initially at 0.200 M
A Solution of 1.69g of this compound in 9.23g of benzene freezes at 2.18 degree celsius. What are the molecular formula and molar mass of the compound? ( the normal freezing point of pure benzene is 5.50 degree celsius)
Using this equation, determine how many moles are formed for every one mole of KIO3. KIO3 + 5I + 6H ? 3I2 + 3H2O + K B)Using this equation, determine how many moles S2O3 are needed to titrate the number of moles of I2 calculated in A.
imagine that you dissolve 10.0g of a mixture of nano3 and kf in 100.0g of water and find that the temperature rises by
if our eyes could see a slightly wider region of the electromagnetic spectrum we would see a fifth line in the balmer
Calculate the fraction of atoms in a sample of argon gas at 400K that have an energy of 10.0 KJ or greater.
Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8x10-5)
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