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(a) How much N2 in moles of gas is in a 40 kg diver's blood at 100 m depth. The diver is under 10.0 atm of pressure. Air is 75% N2. The Henry's law constant for N2 is 1.56*10^5 kPa*kg(H2O)/mol(N2). (b) Using the perfect gas law, if the diver rapidly resurfaces to 1 atm of pressure, how much N2 in Liters will come out of their blood?
A student takes 195. g of BaCl2, and reacts it according to the following equation: 3BaCl2 + Al2(SO4)3 → 3BaSO4 + 2AlCl3 How many moles of AlCl3 are formed?
For a reaction at equilibrium, which of the following is the best way to think about it?
If 85g of propane C3H8 is completely combusted with oxygyen to form catbon dioxide and water ,how many grams of oxygen are consumed
How many moles of water will be formed from 0.2 mole of CH4 reacting with enough O2. In this reaction CH4+2O2--->CO2+2H2O
Compute the amount of work done by the gas if all three weights were removed simultaneously during an isothermal expansion
which ions in water make it 'hard'? is it possible to test for only one of these ions quantitatively in the presence of the other.
What is the pOH of a Ba(OH)2 solution made by dissolving 0.081 grams of Ba(OH)2 in enough water to make 286 mL of solution
The heaviest known isotope of hydrogen is called tritium, 3/1 H. It decays by beta emission, and half-life of 12.3 years. What fraction of a tritium sample will remain after 5.20 years
An experiment requires 44.0 of ethylene glycol, a liquid whose density is 1.114 . Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylinder. What volume of the liquid should he use?
How much energy (heat) is released when 1.9 moles of H2 reacts with 0.7 moles of Cl2 to create HCl(g) if the ΔHrxn = -184.6 kJ.
A sample of an ideal gas at 1.00 atm and a volume of 1.89 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume.
Using concentrations, the solubility of [Ag+] in a solution of 0.01 M KCl is 1.8 * 10-8. Calculate the percent relative error when using concentrations for the solubility of [Ag+] compared to activities
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