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As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.70 atm and a temperature of 25.0 *C , what is the solubility of N2 in a diver's blood? [Use the value of the Henry's law constant k calculated in Part A, 6.26*10^-4 mol/(l*atm).] Assume that the composition of the air in the tank is the same as on land and that all of the dissolved nitrogen remains in the blood.
Oxalic acid, H2C2O4 has acid dissociation constants Ka1=5.9x10^-2 and Ka2=6.4x10^-5. What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H2C2O4
the brown gas no2 and the colorless gas n2o4 exist in equilibrium. in an experiment 0.625 mole of n2o4 was introduced
A 0.831-g sample of SO3 is placed in a 1.00 L container and heated to 1100 K. The SO3 decomposes to SO2 and O2: 2SO3 (g) 2SO2 (g) + O2 (g). At equilibrium the total pressure in the container is 1.300 atm.
Suppose that 0.92 of water condenses on a 85.0 block of iron that is initially at 22. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in ) of the iron block? (Assume a constant enthalpy ..
Integrate the expression = 1/V (?V / ?T) at constant pressure, assuming that is independent of temperature. By doing so, obtain an expression for V as a function of T and at constant P.
Would entropy for a gas be heat Irreverisibly be greater than, less than or equal to a gas heated reversibly? Explain
a sample of oxygen gas occupies a volume of 2.00 l at 27 oc and 2.00 atm pressure.nbsp what volume in l will this
A solution is made by mixing 0.5 L of 1.0 molarity KBr and 0.5 L of 1.0 Molarity K3PO4. What is the concentration of each ion in the solution
Glycine has the structure NH2CH2COOH. it can lose a proton from the carboxyl group and form chelate rings bonded through both the N and one of the O atoms. Draw structures for all possible isomers of tris(glycinato)cobalt(III).
what is the main purpose of scratching beakers wall during the synthesis of the
Calculate the molar mass of a gas that has a density of 0.232 g/L at 156 oC and 222 torr. Use R = 0.0821 L-atm/mol-K for the value of the gas constant.
Compounds of boron and hydrogen are remarkable for their unusual bonding and also for their reactivity. With the more reactive halogen
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