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The amount of 2.50 mol of a perfect gas is heated from 100.0 K to 320.0 K. as a result, the gas expands against a constant pressure. determined the work done by the system
Give the stereochemistry (chirality) of the product when Z-3-methyl-3-hexene is treated with BH3THF followed by basic H2O2 and then H+
How many grams will remain after 98.0 days if Phosphorus-32 has a half-life of 14.0 days Starting with 6.00g of ,?
In an adiabatic compression if one mole of an ideal gas with a Cv=5R/2, the temperature rises from 293 K to 325 K. Calculate the heat, work, change in enthalpy and change in internal energy
The formation of organic compounds by the reaction of Iron(II) sulfide and carbonic acid is described by the following chemical equation: 2 FeS + H2CO3 --> 2 FeO + 1/n (CHOH)n + 2 S
distilled Solution D: 9.08 (m/v) glucose Solution E: 5.0 (m/v) glucose and 0.9 (m/v) Where does each solution go under 1. Crenation, 2. Hemolysis, 3. Neither. Each solution should be placed under one of the 3 named.
Which of the following terms define(s) an acid according to the Bronsted-Lowry theory?
Calculate the molarity of a 5.72 m aqueous sucrose (C12H22O11) solution with a density of 1.50 g/mL.
derive an expression for the compression factor of a gas that obeys the equation of statenbsp pv - nb nrt where b and
A rigid tank contains 1.50 moles of an ideal gas. Determine the number of moles of gas that nust be withdrawn from the tank to lower the pressure of gas from 25atm to 35 atm.
At constant pressure, the combustion of C2H6 releases 259 kJ of heat. Find delta H for the rxn: 2 C2H6 (g) + 7O2 (g) -> 4CO2 (g) + 6H20(l)
what if any experimental evidence do you have that the equilibrium is affected by change in temperature. Briefly explain. Are your observation and explanation in (3) consistent with Le Chatelier's principle. Briefly explain.
The difference between the transition state and the energy of the products. C. The difference between the energy of the products and the energy of the reactants. D. Undefined because it depends on whether the reaction is endothermic or exothermic.
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