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What is the molarity of a solution that contains 36.0g of vitamin B1 hydrochloride (molar mass = 337g/mol) in 190mL of solution?
a gasous mixture of oxygen and nitrogen contains 32.8% nitrogen by mass. what is the partial pressure of oxygen in the mixture if the total pressure is 405mmHG?
dependent Schrodinger equations of a particle with mass m confined in the one-dimensional potential (1/2)kx^2 , where k is some constant.
must be dissolved in 15.0g of camphor to lower its freezing point by 2 degrees celsius? constant k of camphor = 37.7 (*C x kg)/mol
A chemistry student needs 80.0mL of acetone for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of acetone is 0.790g cm^-3.
Using a table of thermodynamic data calculate, the Delta H degrees for the following reaction (at 25 degrees C).
A mass of 0.0600 g of magnesium metal is completely reacted with excess hydrochloric acid. Write the balanced equation to answer the question. What volume of the gas at STP would be produced
oes this result mean that the change in enthalpy of this process must be negative in order for the process to be spontaneous under standard state conditions? How come?
A solution is prepared by adding 0.14 mole Na2HPO4 and 8.2 grams of NaH2PO4 to sufficient water to prepare a 1.00 L solution. What is the pH of the solution?
Molecular Mass by Freezing point Depression (Preliminary Lab).
the permangenate ion and determine the standard reduction potential for the reaction.
At equilibrium the concentration of CO (g) was found to be 0.046 M. Calculate the equilibrium constant for the reaction equation at 527 degrees celcius.
At a pressure of 1.00 atm and a temperature of 20 degree Celsius, 1.72 g CO2 will dissolve in 1 L of water. How much CO2 will dissolve if the pressure is raised to 1.35 atm and the temperature stays the same?
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