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What is the gas pressure (in atm) inside a 1.89-L bulb that contains 1.56-g of Ne at a temperature of 21.1 C? Be sure to report the units as atm
An anesthetic contains 64.9 % carbon, 13.5 % hydrogen, and 21.6 % oxygen by mass. At 120 degrees C and 750 mmHg, 1.00 L of the gaseous compound weighs 2.30 g.
Calculate the pH of a buffer made with 0.50 M phosphoric acid and 0.75 M sodium dihydrogen phosphate. Ka = 7.5 x 10^-3
flask shaken until the solution was uniform. A sample of 25.0 mL of this glucose solution was diluted to 0.500 ml then determine how many grams of C6H12O6 are in 100 mL of the final solution?
if the initial water level in the graduated cylinder is 21.2 ml and the level rises to 27.7 ml after the object is placed in the cylinder, what is the volume of the object?
calculate the equilibrium pressure of N2O4(g) and NO2(g). (c) What percentage (by moles) of the original N2O4(g) is dissociated at the new equilibrium position (total pressure = 1.00 atm)?
It then gives off a photon having a wavelength of 1740 nm. What is the final state of the hydrogen atom? Values for physical constants can be found here.
Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100 cm3 at 95°C, and 1000 mmHg.
the solubility of O2(g) in water is 4.43 mg O2/100 g H20 at 20 degree Celsius when the gas pressure is maintained at 1 atm. What is the molarity of the saturated solution?
one heating 5.03 g of hydrate barium chloride, 4.23 g is left behind. what is the name of this hydrate?
sodium metal reacts violently with water to produce aqueous sodium hydroxide and hydrogen gas. calculate the enthalpy change for this reaction.
Draw a Lewis Structure for C3O2. Draw a Lewis Structure for C2H3NO5
A 14.31 g sample of hydrated magnesium sulfate (MgSO3• x H2O) is heated to remove the water of crystallization and 6.99 g of anhydrous magnesium sulfate (MgSO4) remains.
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