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The purification of hydrogen gas is possible by diffusion through a thin palladium sheet. Calculate the number of kilograms of hydrogen that pass per hour (in kg/h) through a 4.7 mm thick sheet of palladium having an area of 0.25 m2 at 500°C. Assume a diffusion coefficient of 6.0 x 10-8 m2/s, that the concentrations of hydrogen at the high- and low-pressure sides of the plate are 4.8 kg/m3 and 0.72 kg/m3, and that steady-state conditions have been attained.
Calculate the molarity of 500.0 cm3 of solution containing 18.5 g of calcium nitrate Ca(NO3)2
The infrared spectrum of CH3CH2NH2 shows two absorptions not shwon by bromoethane. Identify the bonds responsible for these two absorptions.
How much heat in kilojoules is evolved in converting 1.50 mole of steam at 150 deg celsiys to ice at -35.0 deg. celsius? The heat capacity of steam is 1.84 J/g. deg celsius.
What is the molarity of a solution containing 1.35 mol H2SO4 in 245 mL of solution
Calculate the change in entropy (in J/K) when 89.8 g of nitrogen gas is heated at a constant pressure of 1.50 atm
The increase in the rate of reaction with temperature is due to A. increase in the number of effective collisions. B. decrease in activation energy.
If 75.0 mL of 0.250 M HNO3 and 75.0 mL of 0.250 M KOH are mixed, what is the molarity of the salt in the resulting solution?
When 4.70 g of a nonelectrolyte solute is dissolved in 915 mL of water at 21 degrees C, resulting solution exerts an osmotic pressure of 839 torr.
when sodium azide , NaN3 , is activated in an automobile air bag , nitrogen gas and solid sodium are produced . if 0.0500 moles of NaN3 react , what mass , in grams , of nitrogen would result ?
At a certain temperature, the equilibrium constant for the reaction 2HI(g)39. At a certain temperature, the equilibrium constant for the reaction 2HI(g) H2(g) + I2(g) is 0.49.
What volume of 0.140 M Hydrochloric acid is required to neutralize 2.68g of Magnesium hydroxide.
If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.434 grams of iron and 12.2 mL of 0.52M copper(II) sulfate react to form as much product as possible.
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