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At 21.0 °C, a solution of 32.32 g of a nonvolatile, nonpolar compound in 32.77 g of ethylbromide, C2H5Br, had a vapor pressure of 305.0 torr. The vapor pressure of pure ethyl bromide at this temperature is 400.0 torr. Assuming an ideal solution, what is the molecular mass of the compound?
10.0 L gas cylinder is filled with 5.20 moles of gas. The tank is stored at 1 C. What is the pressure in the tank?
Explain why a 1m solution of the compound FeCl2 in water has a lower freezing temperature than a 1m solution of KCl in water and what is the empirical formula of a compound
does it mean that the solution will shift towards the products because there is excess of reactants? what does it mean when the solution is orange (is it shifting towards products or reactant)?
How do you calculate the force of water hitting a concrete cylindrical pole. The velocity of the water is 2 ft/s, the depth of the water is 10 ft, and diameter of the pole is 3 ft. So what would be the total force exerted on the pole by the water?
How much heat is required to melt 15 grams of ice at 0C? How much heat is released when 100 grams of steam condenses at 100C? If a system of ice and water has a mass of 12 grams
Determine what amount of heat is required to increase the temperature of sixty grams of ethylene glycol from 15.1 degree Celsius to 40.3 degree Celsius?
Your starting mixture contains both KCl and KClO3. Suppose that your starting mixture weighed 2.040 grams total, and suppose that you dertermined during your reaction that you produced 0.0072 mols of O2
What is the specific heat capacity of a metal that has capacity of a metal that has a mass of 25.00 grams and absorbs 1000.0 j of heat in cooling from 80.0 c to 40.0 c?
If 3.93 g of sodium borohydride contains 2.5 × 10^23 H atoms, how many moles of H are present in 27 cm3 of sodium borohydride (of density 1.074 g/cm3)?Answer in units of mol
What was the volume occupied by the sample under the new conditions - Determine what volume of 3.00M HCl in liters is required to react
Two compounds have the same empirical formula. One substance is a gas, the other is a viscous liquid. How is it possible for two substances with the same empirical formula to have markedly different properties?
What is the most important attractive forces (London dispersion, dipole dipole, hydrogen bonding) and the number of bonding domains
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