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A 15.8 g sample of a nonelectrolyte was dissolved is 104.0 g of water. The solution's freezing point was -1.9°C. What is the molar mass of the unknown compound?
A sample of gas at 47°C and 1.03 atm occupies a volume of 2.20 L.What volume would this gas occupy at 107°C and 0.789 atm?
What is the most likely reason OSHA requires ammonium nitrate to be segregated for sulfur or finely divided metals? Explain your answer.
The molar enthalpy of fusion of ice at 0 0C is 6.02 kJ/mol; the molar heat capacity of supercooled water is 75.3 J/molK. (a) One mole of supercooled water at -10 0C is induced to crystallize in a heat-insulated vessel.
The mass of the tablet was 0.162 g. What percent of calcium carbonate was in the tablet?
A solution of I2 was standardized with ascorbic acid. Using .1000 g sample of pure ascorbic acid, 23.25 ml of I2 were required to reach the starch end point.
a large cylinder of He gas,such as that used to inflate balloons,has a volume of 25.0 L at 22c and 5.6 atm. How many moles of He are in such a cylinder
16.57 The complex [Ni(NH3)6]2+ has a ligand field splitting of 209 kJ·mol-1 and forms a purple solution. What is the wavelength and color of the absorbed light.
The mole fraction of potassium nitrate in an aqueous solution is .0194. The density of the the solution is 1.0627 g/mL. Calculate the molarity of the solution.
Compute the pH at the temperature of 25 0C of a solution prepared by mixing 50 mL of 1.60 M sodium hydroxide solution to 0.5 of .0850 M Furoic acid HC 5 H 3 O 3 .
What is meant by a state of ‘dynamic equilibrium'? What happens to the concentration of reactants and products when a reaction reaches a state of dynamic equilibrium?
Calculate the theoretical yield of when 114 g of C2H6 reacts with 206g of Cl2 , assuming that and react only to form and .
Find out the Celsius temperature of 2.49 mol of gas contained in a 1.00 L vessel at 1.8 atm pressure.
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