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Given mass of a gas 0.26g, pressure is 763mmHg and volume of 147mL.by using an ideal gas law calculate the molar mass of the gas
Calculate the partial pressure of the hydrogen gas using the atmospheric pressure and the vapor pressure of water at the temperature of the solution. Assuming ideal gas behavior, calculate the number of moles of hydrogen gas evolved.
A solution has a volume of 2.0 L and contains 36.0 g of glucose (C6H12O6). If the molar mass of glucose is 180 g/mol, what is the molarity of the solution.
Consider the reaction CaCN2 + 3H2O ->CaCO3 + 2NH3 . How much NH3 is produced if 187 g of CaCO3 are produced?
System conducts 1.30x10^2 cal heat to srroundings while delivering 316 cal work. What is the change in internal energy of the system (in Cal).
Identify the rate determining step, reaction intermediates and the experimental rate law (intermediates can not be in the rate law)
equilibrium constant, Kp, for the reaction = 0.295 (at 400 degrees C.)then write the kp of the reaction and Calculate kc at 400 degree Celsius.
C6H5OH(s) + 7O2(g) --> 6CO2(g) + 3H2O(g) A 2.000 gram sample of pure phenol, C6H5OH(s), is completely burned according to the equation above.
high boiling point are obtained now you need to identify the limiting reagent and compute the percent yield of nitrobenzene
The vapor pressure of a solution containing 53.6 g glycerin (C3H8O3) in 133.7 g ethanol (C2H5OH) is 113 torr at 400C. Calculate the vapor pressure of pure ethanol at 400C
How many liters of NO(g) can be made from 17.57 L of O2(g) and 16.55 L of N2(g) at STP?
A weather balloon at Earth's surface has a volume of 4 L at 294 K and 746 mm Hg. If the balloon is released and the volume reaches 4.19 L at 715 mm Hg.
A steel tank with a volume of 9.583 L contains N2 gas under a pressure of 4.972 atm at 31.8 °C. Calculate the number of moles of N2 in the tank.
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