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A 4.50-g sample of liquid water at 25.0 C is heated by the addition of 133 J of energy. The final temperature of the water is __________ °C. The specific heat capacity of liquid water is 4.18 J/gK.
commercial concentrated aqueous ammonia is a solution of 28.0%, by mass, ammonia, NH3, (molar mass=17.0 g/mol) in water. the density pf the solution is .900g/mL.
Physiological saline solutions used for intravenous injections have a concentration of 0.90% NaCl by weight
By Solving this problem student understand about isotopic abundance and how to calculate atomic weight (average atomic mass) of an element -
Suppose that in changing samples, a portion of the water in the calorimeter weere lost. In what way, if any, would this change the heat capacity of the calorimeter?
2NO2 + Cl2 = 2NOCl The inital pressure of NO2 was 1.577 atm and the inital pressure of Cl2 was 0.427 atm. At equilibrium, the partial pressure of NOCl is 0.624 atm. Calculate K.
In high spin complexes, the crystal field splitting energy is small and in low spin complexes, electrons are concentrated in the lower energy orbitals.
How much heat (in kJ) is evolved in converting 1.00 {mol} of steam at 160.0C to ice at -45.0C? The heat capacity of steam is 2.01 J/g*C and of ice is 2.09 J/g*C.
Find out how much energy is needed to raise the temperature of 22.8 g of diethyl ether from -10.0 degree celsius to 142.0 degree celsius?
The mass of a cube of iron is 292 g. Iron has a density of 7.87 g/cm3. What is the mass of a cube of lead that has the same dimensions.
If 1.50 g of (NH4)2SO4 is dissolved in enough water to form 200. mL of solution, what is the molarity of the solution.
a gas has a volume of 95 mL at a pressure of 930 torr. what volume will the gas occupy if the pressure is increased to 970 torr?
How much heat is required to vaporize 353 g of liquid ethanol at its boiling point? ΔHvap = 38.6 kJ/mol.
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