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If you prepare a 1.00 m solution of NH4ClO4 beginning with water at 25.5C, what is the final temperature of the solution in C? Assume that the specific heats of both pure H2O and the solution are the same, 4.18 J/( K*g)
When 3.00 g KNO3 are dissolved in 50 g glycerol, the freezing point changes from 17.8°C to 13.6°C. What is the freezing point depression constant (Kf ) for glycerol.
Imagine that you model your lungs as a 5 L sealed balloon at sea level: Estimate the volume of your lungs at 100 m below the sea level.
if 19.65mL of .145M nitric acid is required ti neutralize 50.0mL of barium hydroxide what is the molar concentration of the base? 2HNO3+Ba(OH)2-->Ba(NO3)2+2H2O
The half-life of radon-222 is 3.8 days. How much of a 100 g sample is left after 15.2 days?
determine K for this reaction When a sample of 5.63 grams of pure C 5 H 6 O 3 (g) was sealed into an otherwise empty flask of 2.50 L and heated to 200.
what would be the atmospheric pressure of MTBE in Pa If this sample were at equilibrium with atmospheric MTBE? KH = 1.7 M/atm.
NH3(Ammonia ) is widely used in many household cleaners and as a fertilizer. Calculate How much ammonia (in units of mol) is produced when 7.8 mol of H gas react with an excess of N gas.
An 11.0 gram sample of CaCl2(s) is dissolved in 125 grams of water with both substances at 25.0°C. If the final temperature of the mixture is 39.2 °C.
The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100°C.
Ammonia is often produced by reacting nitrogen gas with hydrogen gas. How many liters of ammonia gas can be formed from 23.5 L of hydrogen gas at 93.0°C and a pressure of 34.7 kPa?
The volume of a 24.0g sample of methane gas is 22.8L at 40.0*C and 4.00atm. What will it's volume be at 68.0*C and 4.00atm.
Compute the volume of the tank if this tank has 115 moles of neon gas and has a pressure of 57 atm at a temperature of 45 0C.
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