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How many moles of ammonium sulfate can be made from the reaction of 30.0 mol of NH3 with H2SO4 according to the following equation? 2NH + H2SO4 > (NH4)2 SO4
How much heat is required to convert 27.0 grams of ethanol at 28 degrees celcius to the vapor phase at 78 degrees celcius?
In the titration of 50.0 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 10-4), with 0.50 M HCl, calculate the pH under the following conditions.at the stoichiometric point
Molar CuSO4(aq) and Pb(NO3)2(aq) solutions are in separate compartments of a voltaic cell. If sulfuric acid is then added to the Pb(NO3)2 solution, thereby forming a precipitate of PbSO4, what will
A protein subunit from an enzyme is part of a research study and needs to be characterized. A total of 0.185 g of this subunit was dissolved in enough water to produce 2.00 rm mL of solution. At 28
What is the vapor pressure(in mm Hg)of a solution made by dissolving 18.3g of NaCl in 500.0g of H2O at 70 degree celcius. The vapor pressure of pure water at 70 degree celcius is 233.7 mm Hg.
The other contains 8.3 L of helium at 4.1 atm of pressure. If the valve is opened, what is the final pressure of the two tanks combined?
A 0.500 L solution of 7.50 M hydrochloric acid is used to neutralize a 250.0 g sample of calcium hydroxide. Calcium chloride - a chemical used to control highway dust, strengthen concrete mixes, and
How many grams of ice at 0 degrees celcius and 101.3 kpa could be melted by the addition of 0.400 kj of heat?
What mass of CaCO3 will produce 8.0 L of CO2, measured at standard temperature and pressure conditions? Molar mass of CaCO3 = 100. g per mole.
When 157mg of dipentylamine was added to 122mg of benzoic acid and 2mL of water, a completely homogenous solution was formed. Draw the sturctures of the species present in the water.
A Saturated solution of potassium chloride is prepared in 100.0g of water at 20C. If the solution is heated to 50C, how much more KCl must be added to obtain a saturated solution?
A sample of gas is collected over water at a temperature of 35.0C when the barometric pressure reading is 763 torr. What is the partial pressure of the dry gas, given PH2O =42.2 torr?
Calculate the final temperature of the solution assuming no heat lost to the surroundings and assuming the solution has a specific heat capacity of 4.18 J/°C·g.
A 49g piece of ice at 0 degrees C is added to a sample of water at 9 degrees C. All of the ice melts and the temperature of the water decreases to 0 degrees C. How many grams of water were in the sa
A 493 mL sample of solution contains 33.2 g of CaCl2. Calculate the molar concentration of Cl in this solution
Methanol, a potential replacement for gasoline, can be made from H2 and CO by reactions CO + 2H2 - CH3OH. How will this reaction be affected if the volume of the container is replaced?
What is the value of work (w) when a piston of volume 0.2 L expands against an external pressure of 200 kPa to a volume of 3.4 L?
A soultion containing and unknown amount of tartaric acid with NaOH solution to titrate both acidid hydrogens. Write a balanced equation for the nuetralization reaction and calculate the molarity of
you have 3 L of gas at a certain temperature and pressure. What would the volume of the gas be if the temperature doubled and the pressure stayed the same?
How many moles of (NH4)2SO4 are there in 100.00 g of ammonium sulfate? How many moles of ammonium ions are in 100.00 g of ammonium sulfate? How many ammonium ions are in 100.00 grams of ammonium sul
An evacuated (empty) 276 mL glass bulb weighs 129.6375 g. Filled with an unknown gas, the bulb weighs 130.0318 g. Calculate the gas density in g/L, and express it with an appropriate number of sign
Assuming STP, how many liters of carbon dioxide are produce when 5.74 g of CaCO3 reacts with an excess of H3PO4.
Write the balanced net ionic equation for the reaction that occurs when 0.1 M solutions of copper(II) sulfate and calcium perchlorate are mixed.
The specific heat of an unknown metal is found to be 0.233 j kg. The law of dulong and petit predicts a molar heat capacity of J/K mol. Use this law to estimate the molar mass of the element.