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Phosphoric acid can be prepared by reaction of sulfuric acid with "phosphate rock" according to the equation: Ca3(PO4)2 + 3H2SO4 -> 3CaSO4 + 2H3PO4 What is the molar mass of Ca3(PO4)2?
The density of gold is 19.31 g/cm3, and the density of platinum is 21.43 g/cm3. If equal masses of gold and platinum are transferred to equal volumes of water in seperate graduated cylinders, which
If 0.176 moles of Mg have combined with 0.220 moles of O, what is the empirical formula of the product?
Density measurements can be used to analyze mixtures. For example, the density of solid sand (without air spaces) is about 2.84g/mL. The density of gold is 19.3 g/mL. If a 1.00kg sample of sand cont
A solution of ethanol (C2H5OH) in water is prepared by dissolving 65.7 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this
The stomach to give carbon dioxide, water and a soluble ionic salt. write a balanced equation for the reaction involving hydrotalcite and the hydrochloric acid.
If you used the 8900 kilojoules you expend in energy in one day to heat 51000 of water at 20, what would be the rise in temperature?
Once released into the atmosphere, the SO2 is likely to react with oxygen to form SO3. What can happen next if the SO3 encounters water droplets?
calculate the number of moles of gaseous N2 contained in a sample of 300 ml of gas saturated with water vapour at 25 degree celcius and 95 kPa.
A sample of 1.42 g of Helium and an unweighed quantity of Oxygen are mixed in a flask at room temperature. The partial pressure of Helium is 42.5 torr and of oxygen is 158 torr. What is the mass of
In the commercial manufacture of nitric acid, how many liters of nitrogen dioxide will produce 30 liters of nitric oxide given that both gases are at STP?
How many grams of sodium sulfide are formed if 1.60 g of hydrogen sulfide is bubbled into a solution containing 2.13 g of sodium hydroxide, assuming that the sodium sulfide is made in 94.0 % yield?
A solution was prepared by dissolving 28.0g of KCl in 225g of water. Calculate the mass percent of KCl in the solution.
A solution is prepared by condensing 4.00L of a gas, measured at 27°C and 746mmHg pressure into 58,0g of benzene. Calculate the freezing point of this solution.
How many joules of heat are required to heat 143 g of aluminum from 55.0 oC to 66.5oC?
The pressure inside the flask is 390 torr at 20 degrees C. What is the mass percent of MgO in the mixture? Assume that only the MgO reacts with CO2.
Radio wave radiation falls in the wavelength region of 10.0 to 1.00E+3 meters. What is the frequency of Radio wave radiation that has a wavelength of 426 m.
What is the molarity of a HCl solution if the reaction of 200mL of the solution with excess CaCO3 produces 10.5L of Co2 gas at 725mmHg and 18C?
Assuming zinc is the limiting reagent, how much zinc (in grams) do need to fill a 1.0 liter balloon with hydrogen gas at a temperature of 25 degrees celcius and a pressure of 780 mmHg.
If 450 g SO2 escaped into the atmosphere and all the escaped SO2 were converted to H2SO4. How many grams of H2SO4 would be produced in the atmosphere?
Which of the following statements about colligative properties of solutions is FALSE?
Given that the C-to-C bond in ethyne is a triple bond, the average C-H bond energy in CH4 is 415 kJ/mol along with information in the Chemistry Tables link to the left, calculate the average C-H bo
What mass of calcium metal could be obtained from one kg of limestone that is 50.0% pure CaCO3?
Consider a hydrogen atom in its ground state. What is the energy of its electron? Consider the hydrogen atom in an excited state of 3s^1. What is the energy of its electron?
What mass of hydrogen can be produced from 2.90 g of aluminum and 14.0 g of HCl in the above unbalanced reaction? Use at least as many significant figures in your molar masses as in the data given.