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In one experiment 1.0 mol H2O and 1.0 mol CO are put into a flask and heated to 350 C. In a second experiment 1.0 mol H2 and 1.0 mol CO2 are put into another flask with the same volume as the first. This mixture is also heated to 350 C. After equilibrium is reached will there be any difference in the composition of the mixtures in the two flasks?
The angular momentum quantum number (?), the magnetic quantum number (m?), and the spin quantum number (ms) have strict rules which govern the possible values. Identify allowable combinations of quantum numbers for an electron
At a certain temperature, K = 9.1 10-4 for the following reaction. FeSCN2+(aq) Fe3+(aq) + SCN -(aq)
In the Balmer-Rydberg equation, what value of is used to determine the wavelengths of the Balmer series?
What is the percentage composition of a compound consisting of carbon and hydrogen if 58g of the compound has only 10g of hydrogen.
When 0.2250 g Mg was heated with 0.5331 g N2 gas, all the Mg was consumed forming 0.3114 g Mg3N2.What mass of N2 is left over ?
What mass of C4H6 in grams is consumed in the reaction below when 39.8 grams O2 (g) are also consumed? C4H6 (g) + O2 (g) ' CO2 (g) + H2O (g) (not balanced)
A 7.50 g piece of iron at 100 C is dropped into 25.0g of water at 22.0 C. Assuming that the heat is lost by the iron equals the heat gained by the water, determine the final temperature of the iron/water system. Assume a heat capacity of water 4.1..
The reaction of calcium bicarbonate, Ca(HCO3)2 with hydrochloric acid, HCl, produces a solution of CaCl2, gaseous carbon dioxide, CO2, and water, H2O.
Calculate the mass ( kg ) of the solute C4H8O and the volume ( mL ) of the solvent C6H6 that should be combined to generate 6450 g of a solution that is 2.07 m C4H8O.
Determine the partial pressure and total pressure of each gas in the vessel and process of reaction runs until eighty five of the Oxygen is used and the vessel get cooled to its starting or initial temperature.
The initial concentrations of the three gases are 0.550 M H2S, .550 M H2, and .275 M S2. Determine the equilibrium concentrations of the gases.
A compound containing nitrogen and oxygen is decomposed in the laboratory and produces 1.78 of nitrogen and 4.05 of oxygen emperical formula
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