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Assuming that the reaction SO2(g) + H2O(l) --> H2SO3(l)is quantitative, how much sulfurous acid is formed when 100.0 g of sulfur dioxideare mixed with 60.0 g of water?
The element copper has an atomic weight of 63.5 and consists of two stable isotopes copper-63 and copper-65. The isotope copper-63 has an atomic mass of 62.9 amu and a percent natural abundance of 69.1 %.
The formal charge on the P atom is zero and It is best described with three resonance structures.
Calculate the mass of Nitrogen at room temperature dissolved at room temperature in an 80 L aquarium. Assume a total pressure of 1 atm and .78 mole fraction.
How many atoms are contained in one unit cell of of this element? The atomic mass of the element is 193.5 amu.
How many grams of a stock solution that is 87.5 percent H2SO4 by mass would be needed to make 275 grams of a 55.0 percent by mass solution.
Sulfur dioxide gas is oxidized in 50 percent excess air with 70 percent conversion to sulfur trioxide. The gases enter the reactor at 350 oC and leave at 450 oC.
The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature.
2 g of a hydrocarbon fuel is burned in a colrimeter that contains 250 grams of water initially at 25 degrees celcius. After the combustion, the temperature is 26.55 degrees celcius.
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Kb of NH3 is 1.8 × 10-5.
When isobutylene (CH3 - C=CH2) is treated with acid, two products result: 2, 4, 4-trimethyl-2-pentene and 2,4,4-trimethyl-1-pentene
Calculate the pH of the final solution after 250 mL of a 0.157 mol dm-3 solution of HCl is added to 500 mL of a 0.103 mol dm-3 solution of NaCN (Ka HCN = 6.2 × 10-10).
If 358 mL of H2SO4 is neutralized with 60.0 mL of 1.50 M NaOH, what is the initial concentration of the acid?
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