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The atomic weight of a newly discovered el-ement is 10.600 amu. It has two naturally occuring isotopes. One has a mass of 10.000 gms and a natural abundance of 70.000%. What is the isotopic mass of the other isotope?
In a particular experiment, 2.25 g of NH3 and 3.75 g of O2 are placed in a container and allowed to react. How many grams of NO will have been formed when all of the limiting reactant has been consumed.
2ZnS + 3O2 = 2ZnO + 2SO2 how many moles of Zno are produces when 32 gms of oxygen is allowed to react with an excess of ZnS?
when 31g of phosphorus reacts with oxygen, 71g of an oxide phosphorus is the product. What mass of oxygen is needed to produce 13g of this product?
The concentration of each gas once equilibrium is reached. The new equilibrium concentrations if the volume is suddenly halved (still at 298K)
A sample of an unknown gas effuses in 12.4 min. An equal volume of H2 in the same apparatus at the same temperature and pressure effuses in 2.59 min.
Find the pH of a 0.130 M solution of a weak monoprotic acid with a Ka value of 1.6 *10(to the power of -6)
In a reaction 8200 g of sodium reacts with 74.00 g of ferric oxide to form sodium oxide and iron metal. Calculate the mass of sodium iron produced.
Ferrocene cannot be nitrated using the conventional HNO3-H2SO4 mixed acid conditions, even though nitration is an electrophilic
Determine the limiting reactant if 140 grams of Calcium phosphate combines with 3.63 mol of sulphuric acid and also explain how many moles of calcium sulphate can be obtained?
Suppose 10.0 g of CH4 is used in a reaction that can theoretically produce 95.8 g of CCl4. What is the percent yield of CCl4 if the reaction produces only 80.0 g of CCl4.
Calculate the amount of heat liberated (in kJ) from 399 g of mercury when it cools from 73.0°C to 12.0°C.
Calculate the volume of C2H2 that is collected over water at 23 Celcius by reaction of 0.751 g of CaC2 if the total pressure of the gas is 740 torr. (The vapor pressure of water is 21.07 torr .)
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