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Aluminum sulphate is used in sand paper, among other uses. How many g of aluminum oxide dihydrate will be needed to produce 500 g of aluminum sulphate by the (unbalanced) reaction below? Al2O3 •2H2O + H2SO4 Al2(SO4)3 + H2O
A sample of gas is made entirely of carbon dioxide and water, and there are 259 moles of carbon dioxide and 513 moles of water. If the total pressure of the sample is 21 atm, what is the partial pressure of each gas?
Stoichiometry of reactions, When a mole of C7H16 is combusted, it reacts with 11 moles of O2. How many moles of CO2 product are obtained? How many moles of H2O product are obtained?
How many milliliters of 0.0120 M Na2S2O3 solution are needed to dissolve 0.740 g of AgBr.
What is the resulting pH of this solution? b. The OCl- form of this acid is less effective as a disinfectant
calculate the pH of the 1 L solution of 0.25 M TRIS plus the addition of 0.05 M HCL. Show how many moles of TRIS and TRIS HCL are present after the addition of the HCL. Use the Henderson Hasselbalch equation to calculate the pH?
During studies of the reaction below, 2 N2H4(l) + N2O4(l) ? 3 N2(g) + 4 H2O(g) a chemical engineer measured a less-than-expected yield of N2 and discovered that the following side reaction occurs
What atomic or hybrid orbitals make up the sigma bond between Br and Cl in bromine trichloride, BrCl3 ?
Suppose one wated to take another approach where C is heated until 5% of the atoms occupy the electronically excited state. Consedering only the lowest-energy ground state and the elctronically excited state
An unknown mass of each of sand, initially at 24.0, absorbs 1970 of heat. The final temperature is 62.2 degrees C. Find the mass of sand.
Would your calculation of the atomic mass of the metal be too high or too low if your hot metal sample cooled off, unbeknownst to you, while being transferred to the calorimeter?
when a metal was exposed to light at a frequency of 4.63*10^15 Hz, electrons were emitted with a kinetic energy of 3.10*10^-19 J.
In combustion studies of the use of H2 as an alternative fuel, HO is sometimes formed in flames by the reaction, H(g) + 1/2 O2(g) HO(g) Use the data below to calculate the value of Kc
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