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If the formula for magnesium fluoride is MgF2 and the formula for potassium chlorate is KClO3 , then what is the formula for magnesium chlorate?
When the solution of copper was heated in the flame, a bluish green color was observed . how you might show experimentally the green color results from a mixture of light of various wavelengths or if only 1 wavelength of light is being emitted?
Compute the mass of Trisodium phosphate required to remove all Ca^2+ ions from 2.50 Litres of the H 2 O sample?
In Horner-Wadsworth-Emmons reaction, a 1,2-disubstituted alkene was produced in which the olefinic protons exhibited at vicinal coupling of 9.0 Hz in the 1H NMR. What is the stoichiometry of the double bond.
Find out what will be the half-lives if [NOBr]o = 0.054 M - The rate constant for the second order reaction Is 0.80 M-1s-1 at 10 degree celsius temperature
Calculate the molecular weight of the compound? Given that Kf=1.86 and the compound in not ionic.
To find the % by mass of a compound in a given sample - Determine the percent by mass of calcium carbonate in the sample. State any assumptions.
This given reaction: 2 O3(g) -→ 3 O2(g) has an empirically determined rate law (with a single unimolecular event). Determine what is the observed rate If k =4.0 × 105s-1, [O2] = 0.2M and [O3] = 0.5 M?
Compute the number of moles of H2O will be formed from the reaction 75.1g benzene?
Find out What mass of the NaHCO3 reacts with the vitamin C When the tablet dissolves in H2O, it "fizzes" because the reason for this is the CHO3 reacts with the citric acid(C6H8O7 a weak organic acid) and the vitamin C?
Gas stoichiometry and Percentage of calcium carbonate in the sample
Find the concentration and pH solution - What is the pH of a solution of 0.65 M acid and 0.51 M of its conjugate base if the pKa = 5.30?
Find out the required pressure to compress 180 liters of N at 1.0 atm into a tank whose volume is 34 liters.
Calculate the mass of Sodium and Zinc in grams in the following equations using ideal gas law - Determine the amount of Zinc metal in grams consumed in the reaction.
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