If 227 g of Co is reacted with iodine to give 2182.19 g of a Coxly...
If 22 g of some metal, M, is reacted with excess oxygen to give 29.4126 g of M2O5, what is the name of the compound?
According to the general procedure of Experiment A2b, 227 mg of (E)-stilbene (180.25 g/mol) was reacted with 435 mg of pyridinium bromide perbromide (319.82 g/mol) to afford 342 mg of meso-stilbene dibromide (340.05 g/mol) as a white solid. Calculate the percent yield for this reaction.
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EZ Data and calculations grams it iodine 1.849479 moles iodine grams in a start] 1.592g Lgrame tin at end 1.5749 dams tin ved 0.018 molestina ratto, moles I moeisn empirical formula name of compound 1.61419 mass of filter paper plus produet mass of filter paper mass of product 0.42939 1.1848 Table 1. Determination of the formula Mass of iodine, g 1.84947 9 amount of iodine, mol Mass of tin at start, g| 1 1. 59...
40.505-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide. Calculate the empirical formula of the product. D. 565. Cox Imal Co A 0.750-g sample of tin foil was heated in air and reacted with oxygen gas to give 0.953 g of tin oxide. Calculate the empirical formula of the product.
Fe2O3 (s) + CO (g) ----> Fe (s) + CO2 13.5 g of Fe2O3 is reacted with 15.0 g of Co. 8.30 g of Fe is obtained. Identify the limiting reagent and calculate the theoretical yield and percent yield for Fe.
5. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of prod Calculate the empirical formula of the iron sulfide.6. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.861 g of product Calculate the empirical formula of the iron sulfide.
A compound of cesium and iodine contains 52.01 g of metal and 49.37 g of nonmetal. How many grams of cesium are in a 85.15−g sample of the compound? How many grams of iodine? _g Cs _g I
Table 4.1 Mask of flask + iodine: 77.443g -Mass of empty flask: 75.41g =Mass of iodine used: 2.032g Mass of zinc used: 2.055g Table 4.2 Mass of beaker + crystals: 110.014g -Mass of beaker: 107.482g =Mass of crystals formed: 2.532g Table 4.3 Mask of flask + solid; 1st weighing: 76.845g Mask of flask + solid; 2nd weighing: 76.844g Mass of excess reactant recovered: ? I solved questions 1-4 2. How many grams of excess reactant remained after reaction: 76.844g-75.41g =...
002 14. When 10.0 g of phosphorous reacted with oxygen 100 g of phosphorous reacted with oxygen, it produced 17.77 g of a phosphorous oxide. This new compound was found to have a formula mass of approximately 220 g/mole. Find the molecular formula,
A 0.500-g sample of chromium metal reacted with sulfur powder to give 0.963 g of product. a) The mass of sulfur that reacted is _____ b) The empirical formula of the chromium sulfide is _____