Combustion analyses of an unknow. hydrocarbon produced the following resuits : C $2.14%. , H 13.13%,0 34.73%. deter mine the empiracle For mula.
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- Write the empirical formula for the hydrated KAl(SO4)2, based on moles of anhydrous KSI(SO4)2= 0.046 mol molar mass of H2O= 18g/ mol moles of H2O= 0.0444mol ratio pf moles H20 to moles of anhydrous KAI(SO4)2= 9.65/1 . Show all work including units. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O.Compound A reacts with Compound B to form only one product, Compound C , and it's known the usual percent yield of C in this reaction is 91.% . Suppose 8.0g of A are reacted with excess Compound B, and 8.2g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C ?Round your answer to the nearest 0.1g How much B was consumed by the reaction?A 0.157g of a compound containing C, H, N and possibly O, yields 0.213g CO2 and 0.0310g H2O upon combustion. Another sample of the same compound weighing 0.103g yields 0.023g NH3 in a nitrogen analysis. Calculate the empirical and molecular formulae given the MW= 450 +20 (Answer: C7H5O6N3; C14H10O12N6)
- For the following reactions of one mole ofreactant, predict the product, including its structuralformula and name, and state the chemical amount (inmoles) of hydrogen required for complete reaction.CH2CHCHCH2 + ___ H2(g) →C6H12O6 --> C2H5OH + CO2How many molecules of C2H5OH are produced frm 750g of C6H12O6?Paclitaxel, C47H51NO14, is an anticancer compound that isdifficult to make in the lab. One reported synthesis requires11 steps, and the final yield of paclitaxel is only 5%. Assumingall steps have equivalent yields, what is the average percentyield for each step in the synthesis?
- Please display on how to do the problem step by step: Combustion of 732 mg of an unknown organic compound gave 16.432 mg of CO2and 2.840 mg of H2O. (a) Find the wt% of C and H in the substance. (b) Find the smallest integer mole ratio of C:H in the compound.Carbon dioxide emissions associated with a one-night stay in a hotel room are calculated at 28.98 kg of CO2 per room day for an average hotel. The 250 rooms of your hotel are all occupied for two days during a college football game. How much CO2 did the guests and hotel release into the atmosphere? Round your answer to the nearest whole number. kgsThe density I found is 11.52g. What is the mmol of cyclohexanol? What is the theoretical yield of cyclohexene?
- If the empirical formula of a compound is found to be CH2, which of the following value is a plausible molecular mass for the compound? The answer is 70.15. How did you get that?Combustion of a compound containing just C, H, N, and O showed that it contains 46.21 wt% C, 9.02 wt% H, 13.74 wt% N, and, by difference, 100 - 46.21 - 9.02 - 13.74 = 31.03 wt% O. That is, 100 g of unknown contain 46.21 g of C, 9.02 g of H, and so on. Find the atomic ratio C:H:N:O. Divide each stoichiometry coefficient by the smallest one and express the composition in the lowest reasonable integer ratio (CxHyNzOw, where x, y, z, and w are integers and one of them is 1).find the limiting reagent the number of N2O4 molecule formed is _______, andthe number of ______ molecule in excess is_______