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- C6H5Cl + 2 NH3 --> C6H5NH2 + NH4Cl Assume that 20.0 g of chlorobenzene at90% purity is mixed with 8.30 g of ammonia. a)What is the limiting reactant?For the reaction C4H10 + O2 --> CO2 + H2O a) what weight of C4H10 in grams is needed for 3.01 x 10E23 particles of O2? b) how many moles of CO2 will be produced from 5.0 moles of C4H10? c) what weight in grams of H2O will be produced from 12.5 ml of C4H10? density (p)?of C4H10 = 0.506 g/mLMethane is produced in the human gut during digestion. As it passes through the digestive tract, it collects at thelower end and is emitted as flatulence. About 10% of a fart is composed of methane.__CH4 + __O2 → __ CO2 + __H2Oa) The average human fart contains 0.00643g of methane gas. Ifyou were to light said fart (and you SHOULD NOT), what mass ofoxygen would combust along with it?b) People, on average, pass 0.75L of gas per day. This is about0.0536g of methane per 24 hour period (remember, only ~10% ismethane). What mass of water could be generated by one personigniting their “methane emission”? c) How many water molecules is this? (SHOW ALL WORK IN TRAIN TRACKS)
- Consider a blend of mass 5g formed from 2.2 g of C12H24 and 2.8g of C998H1000 paraffin's:, What are Mn and Mw of the blend?A mixture weighing 28.516g containers 4.518g NH4CL, 15.20g SiO2, with the remainder NaCl. find the percent, weight, of each component. Show you method for making the calculations.Acetic acid (CH3COOH) can be produced based on the reaction: CH3COOC2H5+ H2O ⟶CH3COOH + C2H5OH. If there are 344.5 g of CH3COOC2H5 and 165.8 g of H2O a. How many moles of acetic acid will be produced? b. Calculate the percent yield if 125 g of acetic acid was produced (express your answer in 1 decimal place only).
- a hydrated CuSO4 salt was heated and thus dehydrated. Determine the % H2O by weight in the hydrated CuSO4 salt. SHOW WORK TO RECEIVE FULL CREDIT mass of empty dish 43.571 gmass of dish + hydrated salt 44.326 gmass of dish + dehydrated salt 44.054 g 4. Using the data found in question number 3, determine the empirical formula for the hydrated CuSO4salt. What is the chemical name of this dehydrated salt? 5. Suppose that after your second heating, you were impatient and did not wait until your porcelain evaporating dish to cool. Instead, you weighed it while it was still hot. How would this specifically affect the calculated percentage of water in the compound?The following is the balanced equation for the combustion of butanol in oxygen:C4H9OH(g) + 6O2 --> 4 NO(g) + 6H2O(g) a. How many grams of butanol must be burned to produce 18.50g of carbon dioxide? b. How many grams of water are also produced? c. How many grams of oxygen are needed to produce 18.50g of carbon dioxide? d. Use the results from a, b and c to show this reaction obeys the law of conservation of mass.Given the following reactions: Fe(s) + Br2(g) \rightarrow→ FeBr2(s) 3 FeBr2(s)+ Br2(g) \rightarrow→ Fe3Br8(s) If each reaction gives an 82.0 % yield, what mass (in grams) of Fe3Br8 is produced from 1.00 g of Fe, assuming Br2 is in excess? Enter the numerical value (no units) using 3 significant figures.
- Use dimensional analysis: A) Write a balanced combustion reaction for C6H10. B) If 45.0 g of C6H10 react with 156 g of oxygen, how many grams for carbon dioxide should be made? C) What is the limiting reagent? D) How many grams of excess reagent is used and how many grams remain? E) A student made 102 g of carbon dioxide what is her % yield?The ratio by mass of carbon to hydrogen in 100 g of a certain compound is 6 to 1. What will be the ratio in 200 g of the same compound? (Show Work)How many moles of cacl2 and 2H2O are present in 1.5 g of cacl2 and 2h2o? Also how many moles of pure cac1 to a present and the 1.50 g of cacl2 and 2H2O