Sofia8.50g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 136. g/mol, is burnedcompletely in excess oxygen, and the mass of the products carefully measured:productmasscarbon dioxide22.01 g4.50 gwaterdoUse this information to find the molecular formula of X.ArPrivcyTerms of LaeCheck2019 McGraw-Hill Education All Rights Reserved7:09 PM12/4/2019Explanation99+O Type here to searchhpandC ిprt schofe 144f8f7f6 1015lockbackspacef4&8.eschome00%24

X react with oxygen to give CO2 and H2O. So the number of moles of carbon in CO2 and number of…

Answered: Sofia 8.50 g of a certain Compound X,…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 25QAP: Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and...

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Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a density of 1.71 g/L. (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of 85.7% C and 14.3% H. What is the molecular formula of cyclopropane?
An herbicide is found to contain only C, H, N, and Cl.The complete combustion of a 100.0-mg sample of theherbicide in excess oxygen produces 83.16 mL of CO2 and73.30 mL of H2O vapor expressed at STP. A separate analysisshows that the sample also contains 16.44 mg of Cl.(a) Determine the percentage of the composition of thesubstance. (b) Calculate its empirical formula. (c) Whatother information would you need to know about thiscompound to calculate its true molecular formula?
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?
For every one molecule of NaHCO3(s) there is one molecule of CO2(g) that forms: NaHCO3(s) + CH3CO2H(aq) --> CO2(g) + H2O(l) + NaCH3CO2(aq) This means that if we know how many moles of gas we need, we need the same number of moles of sodium bicarbonate to produce it. Now, we need something to fill with gas. I'll be filling a 1-quart sealable plastic bag. 1 quart is 946 mL (0.946 L). We can use the ideal gas law to determine how much gas (in moles) is needed to fill 946 mL. Remember there are four variables for the ideal gas law. Ideal Gas Law: PV = nRT P = pressure: typically 715 mm Hg in Spokane <-- unit dictates which R to use V = volume: 1 quart bag = 0.946 L <-- must be in Liters T = room temperature: 20 °C in my lab, +273 = 293 K <-- must be Kelvin n = moles: what we are solving for I used atmospheric pressure in mm Hg, so I'll have to pick the R value with "mm Hg" in the units: R = 62.4 L × m m H g K × m o l Now, use these values to calculate how many moles of…
The manufacture of aluminum includes the production of cryolite (Na3AlF6) from the following reaction: 6〖HF〗_((g))+3〖NaAlO〗_(2(s))→ 〖Na〗_3 〖AlF〗_(6(s))+3H_2 O_((l))+ 〖Al〗_2 O_(3(s)) How much HF (hydrogen sulfide) is required to produce 2.50kg of Na3AlF6? How many cm3 of HF(g) are needed to produce 26.0g of Na3AlF6? The density of HF (g) at 25is 1.15g/L.
The most important commercial process for converting N2 from the air into nitrogen-containing compounds is based on thereaction of N2 and H2 to form ammonia 1NH32:N21g2 + 3 H21g2¡2 NH31g2How many moles of NH3 can be formed from 3.0 mol of N2 and 6.0 mol of H2?
Sulfuric acid, H2SO4, can be formed from the chemical reaction 2SO2+O2+H2O--->2H2SO4. Suppose 400g of SO2; 175g of O2, and 125 g H2O are mixed and the reaction proceeds until one of the reactants is used up. How many grams of H2SO4 is produced?A. 612gB. 620gC. 622gD. 630g
Methane 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)
Adipic acid, H2C6H8O4, is used to produce nylon. It is made commercially by a controlled reaction between cyclohexane ( C6H12 ) and O2:. (Only the 4th sub part (d) is needed to be answered). 2 C6H12 (l) + 5 O2 (g) → 2 H2C6H8O4 (l) + 2 H2O (g) (Given: Atomic Wts (g/mol): C= 12.01 ; H=1.01 ; O=16.00 ) If 25.0 g of cyclohexane is reacted with 20.0 g of O2, a. Identify the limiting reactant and excess reactant? b. How much in grams of the excess reactant will be left after the reaction? c. What is the theoretical yield in terms of the product adipic acid? d. If the actual yield is 33.5 g, what is the % yield of adipic acid?
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?
Equimolar amounts of H2(g) and Br2(g) are injected into an evacuated, rigid container, where they react according to the equation below. H2(g)+Br2(g)⇄2HBr(g) ΔHorxn =−72.4 kJ/molrxn (a) If 1.6 g of Br2 is consumed in the reaction with excess H2, how many moles of HBr are produced? BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit) Edit imageView imageDelete image .02 Mol HBr 3 / 10000 Word Limit3 words written of 10000 allowed Question 2 (b) Which element is reduced in this reaction? Justify your answer in terms of the oxidation numbers. BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit) Edit imageView imageDelete image
In the reaction: As2O3 + H2O + I2 = As2O5 + HI, 300 g of As2O3 is added to 400 g of I2 and 50 g of H2O. a) Find the limiting and excess reactants.b) What are the % excess reactants?c) If 160g of As2O5 is formed, what is the degree of completion?d) Illustrate the Law of Conservation of Mass for the reaction.

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