2.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 192. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass 3.44 g carbon dioxide 0.94 g water Use this information to find the molecular formula of X. Check Privecy Explanation Terms of Use 2019 McGraw-Hill Education. All Rights Reserved. 2:06 PM 12/5/2019 99+ O Type here to search hp end home ins prt sc delete 12 f11 f10 fg f8 144 f6 10 esc num lock backspace &

2.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 192. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass 3.44 g carbon dioxide 0.94 g water Use this information to find the molecular formula of X. Check Privecy Explanation Terms of Use 2019 McGraw-Hill Education. All Rights Reserved. 2:06 PM 12/5/2019 99+ O Type here to search hp end home ins prt sc delete 12 f11 f10 fg f8 144 f6 10 esc num lock backspace &

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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 0.235 mL sample of carbon tetrachloride (density = 1.59 g/mL, MM = 153.81 g/mol) contains how many AMU of Cl? Note: Use 6.022 x 1023 and/or 1.661 x 10-24 as appropriate. 5.18 x 1022 2.42 x 10-3 2.07 x 1020 1.30 x 1022 2.07 x 1023 0.333 g of a hydrocarbon (CxHy) was analyzed by combustion analysis and 1.009 g of CO2 (MM = 44.01 g/mol) and 0.516 g of H2O (MM = 18.02 g/mol). Which of the following is the correct empirical formula of the hydrocarbon? C2H4 C2H5 C3H7 C2H3 CH3
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?
At elevated temperature NaHCO3 is quantitatively converted to Na2CO3. By calcining 0.3592 g of an antacid tablet containing NaHCO3, 0.2362 g of Na2CO3 was obtained. Calculate the percentage purity of the tablet (such as % w/w NaHCO3) It would be appreciated if you could write each step to the answer.
A hydrate [hydrates have the general formula AB • xH2O] is found to have the percentcomposition: Na = 19.17%, C = 10.00%, H = 4.17% and O = 66.6%. After heating to 100 oC todrive off the water of hydration, the percent composition is found to be: Na = 27.38%,C = 14.28%, H = 1.19% and O = 57.15%. From this data, determine the probable molecularformula for the hydrate if the molecular weight = 120 amu.
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?
points A 0.1938 g of an organic compound known to contain C and H only was burned. The traps for H2O and CO₂ increased in mass by 0.2750 g and 0.5972 g. respectively. What is the percentage of carbon?
the molecular formula of hydrocarbon is to be determined by analyzing its combustion products. a) the hydrocarbon burns completely, producing 7.2 g of water and 7.2 liters of CO2 at standard conditions. What is the empirical formula of the hydrocarbon? b) Calculate the mass in grams of O2 required for the complete combustion of the sample of the hydrocarbon described in a. c) the molecular weight of the hydrocarbon is determined to be 56.1 amu. What is the molecular formula of the hydrocarbon?
General formula of a polymer is-(CH2CHCHCN)n-, where n is typically greater than 10,000. Then take a sample of this polymer weighs 755.9 g and contains 3.112 x 1020 molecules of -(CH2CHCHCN)n-, so calculate n?
Orciprenaline(C11H17N03,211.258 g/mol) is a bronchodilatorused in the treatment of asthma.The BP assay for orciprenalinetablets is described below. Read thefollowing information carefully andanswer the questions below.(Record your answers in decimalnotation to the indicated significantfigures OR decimal places)ASSAY - 20 tablets weighing 2.597 gwere crushed to a powder. Aportion of the crushed powder(0.5456 g) was shaken with 50 mL of0.1 M HI, the mixture was filteredand made up to 100 mL. 10 mL ofthis solution was further diluted to100 mL with 0.1 M HCI. Themeasured absorbance of thediluted solution at 276 nm was0.582. Additional information: A1%72.3, stated content = 20 mg Calculate:a) The concentration oforciprenaline in the diluted solutionin mg/L b) The actual amount oforciprenaline (in mg) in the powderassayed.c) The actual amount oforciprenaline (in mg) per tablet.d) The percentage of stated contentof per tablet.
1. Balance the following equations:a) ____ Na2SO4(aq) + ____ Pb(C2H3O2)2(aq) → ____ NaC2H3O2(aq) + ____ PbSO4(s) i. How many moles of Pb(C2H3O2)2 are required to react with 1.67 moles Na2SO4? Use dimensional analysis.
In 1997, at the United Nations Conference on Climate Change, the major industrial nations agreed to expand their re-search efforts to develop renewable sources of carbon-basedfuels. For more than a decade, Brazil has been engaged in aprogram to replace gasoline with ethanol derived from the rootcrop manioc (cassava).(a) Write separate balanced equations for the complete combus-tion of ethanol (C₂H₅OH) and of gasoline (represented by theformula C₈H₁₈).(b) What mass of oxygen is required to burn completely 1.00 Lof a mixture that is 90.0% gasoline (d=0.742 g/mL) and 10.0%ethanol (d=0.789 g/mL) by volume?(c) If 1.00 mol of O₂ occupies 22.4 L, what volume of O₂ isneeded to burn 1.00 L of the mixture?(d) Air is 20.9% O₂ by volume. What volume of air is needed toburn 1.00 L of the mixture?