A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed through combustion analysis and yielded 2.579 g of CO, and 0.6536 g of H20. What is the compound's empirical formula? A) C2,H26O5 B) C1,H2,04 C) C4H,0 D) C13H1603 E) C3H1,O2
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- Tartaric acid contains only carbon, hydrogen, and oxygen. A 1.7323 g sample of tartaric acid was subjected to combustion analysis. 2.032 g of CO2 and 0.6240 g of H2O were collected. a) What is the empirical formula of tartaric acid? [C2H3O3] b) As a gas, tartaric acid has a density of 1.89 g/L at 0.692 bar pressure and 387 °C. What is the molecular formula of tartaric acid? [C4H6O6]The thermal decomposition of potassium chlorate can be used to produce oxygen. 2KClO3 --> 2KCl +3O2 What volume of O2 gas at 298 K and 1.0 atm pressure is produced by the decomposition of 7.50 g of KClO3 (FW=122.6)?Assume that a single cylinder of an automobile engine hasa volume of 524 cm3. (a) If the cylinder is full of air at 74 °C and 0.980 atm, how many moles of O2 are present? (Themole fraction of O2 in dry air is 0.2095.) (b) How manygrams of C8H18 could be combusted by this quantity ofO2, assuming complete combustion with formation ofCO2 and H2O?
- Natural gas consists primarily of methane, CH4(g).(a) Write a balanced chemical equation for the completecombustion of methane to produce CO2(g) as the onlycarbon-containing product. (b) Write a balanced chemicalequation for the incomplete combustion of methaneto produce CO(g) as the only carbon-containing product.(c) At 25 °C and 1.0 atm pressure, what is the minimumquantity of dry air needed to combust 1.0 L of CH4(g) completelyto CO2(g)?A 0.480-g sample of a gaseous compound occupies 367 mL at 45 °C and 365 mmHg. Which of the following is the most probable identity of the gaseous compound? Relative atomic masses:H = 1.008; C = 12.011; O = 15.999;S = 32.06; Cl = 35.45 a. SO2 b. H2O c. Cl2 d. CODinitrogen monoxide causes depletion of ozone in the in the stratosphere. Different sources of N20 have different ratios 14N and 15N. a. State one analytical technique that could be used to determine the ratio of 14N:15N b. A sample of gas was enriched to contain 2% by mass of 15N with the remainder being 14N. Calculate the relative molecular mass resulting of N2O.
- A key part of the carbon cycle is the fixation of CO2by pho-tosynthesis to produce carbohydrates and oxygen gas.(a) Using the formula (CH2O)nto represent a carbohydrate,write a balanced equation for the photosynthetic reaction.(b) If a tree fixes 48 g of CO2 per day, what volume of O2 gas measured at 1.0 atm and 78°F does the tree produce per day?(c) What volume of air (0.035 mol % CO2) at the same condi-tions contains this amount of CO2?Oxyacetylene torches rely on a precise mixture of fuel (C2H2(g)) to oxygen to optimize the welding process. _ C2H2 (g) + _ O2 (g) ---> CO2 (g) + _H2O (g) Calculate the volume (in L) of O2(g) required to react completely with 14.5 L of acetylene. Assume both substances are at SATP.Ethane (C2H6) is burned with atmospheric air, and the volumetric analysis of the dry products of combustion yields the following: 10% CO2, 1% CO, 3% O2, and 86% N2. (a) What is the complete combustion equation? (b) What is the theoretical oxygen? (c) What is the percentage of excess air? (d) What is the volume of air in liters (at 25 OC and 1 atm) per / kg fuel?
- calculate the volume of oxygen requiredfor combustion of 20cm^(3) of ethyne (2H_(2))Assume that a single cylinder of an automobile engine hasa volume of 524 cm3. (a) If the cylinder is full of air at 74 °Cand 0.980 atm, how many moles of O2 are present? (Themole fraction of O2 in dry air is 0.2095.) (b) How manygrams of C8H18 could be combusted by this quantity ofO2, assuming complete combustion with formation ofCO2 and H2O?4Fe(s)+ 3O2(g)->2FeO3 How many grams of Fe is needed to react with 9.5 L if O2 at 425K and 18.0psi?