If an automobile travels 225 mi with a gas mileage of 20.5mi / gal,how many kilograms of CO{2} are produced? As- sume that the gasoline is composed of octane, C8H18(l) whose density is 0.69g / mL (b) Repeat the calculation for a truck that has a gas mileage of 5mi /gal

Aspirin can be prepared from salicylic acid (C7H6O3), which has a molar mass of 138.12 g/mol, and acetic anhydride (C4H6O3), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C7H6O3+C4H6O3⟶C9H8O4+C2H4O2 What is the yield, in grams, of aspirin (C9H8O4), which has a molar mass of 180.15 g/mol, possible when reacting 2.18 g of salicylic acid with 1.05 mL of acetic anhydride?

10 Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10º kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH,CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 22.0 atm of ethane gas and raises the temperature to 500. °C. She believes K =0.050 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K , and the mass percent of ethylene you calculate may not be what she actually observes. %

A 19.51 g sample of impure methylamine, which contains 72.58% (by mass) of CH;NH: , is reacted with 30.81 g of pure oxygen gas: 2.1 4CH, NH,(2) + 90,(8) - 4C0,(8) + 10H,0(?) + 2N;(8) 2.1.1 What is the percentage yield of this reaction if 5.54 g of nitrogen gas is collected? 2.1.2 In another experiment, this impure methylamine was used as follows: • An unknown mass of the impure compound is dissolved in enough water to make 500.0 m of solution. • 20 ml of this solution was transferred by pipette to a clean 250 ml volumetric flask and made up to the mark. • The molarity of the CH;NH; in the final solution was determined to be 0.103 M. Determine the mass of CH;NH; present in the original amount of impure compound used make this solution.

A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula

In a car airbag, sodium azide (NaN3) decomposes to form sodium metal and nitrogen gas (reaction1). The sodium metal then reacts with potassium nitrate to produce more nitrogen gas (reaction 2) according to the following equation: Na(s) + KNO3(s) → N2(g) + Na2O(s) + K2O(s) a) Write the balanced chemical equation for the reaction (1) that happened in the airbag. b) Balance the equation of reaction 2 c) In a table classify and compounds in ion 1 and reaction 2 into ionic or covalent. If 2.00 mol of sodium azide react in this way, what is the total number of molecules of N2 will be formed? (The Avogadro constant = 6.022 x 1023 molecules/mol1) (show all your calculations, units and significant figures are important)

Aspirin can be prepared from salicylic acid (C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride (C4 H6 O3), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C;H,O3 + C4H6O3 → C9HgO4 + C2H3O2 What is the theoretical yield, in grams, of aspirin (C9H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.06 g of salicylic acid with 3.71 mL of acetic anhydride? Type answer:

The metal widely used in our civilization is iron (Fe) and it is obtained industrially by the reduction of iron oxide (Fe,0,) with carbon at higher temperatures (over 1000 °C). The equation for the reaction is as follows, Fe,0;(s) + C(s) –Fe(s) + CO2(g) Using the above equation, a. What is the number of moles of Fe? (ensure 3 decimal places for e.g. 0.300) mols b. How much of the product (Fe) can be produced from 10.0g of Fe,O;?(ensure 2 decimal places for e.g. 0.30) c. What is the number of moles for carbon?(ensure only 4 decimal places) (ensure 4 decimal places for e.g. 0.3003) mols bo

Calculate percent yield

LiOH(s) + CO2(g) - Li2CO3(s) + H2O(g) lithium hydroxide canister contains 155 g of LiOH(s). What mass of CO2(g) will the canister be able to absorb? If it is found that after 24 hours of use the canister has absorbed 102 g of carbon dioxide, what percentage of its capacity has been reached?