A Moving to another question will save this response. Question 26 SHOW WORK Given the following reaction: CaC 2(s) + 2H 20 -C2H 2(g) + Ca(OH) 2(aq) Assume that you place 1.85 g of calcium carbide in excess water and collect the acetylene gas over water. Calculate the maximum amount of gas that should be produced in grams round answer to 3 decimal places omit trailing zeroes The actual volume of acetylene and water vapor collected is 810 ml at 30.5°C with a pressure of 557.524 mmHg. Calculate the actual amount of gas collected(in grams) round answer to 3 decimal places omit trailing zeroes The vapor pressure of water at 30.5°C is 32.35 mmHg. Calculate the percent yield of acetylene. round answer to 2 decimal places omit trailing zeros A Moving to another question will save this response.

A Moving to another question will save this response. Question 26 SHOW WORK Given the following reaction: CaC 2(s) + 2H 20 -C2H 2(g) + Ca(OH) 2(aq) Assume that you place 1.85 g of calcium carbide in excess water and collect the acetylene gas over water. Calculate the maximum amount of gas that should be produced in grams round answer to 3 decimal places omit trailing zeroes The actual volume of acetylene and water vapor collected is 810 ml at 30.5°C with a pressure of 557.524 mmHg. Calculate the actual amount of gas collected(in grams) round answer to 3 decimal places omit trailing zeroes The vapor pressure of water at 30.5°C is 32.35 mmHg. Calculate the percent yield of acetylene. round answer to 2 decimal places omit trailing zeros A Moving to another question will save this response.

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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The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2Al(OH)3(s) + Al2O3(s) -> 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s) + 3C(s) + 4Al(s) -> 3CO2(g) Suppose the yield of the first step is 74.% and the yield of the second step is 76.% . Calculate the mass of aluminum hydroxide required to make 4.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .
Cryolite (Na3AlF6) is used in the commercial production of aluminum from ore. Cryolite itself is produced by the following reaction: 6 NaOH + Al₂O3 + 12 HF → 2 Na3AlF6 + 9 H₂O A mixture containing 420.0 kg of NaOH, 228.4 kg of Al2O3, and 600.0 kg of HF is heated to 950 °C until it reacts to completion. What is the maximum mass of Na3AlF6 formed? kg Na3AlF6
Answer With Work Shown Please . 1. CaO + H2O → Ca(OH)2 If you start with 2400 g of CaO, add excess water, and produce 2060 g of Ca(OH)2, what is the percent yield of the reaction? 2.Draw the Lewis dot structure of SiCl4 then determine if the molecule has polar bonds and if it is a polar or non-polar molecule. 3.If you have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 870C, how many moles of gas do I have? R=0.0821 L*atm/K*mol
The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H12O6 +60₂-6CO₂ + 6H₂O The products of the reaction are carbon dioxide (CO₂) and water (H₂O). Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500. mL of air, which is typically enriched to 4% CO₂ and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 1.00 kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO₂ is 2.0 kg/m³. 0 ☐ ☐x10 X
Silicon tetrachloride (SiCl4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2Cl2(g) -> SiCl4(l) In one reaction, 0.507 mole of SiCl4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SiCl4 = 169.9 g/mol; MW Cl = 35.453 g/mol 63 grams 27 grams 72 grams 36 grams
A materials scientist has created an alloy containing aluminum, copper, and zinc, and wants to determine the percent composition of the alloy. The scientist takes a 12.849 g sample of the alloy and reacts it with concentrated HCl. The reaction converts all of the aluminum and zinc in the alloy to aluminum chloride and zinc chloride in addition to producing hydrogen gas. The copper does not react with the HCl. Upon completion of the reaction, a total of 10.4 L of hydrogen gas was collected at a pressure of 724 torr and a temperature of 27.0 °C. Additionally, 2.836 g of unreacted copper is recovered. Calculate the mass of hydrogen gas formed from the reaction. mass: ----- g Calculate the mass of aluminum in the alloy sample. mass: ---- g What is the mass percent composition of the alloy? Cu: -----% Zn: ----% Al: -----%
Consider the following chemical reactions: KClO3 (s) ----------> KCl(s) + O2(g) NaNO3(s) ---------> NaNO2(s) + O2(g) 5.0000 g mixture of potassium chlorate and sodium nitrate is decomposed and the mass of residuals is 3.8600 g. The oxygen gas is collected in 359. mL. container at 25 oC by water displacement technique. Calculate the total pressure in mmHg. the vapor pressure of H2O at 25oC is 18.3 mmHg. K = 39.10 g/mole, Cl = 35.45 g/mole, Na = 22.99 g/mole, N = 14.00 g/mole and O = 16.00 g/mole
A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas city (MCI) to Baltimore (BWI) burned 11800 lb. of Jet A fuel. Jet A fuel is kerosene based, consisting primarily of CnH2n+2 hydrocarbons, with n = 6 to 16, so the Carbon:Hydrogen ratio is close to 1:2. During this flight , how much CO2 (in kg) was released into the atmosphere? (assume the combustion of fuel was complete, so all fuel was converted into H2O and CO2).
Cryolite (Na3AlF6) is used in the commercial production of aluminum from ore. Cryolite itself is produced by the following reaction: 6 NaOH + Al2O3 + 12 HF → 2 Na3AlF6 + 9 H2O A mixture containing 420.0 kg of NaOH, 128.4 kg of Al2O3, and 600.0 kg of HF is heated to 950 °C until it reacts to completion. What is the maximum mass of Na3AlF6 formed? ________kg Na3AlF6
4. A common experiment at Science Fairs is the demonstration of a volcano using a mixture of baking soda, NaHCO3(s), and vinegar, CH₂COOH(aq), with the reaction: NaHCO3(s) + CH3COOH(aq)- CO2(g) + H₂O(l) + Nat(aq) + CH3COO(aq) where the heavier CO2 gas displaces the liquid mixture to the top of the container to simulate lava overflowing. If the volume of the reaction vessel is 0.500 L and the pressure is 0.997 atm and 298 K. given 50.5 ml of 0.351 M CH3COOH() in water, what mass of NaHCO3(s) is required to fill the bottle with CO2 gas?
Calcium hydride reacts with water to produce hydrogen gas according to the following reaction: CaH2(s) + 2 H2O(l) ----> 2H2(g) + Ca(OH)2(aq) This reaction is used to generate hydrogen gas to inflate air bags in cars and life rafts on boats and for similar uses where a simple compact means of hydrogen generation is necessary. Assuming complete reaction with water, how many grams of calcium hydride are required to fill a raft to a total pressure of 2.0 atm at 25oC if the volume of the raft is 1,000 L?