6. Methanol (CH3OH, also called methyl alcohol) is the simplest alcohol. It is used as a fuel in race cars and is a potential replacement for gasoline. Methanol can be manufactured by combination of gaseous carbon monoxide and hydrogen. Write the balanced equation for methanol production: Suppose 68.5 kg of CO(g) are reacted with 8.60 kg H2(g). Calculate the theoretical yield of methanol. If 3.57 x 104 g of CH3OH are actually produced, what is the percent yield of methanol? actual yield Percent yield = X 100% %3D Theoretical Yield

6. Methanol (CH3OH, also called methyl alcohol) is the simplest alcohol. It is used as a fuel in race cars and is a potential replacement for gasoline. Methanol can be manufactured by combination of gaseous carbon monoxide and hydrogen. Write the balanced equation for methanol production: Suppose 68.5 kg of CO(g) are reacted with 8.60 kg H2(g). Calculate the theoretical yield of methanol. If 3.57 x 104 g of CH3OH are actually produced, what is the percent yield of methanol? actual yield Percent yield = X 100% %3D Theoretical Yield

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...

See similar textbooks

Similar questions

14. A substance is found by analysis to contain 45.57% tin and 54.43% chlorine. What is the empirical formula for the substance? 15. Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. a) Write a balanced equation for this reaction. b) How many grams of aluminum hydroxide can be obtained from 5.50 g of aluminum sulfide? 16. When copper (1) sulfide is partially roasted in air (reaction with 02), copper(1) sulfite is formed first. Subsequently, upon heating, the copper sulfite thermally decomposes to copper (1) oxide and sulfur dioxide. Write balanced chemical reactions for these two reactions. 17. Write the molecular, complete ionic & net ionic equation for a single replacement (redox) reaction between zinc and copper (ii)sulfate? Identify the oxidized and the reduced species. 18. How many grams of Mg(OH)2 will be needed to neutralize 25 ml of stomach acid if stomach acid is 0.10M HCI? 19. How many litres of 3.4 M HI will be required to reach the…
Consider the following unbalanced chemical reaction: Al (s) + HCI (g) → AICI3 (g) + H2 (g) 1. Balance the chemical equation 2. How many moles of aluminum metal are needed to produce 3.33 moles of aluminum chloride? 3. Calculate the mass of aluminum metal (g) needed to produce 3.33 moles of aluminum chloride.
magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. When 10.1 g of Mg reacts with 10.5 g of O2, 11.9 g of MgO are collected. What is the balanced equation for this reaction, including all states of matter?
The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 1.2 g of potassium chloride. For your convenience, the molar mass of each substance Is shown below their formulas (in purple). Use this Information to make the requested calculation: 2 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 2900 mg of potassium chlorate:
What is the mass in grams of phosphorus trichloride that can be formed from 232.6 grams of chlorine gas based on the balanced chemical equation? balanced chemical equation: P4(s) + 6 Cl2(g)-> 4PCl2(g)
peact Baking soda is often included in recipes to make food rise. When heated, it will produce sodium carbonate, water vapor, and carbon dioxide. Which of the five types of chemical reactions does the equation represent? Provide evidence and reasoning
For the following reaction: C3Hg(g) + O2(g) ————> CO2(g) + H2O(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams for each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams
Consider the reaction: C2H4 + O2 → CO) (Unbalanced). If 0.96 g of C2H4 g was Used 5.2 g of CO2 produced, calculate the percentage yield in the reaction. (Hint Balance the equation first).
What mass of CO2 (in Kg) does the combustion of a 12-gallon tank of gasoline release into the atmosphere? Assume the gasoline is pure octane (C8H18) and that it has density of 0.70 g/mL. You will need a balanced chemical equation for combustion of octane.
Consider the reaction of solid P, and chlorine gas to form gaseous phosphorus trichloride. a) Write the balanced chemical equation for the reaction. b) The balanced chemical equation is P,(s) + 6 CI,(g) → 4 PCI,(g). What is the mass in grams of phosphorus trichloride that can be formed from 222.3 grams of P, based on the balanced chemical equation? c) The balanced chemical equation is P,(s) + 6 CI,(g) → 4 PCI,(g). What is the mass in grams of phosphorus trichloride that can be formed from 304.8 grams of chlorine gas based on the balanced chemical equation? 28 d) Given that 222.3 grams of P, react to make 985.6 g of PCI, and 304.8 g of CI, react to make 393.5 g of PCI, which reactant is limiting? e) The theoretical yield for the reaction is 393.5 g of PCI,. If only 218.7 g of phosphorus trichloride were collected, what is the percent yield of the reaction?
The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 5.4 kgkg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)
Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P,(s) + 50,(g) 2 P,0; (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H,PO,): P,0;(g) + 3H,0(1) 2 H;PO, (1) Suppose the yield of the first step is 77.% and the yield of the second step is 67.%. Calculate the mass of phosphorus required to make 6.0 kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.