"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 75 L tank with 18. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.0 mol of carbon monoxide gas, 12. mol of water vapor and 12. mol of carbon dioxide. A The engineer then adds another 9.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. Answer Submitted: mol

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 75 L tank with 18. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.0 mol of carbon monoxide gas, 12. mol of water vapor and 12. mol of carbon dioxide. A The engineer then adds another 9.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. Answer Submitted: mol

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

Hydrogen peroxide decomposes as shown below: 2 H2O2 → 2 H2O + O2 molar mass H2O2 = (34.0 g/mol) A sample of hydrogen peroxide solution was analyzed using the procedure from the “Enzymatic Decomposition and Analysis of Hydrogen Peroxide” experiment. A 5.89 g sample of the solution generated 0.0237 mol of oxygen gas. Calculate the grams of H2O2 in the solution.
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: -----%
Give Up? O Resources 9.4% re: Hint 8 > Consider these reactions, where M represents a generic metal. 2 M(s) + 6 HC1(aq) → 2 MCl,(aq) + 3 H, (g) 1. AĦ, = –783.0 kJ HCI(g) HCl(aq) → AH2 = –74.8 kJ H,(g) + Cl, (g) → 2 HCl(g) AH3 = –1845.0 kJ MCI, (s) → MCl, (aq) 4. AH -124.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl,(g) → 2 MCl, (s) S. AH kJ about us privacy policy terme of use contact.ua help en 2. 3.
Consider the reaction below LiOH+KCL LiCL+KOH If 20.0 grams of lithium hydroxide LiOH are used, what is the theoretical yield of lithium chloride LiCL?
In the picture shown, the limited reactant is ____. The excesss reactant is ____. The product of the reaction is ___.
Given the reaction CH 4 + 2O 2 ----------> 2H 2O + CO 2 which statement is FALSE? 16 g O2 reacts to form 18 g H2O 16 g CH4 combines with 64 g O2 1 mol CO2 is formed from 2 mol O2 1 mol CH4 reacts to form 2 mol H2O 18 g H2O is produced from 1 mol O2
Remalning Time: 1 hour, 28 minutes, 18 seconds. * Question Completion Status: QUESTION 4 For the following question(s), consider the following balanced equation. Mg 3N 2( S) + 6H 20(1) → 3Mg(OH) 2( s) + 2NH 3( g) When 2.50 mol of Mg 3N 2 are allowed to react, how many moles of H 20 also react? [SHOW YOUR WORK FOR THIS PROBLEM] 15.0 mol 2.50 mol O 9.00 mol O 6.00 mol O 1.25 mol QUESTION 5 Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save All Ar Type here to search 28
15. Citric acid, C6H807 (aq), is often used as an additive to make candies "sour. a. Draw a flowchart that shows how to caloulate the molar mass of citric acid, b. Verify the steps in your flowchart by calculating the molar mass of citric acid.
A chemist uses carbon, CaO, HCl and H₂O for C₆H₄Cl₂ (147.09 g mol⁻¹). Assuming that the efficiency of the reaction is 68% and some C₆H₄Cl₂ and 3 moles of CO are formed from the initial total carbon, how many grams of C₆H₄Cl₂ are obtained from 500 g of carbon?
Consider the following reaction: 2 NH, (9) + 3 Cl, (9) A mixture is prepared from 15.0 mol of ammonia and 15.0 mol of chlorine gas. Determine the total moles of N, (g) + 6 HCI (g) gas in the container after the reaction has gone to completion.
11a, 11c and 12c
Titanium is a strong, lightweight, corrosion-resistant metal that is used in rockets, aircraft, jet, engines, and bicycle frames. It is prepared by the reaction of Titanium (IV) chloride with molten magnesium between 950 °C and 1150 °C. TiCl4(g) + 2Mg(1) → Ti(s) + 2MgCl2(1) In a certain industrial operation 3.54 x 107 g of TiCl4 are reacted with 1.13 x 107 g of Mg. (i) What is the theoretical yield of Ti in grams? (ii) what is the percent yield if 7.91 x 106 g of Ti are obtained?