5. Using the chemical equation: COg) + 2 H2(g) → CH3OH)a. Starting with 12.5 g H2 and 74.1 g CO, which is limiting reactant?b. What mass of methanol can be obtained (in theory)?c. What mass of the excess reactant is left over?

Answered: Image /qna-images/answer/fcf653f8-50fa-4125-ae28-2fa21825dbe6.jpg

Answered: 5. Using the chemical equation: CO(9) +…

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

Aluminum chloride is made from scrap aluminum through the following balanced reaction. 2 Al (s) + 3 Cl2 (g) --> 2 AlCl3 (s) a. If you begin with 19.7 moles of aluminum and 9.88 grams of chlorine, how much aluminum trichloride is produced? b. What is the mass of excess reagent?
22. The combustion of hexane (C,H14), a component of gasoline, is represented by the balanced chemical equation: 2 C6H14() + 19 O2(g) ® 12 CO2(g) + 14 H20(g). If 1.0 mole of hexane undergoes moles of O2 are required. combustion, a. 19 moles b. 7 moles C. 9.5 moles d. 26 moles e. 21 moles a O b O c e
10. Balance the equation for the combustion of butane, C,H,. C.H10 + O, > со, + H2O a. If 31.4 grams of butane burn according to this reaction, how many grams of oxygen would you need to ensure all the butane burned? (112 g O,)
2. Given: 1 P₁ +50₂ → 1 P40₁0 10 4 calculate a. The mass (in u) of P4 required to produce 2.66 x 10 23 molecules of product. b. The number of O₂ molecules required to react completely with 3.00 g P₁.
1. A mixture of hydrazine (N2H4) and hydrogen peroxide (producing nitrogen and water) is used as a fuel for rocket engines. A. Write the valid chemical equation. B. What mass of N2H4, in grams, is needed to react completely with 35.0 g of H2O2? When, H= 1.01g. O=16.00g. N=14.01g.
If a reaction is run that is supposed to produce 125 g (theoretical yield) of product and the actual yield of product that was produced was 73.5 g, what is the percent of yield of this reaction? A. 170% B. 1.70% C. 73.5% D. 58.8%
Glucose (CeH12O6) can be fermented to yield ethanol (C2H5OH) and carbon dioxide (CO2). a. What is the theoretical yield of ethanol (in grams) produced with a 72% yield2 and actual yield of 43.5 g? b. What is the mass of glucose (in grams) in the fermentation reaction? C6H1206 → 2 C2HSOH + 2 cO2 Molar mass of CGH1206 = 180.156 g/mol Molar mass of C2HSOH = 46.07 g/mol Molar mass of CO2 = 44.01 g/mol
Consider the generic chemical equation: 2 A + 4 B --------> 3 C 1. If 10.0 moles of each reactant were used to complete that reaction, which of the following is true. a. A is the limiting reactant and 15.0 moles of C will be produced. b. A is the limiting reactant and 20.0 moles of C will be produced. c. B is the limiting reactant and 7.50 moles of C will be produced. d. B is the limiting reactant and 22.5 moles of C will be produced. 2. What is the percent yield of this reaction if 6.40 moles of C were actually produced?
Iron oxide reacts with carbon to produce elemental iron and carbon monoxide according the the equation shown below. Consider the reaction of 51.4 grams of Fe2O3 with 24.98 grams of C to produce 19.20 grams of Fe. Fe2O3(s)+3c(s)-------2Fe(s)+3CO(g) a. actual yield b. theoretical yield c. percent yield
3 Fe(s)+2 O 2 (g) —> Fe 3 O 4 (s) When 14.5 g Fe and 11.2 g of O 2 are mixed.. How much of excess reactant is left over?
#11 please
3. Given: NaCl 1 NiCl₂ + 2 NaOH → 1 Ni(OH)₂ + 2 A student combines 2.44 g of NiCl₂ with 6.44 g NaOH. Determine a. The limiting reactant. b. The mass of the excess reactant that remains at the end of the reaction. c. The number of NaCl molecules that are formed if the reaction is 51% efficient.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

5. Using the chemical equation: CO(9) + 2 H2(g) → CH3OH) a. Starting with 12.5 g H2 and 74.1 g CO, which is limiting reactant? b. What mass of methanol can be obtained (in theory)? c. What mass of the excess reactant is left over?