To produce zinc metal, carbon monoxide reacts with zinc (II) oxide according to: Zno + CO - Zn + CO2 The carbon monoxide, however, is initially prepared from: 2C+ 02 200 How many grams of zinc metal (Zn) may be prepared if If 81.0g of C is used with excess amount of Zno? Your answer should be numerical and neglect units (e.g., if you calculate 3.5g then input 3.5).

To produce zinc metal, carbon monoxide reacts with zinc (II) oxide according to: Zno + CO - Zn + CO2 The carbon monoxide, however, is initially prepared from: 2C+ 02 200 How many grams of zinc metal (Zn) may be prepared if If 81.0g of C is used with excess amount of Zno? Your answer should be numerical and neglect units (e.g., if you calculate 3.5g then input 3.5).

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 is manufactured on an industrial scale by this sequence of reactions: CH, (g) + H,0 (g) CO (g)+3 H, (g) K1 CO (g) + H,0 (g)= CO, (g)+H, (g) K2 The net reaction is: CH4 (g) +2 H,0 (g) CO, (g)+4H, (g) K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and K,. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K
E-85 is an alternative fuel for automobiles and light trucks that consists of 85.0% (by volume) ethanol (C2H5OH), and 15.0% gasoline. When ethanol burns completely it produces CO2 and H2O. The balanced equation for the burning of ethanol isC2H5OH+3O2-->2CO2+3H2OThe density of ethanol is 0.790 g/mL. How many moles of carbon dioxide are produced by the complete combustion of the quantity of ethanol in 8.00 gallons of E-85 fuel? _mol CO2
For the following reaction, 3.37 grams of hydrogen gas are mixed with excess ethylene (C₂H4). The reaction yields 44.1 grams of ethane (C₂H6). hydrogen (g) + ethylene (C₂H4) (g). →→→→ethane (C₂H6) (g) What is the theoretical yield of ethane (C₂H6) ? What is the percent yield for this reaction ? Submit Answer % grams Retry Entire Group 2 more group attempts remaining
00 %24 4+ dl w/ S' Enter your answer in the provided box. Using the balanced equation for the combustion of ethanol, answer the following question. C2H,O(1) + 3 02(g) – 2 CO2(g) + 3 H,0 (g) ethanol How many grams of H,0 are formed from 1.2 mol of ethanol? OH 8 #3 5. 9. 2 4 0O
In a certain ecperiment, 50 g of sodium chloride is reacted with 75.0 g of sulfuric acid, and 52.0g of sodium sulfate is produced. Determine the percent yield for this reaction. Unbalanced equation: NaCl (s) +H2SO4(i) -> HCl(g) + Na2SO4(s)
A chemist mixes 14.10(g) of C8H18 with 72.45(g)O2 here is the balanced equation 2C8H18(g)+25O2(g)→16CO2(g)+18H2O(g) Identify the limiting reaction
I have attached an image. Thank you.
(6)For the following balanced reaction use the mass of the chemical provided to solve the mass of the chemical asked for. 6 CO2 + 6 H2O --> 1 C6H12O6 + 6 O2 202 g of CO2 is consumed by a plant undertaking this photosynthesis reaction. Find the mass of C6H12O6 produced.
Consider the combustion reaction of a hydrocarbon compound here: C2H4(g) + 302(g): 2 CO2(g) + 2 H20(g) ----> When 5.00 mol of C2H4 and 12.0 mol of O2 are added to the reactor, How many moles of CO2 can be produced by the reaction? O 4.00 mol of CO2 O 10.0 mol of CO2 O 5.00 mol of CO2 O 8.00 mol of CO2
FeSO4 + Potassium phosphate à Iron (II) phosphate + K2SO4 State the Molar Ratio of the reaction.
Each step in the following process has a yield of 60.0%. CCl₂ + 4HCI → CCL₂F₂ + 2HCl The CCI, formed in the first step is used as a reactant in the second step. If 5.00 mol CH₂ reacts, what is the total amount of HCI produced? Assume that Cl₂ and HF are present in excess. CH4 + 4Cl₂ CCl₂ + 2 HF moles HCl: 12.48 Incorrect mol
What is the minimum mass of oxygen, in grams, needed to burn 30.3 g of C3H6O? Give your answer to three significant figures. The unbalanced chemical equation is: Molar masses, in g mol-¹: H, 1.008 Number Units C3H6O + O₂ C, 12.01 CO₂ + H₂O O, 16.00