C What mass of O2, in grams, is required for complete combustion of 39.0 g of methane? Mass = 155.52 Correct 1. Convert the mass of CH4 to amount of CH4. 2. Use the stoichiometric factor to calculate the amount of O2 required. 3. Calculate the mass from amount. 2 mol O2 32.00 g 1 mol CH4 16.04 g 39.0 g CH4 x = 156 g O2 1 mol CH4 1 mol O2 dWhat is the total mass of products expected from the combustion of 39.0 g of methane? Total mass =

C What mass of O2, in grams, is required for complete combustion of 39.0 g of methane? Mass = 155.52 Correct 1. Convert the mass of CH4 to amount of CH4. 2. Use the stoichiometric factor to calculate the amount of O2 required. 3. Calculate the mass from amount. 2 mol O2 32.00 g 1 mol CH4 16.04 g 39.0 g CH4 x = 156 g O2 1 mol CH4 1 mol O2 dWhat is the total mass of products expected from the combustion of 39.0 g of methane? Total mass =

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

4.- According to the following reaction: C3H8 + CO2 + H₂O What is the mass of CO2 produced if 865 g of C3H8 are consumed?
TABLE 3. PERCENT YIELD Mass salicylic acid 9 Mass of synthesized aspirin g 9 Theoretical Yield (aspirin) Percent Yield % Calculations: Note: Show calculations in a separate bond paper. (For the percent yield, you must first determine the limiting reactant from the following data: molar mass of salicylic acid = 138 g; molar mass of acetic anhydride = 102 g; density of acetic anhydride = 1.08 g/mL). TABLE 4. MELTING POINT DATA Sample Melting Point Range salicylic acid synthesized aspirin
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,)
C3H8(g) + O2(g) ------> CO2(g) + H2O(g) a. Balance the reaction: b. Determine the limiting reactant from 20.0 grams of 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:
10
the reaction of 15 moles of carbon with 30 moles of oxygen will result in a theoretical yield of ____ moles of CO2 is what?
When 33.9 g of CH4 reacts completely with excess chlorine yielding 52.0 g of HCI, what is the percentage yield, according to CH418) + Cl2g) - CH3Clg) + HClig) 67.2 34.8 65.2 32.8 O 77.3
10. What are shared in covalent bonds?* Cations Protons Electrons Anions 11. What type of reaction does the equation describe? LICIO2 --> LICI + 02 * Synthesis Double Replacement Single Replacement Decomposition 12. Molybdenum has a molar mass of 95.94 g/mol. How many moles are in 150.0g of Molybdenum? O 0.1563 mol O 0.6396 mol O 1.563 mol 6.396 mol O O
Consider the following chemical reaction: Fe (s) + O2(g) ---------> Fe2O3(s) 2.00 moles of iron is reacted with oxygen gas. Calculate moles of the product. A.) 4.00 moles B.) 0.500 moles C.) 2.00 moles D.) 1.00 moles
When 5.0 g of propane are reacted with O2, carbon dioxide and water are produced. How many grams of H2O can be produced by the complete reaction of those 5.0 g of propane with excess oxygen? 20 g 1.1 g 8.2 g 0.45 g 2.04 g
Sodium and chlorine react to form sodium chloride: What is the theoretical yield of sodium chloride for the reaction of 32.0 g Na with 107.2 g Cl2? A. 1.40 x 104 g NaCl B. 35.4 g NaCl C. 122 g NaCl D. 81.2 g NaCl
1. Ammonia can be generated by heating together the solids NH4Cl and Ca(OH)2. Other products of the reaction include CaCl2 and H2O. Initially a mixture of 33.0 g each of NH4Cl and Ca(OH)2 was heated. a. If the calculated percent yield was 98.27%, what is the experimental mass of the ammonia obtained? 2. A coffee-cup calorimeter having a heat capacity of 472 J/°C is used to measure the heat evolved when the following aqueous solutions, both initially at 22.6°C, are mixed: 100. g of solution containing 6.62 g of lead(II) nitrate, Pb(NO3)2, and 100. g of solution containing 6.00 g of sodium iodide, NaI. The final temperature is 24.2°C. Assume that the specific heat of the mixture is the same as that for water, 4.184 J/g · °C. The reaction is: Pb(NO3)2(aq) + 2NaI(aq) → PbI2(s) + 2NaNO3(aq) a. Calculate the heat evolved (in kJ) in the reaction. b. Calculate the ΔH (in kJ/mol) for the reaction under the conditions of the experiment.