Answered: Calculate the moles of CO2 when 20.0…

Science

Chemistry

Calculate the moles of CO2 when 20.0 grams of C3H8 reacts with an excess of 02 C3H8 + 502 → 3CO2 + 4H20

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.35PAE

See similar textbooks

Related questions

Q: How many molecules of CO2 are produced if 67.23g of C2H8 are reacted in excess oxygen?

A: The combustion of C2H8 in the excess of oxygen can be represented by the following reaction:-…

Q: Calculate the theoretical yield for S8 when reacting 84.0 g of 8SO2 and 84.0 g of 16H2S,…

Q: Methanol (CH4O) is converted to bromomethane (CH3Br) as follows: CH4O + HBr → CH3Br + H2O If…

A: Solution: Percentage yield gives us the actual amount of product theoretically produced…

Q: According to the balanced reaction below, calculate the quantity of moles of NH₃ gas that form when…

A: Given : 3 N₂H₄(l) → 4 NH₃(g) + N₂(g) number of moles ofN₂H₄ = 4.20 mol To calculate :- number of…

Q: Ammonium dichromate decomposes according to the following reaction. (NH4)2Cr207 → N2 + 4H2O + Cr2O3…

Q: For the following reaction: 6Na + Fe2O3 --> 3Na2O + 2Fe Determine the theoretical yield of iron that…

A: Consider the given balanced reaction as; Reaction: 6 Na + Fe2O3 → 3 Na2O + 2…

Q: Determine the amount of excess reagent (in grams) left over after 0.3893 g C6H6 reacts with O.3914 g…

A: The substrate which is not fully consumed in the reaction,is called excess reagent. And the…

Q: Given the balanced chemical reaction: 2CH3OH + 302 - 2 + 4H₂0 Use the mass of the following elements…

Q: Hydrolysis of the compound B5H9 forms boric acid, H3BO3. Fusionof boric acid with sodium oxide forms…

A: Given: Mass given of borate salt (Na2B4O7) =151 g Mass to be calculated of B5H9 = x (say)

Q: Using the following equation, determine the % yield from the following reaction if 3.040E+1 g of…

A: Mass of octane = 30.04 g Mass of CO2 = 81.85 g

Q: (S) Indicate the calculation of how many grams of aluminum oxide (Al2O3) would be produced from the…

A: From the balanced reaction we can calculate the mass of reactant required and the product formed .

Q: Boron trichloride is prepared from the following reaction:…

A: Mass of B2O3 = 3.387 g Mass of Cl2 = 9.504 g Mass of C = 2.509 g We need to find limiting…

Q: 19)Consider the unbalanced chemical equation below. How many grams of CO2 can you produce from 5.33…

Q: A)What mass of ammonia gass can be produced from a reaction between 565.0g H2 and 880.0g of N2…

Q: Given the reaction: N2(g) + 3H2(g) → 2NH3(g) What is the total number of moles of NH3(g) produced…

A: The question is about to calculate the total Number of Moles of NH3 produced when 10 moles of H2 (g)…

Q: How many grams of magnesium oxide can be produced by reacting 0.248g magnesium that is 97.5% pure…

A: Given- Mass of magnesium = 0.248 g Molecules of oxygen = 5.36 x 1021 Magnesium is 97.5 % pure To…

Q: Ammonia is produced from the reaction of nitrogen and hydrogen according to the following equation:…

A: The values are given as follows:

Q: 5.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Given: 5g of compound X is made up of carbon, hydrogen and oxygen. Its molar mass is 128g/mol. It is…

Q: PBr5 is prepared according to the following reaction: PBr3 + Br2 → PBr5 When 65.6 g of Br2 reacts…

A: The reaction is, PBr3 + Br2 → PBr5 Clearly, from the above reaction,…

Q: Consider the following balanced chemical equation: C2H6O + 3O2 → 2CO2 + 3H2O If 3.5 moles of…

A: The given balanced chemical equation is as follows: C2H6O + 3O2 → 2CO2 + 3H2O The mole of oxygen…

Q: (29) When 35.0 kg of SiO2 reacts with 25.3 kg of carbol recovered, what is the percent yield for the…

Q: following combustion reaction: C₇H₈(l)+ 9 O₂(g) → 7 CO₂(g) + 4 H₂O(g)

A: Balanced chemical reaction, C7H8(l) + 9 O2(g) ---> 7CO2(g)+ 4H2O(g) Moles of C7H8 = 0.05090 mol…

Q: How many moles of NH₃ can be produced from 2.02 moles of nitrogen in the following reaction: N₂…

A: Balanced reaction is the reaction in which the number of atoms of reactants and products are equal.

Q: 2.94 g of hydrated calcium chloride CaCl2•xH2O is treated with excess K2SO4 in a double replacement…

A: Balanced double replacement reaction is CaCl2. xH2O + K2SO4 → CaSO4 + 2KCl + xH2O

Q: 7. Given the reaction: Pb(CH3COO)2 + H2S → PbS + 2CH3COOH How many grams of PbS is produced when…

A: Given, mass of H2S = 5.00 g Molar mass of H2S = 34.1 g/mol Molar mass of PbS = 239.3 g/mol

Q: For the reaction CaCl2 + 2AgNO3 --> 2AgCl + Ca(NO3)2 , if AgNO3 is added in excess, what is the…

Q: According to the balanced reaction below, calculate the quantity of moles of NO2 gas that forms when…

Q: For the reaction CaCl2 + 2AgNO3 --> 2AgCl + Ca(NO3)2 , if AgNO3 is added in excess, what is the…

A: As AgNO3 is in excess, so CaCl2 is limiting reagent. Mass of CaCl2 = 18.7 g Molar mass of CaCl2 =…

Q: Based on the balanced equation 2I2O5 + 10NO → 5N2O4 + 2I2 calculate the number of excess…

A: Given, number of molecules of N2O5 = 196 molecules number of molecules of NO = 1020…

Q: Glucose, C6H12O6,, is used as an energy source by the human body. The overall reaction in the body…

A: We have given the overall balanced chemical equation C6H12O6(aq) + 6O2(g) ⟶ 6CO2(g)…

Q: If you had 8 CO2 molecules and 6 H2O molecules…. How many molecules of C2H4 could you produce?

Q: What is a limiting reagent and theoretical yield in grams of NO2 when 10.0 g NH3 react with

A: Given , mass of NH3 = 10.0g. Mass of O2 = 10.0 g. The balance reaction is…

Q: mass

Q: Fernando is doing his pre-lab homework for Chemistry. He is asked to predict how many grams of CO2…

A: We know that: percent yield=experimental yieldtheoretical yield×100

Q: How many moles of NH₃ can be produced from 4.77 moles of nitrogen in the following reaction: N₂ (g)…

Q: Asprin, C9 Hg C4, is synthesized by the reaction of salicylic acid, C7H6O3, with acetic anhydride,…

A: The balanced reaction taking place is given as, Given: Mass of C7H6O3 taken = 0.04 Kg = 40 g…

Q: If exactly 4.089 moles of propanol (C3H8O) is combusted in the presence of excess oxygen what is…

A: Given data: The moles of propanol combusted is 4.089 mol. To calculate: The mass of O2 was used in…

Q: Aniline (C6H5NH2) can be produced from chlorobenzene (C6H5Cl) via the following reaction: C6H5Cl…

A: Reaction: C6H5Cl(l) + 2NH3 (g) → C6H5NH2(l) + NH4Cl (s) In general, 1 mole of C6H5Cl reacts with 2…

Q: Given the following reaction equation: C4H10 (g) + O2(g) → CO2 (g) + H2O (l) 1) Balance this…

A: the solution is as follows:

Q: Copper (II) oxalate tetrahydrate can be produced by the reaction of copper(Il) chloride tetrahydrate…

Q: C6H14+O2>>>CO2+H2O What mass of Oxygen(O2) is required to react completely with 25.0g C6H14?

A: For the given reaction, the balanced chemical equation can be expressed as follows : 2C6H14 + 19O2 →…

Q: 2C4H10 + 13O2 = 8CO2 + 10H2O How many grams of CO2 are produced by burning 9.41 g of C4H10?

Q: Methanol (CH4O) is converted to bromomethane (CH3Br) as follows: CH4O + HBr ® CH3Br + H2O…

Q: Step 2b: Use dimensional analysis to determine the theoretical yield of the product. Calculate the…

Q: Calculate the theoretical yield in grams ALI3 from the complete reaction of 18.3 grams AL according…

A: Given - Reaction 2Al (s) +3 I2 (s) -> 2AlI3 (s) Mass of Al = 18.3 g To find- Theoretical yield…

Q: Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00…

A: We have to calculate the theoretical yield of CO2 from the reaction of 4.00 moles of C8H18 with 4.00…

Q: calculate the theoretical yield in grams All3 from the complete reaction of 113g l2 According to the…

A: 2 Al(s) + 3 l2(s) --> 2 All3(s) According to the above reaction, 3 moles…

Q: A mixture of 0.020 mol of Mg and 0.020 mol Cl2 reacted completely to form MgCl2 according to the…

Concept explainers

Analytical Tools

Analytical tools or analysis tools help one to get into a conclusion or results from the data collected. Analytical tools can be applied for simple data sets and also in the case of big data analytics.

Question

can u help me with this?

Calculate the moles of CO2 when 20.0 grams of C3H8 reacts with an excess of
O2
C3H8 + 502 → 3CO2 + 4H20

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

4.43 Magnesium nitride forms in a side reaction when magnesium metal burns in air. This reaction may also be carried out in pure nitrogen. 3Mg(s)+N2(g)Mg3N2(s) If 18.4 g of Mg3N2forms from the reaction of 20.0 g of magnesium with excess nitrogen, what is the percentage yield?
Hexamethylenediamine (C6H16N2) is one of the starting materials for the production of nylon. It can be prepared from adipic acid (C6H10O4) by the following overall equation: C6H10O4(l) + 2NH3(g) + 4H2(g) C6H16N2 (l) + 4H2O (l) What is the percent yield for the reaction if 765 g of hexamethylenediamine is made from 1.00 103 g of adipic acid?
4.45 If 21 g of H2S is mixed with 38 g of O2 and 31 g of SO2 forms, what is the percentage yield? 2H2S+3O22SO2+2H2O
4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.
Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.
Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide. Starting with 2.2 mol NO, calculate how many moles and how many grams of O2 are required for complete reaction. Calculate what mass of NO2, in grams, is produced.
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
For the following reactions, write the ratios that can be established among molar amounts of the various compounds. 2H2+O22H2O 2H2O22H2O+O2 P4+5O2P4O10 2KClO32KCl+3O2 xs
Using the same reaction, calculate the mass of nitrogen produced when 200. g N2O4 and 100. g hydrazine react.
ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.