125.5 grams of CO2 are calculated to be produced by a reaction using 70.1 grams of O2 but only 78.8 grams of CO2 are actually produced, what is the percent yield? Round your answer to 1 decimal place.

125.5 grams of CO2 are calculated to be produced by a reaction using 70.1 grams of O2 but only 78.8 grams of CO2 are actually produced, what is the percent yield? Round your answer to 1 decimal place.

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

Related questions

Q: If 3.29 g Cu(NO3)2 are obtained from allowing 2.05 g of Cu to react with excess HNO3: Part A What is…

Q: One way to collect zinc is to react solid zinc (II) oxide with carbon, which produces solid zinc and…

A: The number of moles of any substance can be calculated by dividing its mass and molar mass, the…

Q: Use the balanced equation, N₂ + O₂ 2NO, to answer the following question. How many grams of N, are…

Q: In an experiment, 12.4 g of KClO3 were carefully decomposed, and 4.52 of O2 gas were collected.…

A: Molar may of 02 =2X16 =32 g/mol Number of moles of Kcl103 initially =12.4 g/122.5g/mol =0.1 mol From…

Q: Mn (s) + 2 CuCl (aq) --> 2 Cu (s) + MNCI2 How many grams of Cu will be produced by 4.4 moles of Mn?…

A: Given reaction, Mn(s) + 2 CuCl(aq) → 2 Cu(s) + MnCl24.4 moles of Mn

Q: Use the balanced equation, N2 + O2 --> 2NO, to answer the following question. How many grams of…

A: The objective of this question is to determine the amount of O2 in grams that will completely react…

Q: Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium…

A: Answer: This question is based on the stoichiometric calculation of the reaction that we have…

Q: What are the theoretical yields of H2O and CO2 (in grams)? a.103.51 g and 152.27 g b. 56.50 g and…

Q: If you are given a chemical reaction and the measured amounts (in grams or mL) of all reactant(s),…

A: Solution - Theoretical yield is the amount of product that can be formed from given reactants by…

Q: Stoichiometry can be used to determine the mass (in grams) of a product. O True O False

Q: For the following reaction, 3.75 grams of carbon disulfide are mixed with excess chlorine gas. The…

Q: Generic Chemical Equation : 2a+4b----> 3c Q: If 10.0 miles of each reactant were used to complete…

A: The equation is 2a+4b---->3c From the equation, it is clear tha 2 moles of 'a' requires 4 moles…

Q: As part of the third-year chemistry lab curriculum students synthesize the compound phospbomolybdic…

A: Where WH, Wp, WMo, Wo are atomic weight of hydrogen, phosphorus, molybdenum and oxygen respectively.…

Q: grams

Q: Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2…

Q: A student is trying to figure out how many moles of potassium chloride are made from 4,0 grams of…

A: To get the anwer we must convert the amount of chlorine gas into moles & then multiply it by 2,…

Q: Consider the balanced chemical equation below: CH4 (g) + 3Cl2 (g) → CHCl3 + 3HCl If 16.05 grams of…

A: Solution -

Q: In the decomposition reaction,50.10 g of calcium chlorate was heated to produce calcium chloride and…

A: Calcium Chlorate is Ca(ClO3)2 Reaction: Ca(ClO3)2 --> CaCl2 (s) + 3O2(g)

Q: The reaction of 35.0 g of Al with 44.1 g of Cr₂O₃ produced 13.0 g of Cr. 2Al + Cr₂O₃ ⟶ Al₂O₃ + 2Cr…

A: The balanced reaction taking place is given as, => 2 Al + Cr2O3 → Al2O3 + 2 Cr Given: Mass of…

Q: 2. Consider this reaction: Cu₂0(s) + C(s) → 2 Cu(s) + CO(g) When 11.5 g of C reacts with 114.5 g of…

Q: 300 g of oxygen are allowed to develop metal oxide, which is a chemical combination of 100% of the…

A: A chemical reaction in which the number of atoms of each element on the reactant and on the product…

Q: consider the following balanced equation. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Determine the…

A: Given, N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Given, mass of N2O4 react = 60.0 g mass of N2H4…

Q: Gaseous butane (CH3(CH₂)₂CH3) reacts with gaseous oxygen gas (0₂ to produce gaseous carbon dioxide…

A: To determine the theoretical yield of water formed from the reaction of butane and oxygen gas,

Q: Ammonia can be produced using the Haber process, depicted below (not balanced): H2 (g) + N2 (g) →…

A: The ratio of actual yield to the theoretical yield multiply by 100 is known as percent yield.

Q: For the following reaction, 6.92 grams of carbon (graphite) are allowed to react with 9.86 grams of…

A: Given,The reaction:carbon (s) + oxygen (g) carbon dioxide (g)mass of carbon = 6.92 gmass of oxygen…

Q: Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2…

A: Given data : 1. Mass of methane = 15.7 g 2. Mass of oxygen gas = 89.7 g Balance Chemical reaction…

Q: Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and…

Q: Consider the reaction: 4 NH3(g) + 5O₂(g) →4 NO(g) + 6H₂O(g). If the reaction of 150.0 g of ammonia…

A: The mass of ammonia is 150.0 g.The mass of oxygen is 150.0 g.The actual yield of nitrogen monoxide…

Q: Aqueous sulfuric acid (H₂SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous…

A: To calculate the maximum mass of sodium sulfate (Na2SO4) that could be produced by the chemical…

Q: Gaseous butane (CH3(CH2)2CH3) reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide…

A: We have to calculate the theoretical yield of carbon dioxide.

Q: Gaseous butane (CH3(CH2)2 CH3) reacts with gaseous oxygen gas (①2) to produce gaseous carbon dioxide…

A: The objective of this question is to calculate the theoretical yield of carbon dioxide (CO2) from…

Q: Can someone find the percent yield of copper the experimental yield of copper = 0.73 Zn mass (g) =…

A: The reaction taking place can be written as, => Zn + CuCl2 ---------> ZnCl2 + Cu Given : Mass…

Q: How many grams of H₂O are formed when 89.6 g of Si₂H6 reacts with excess O2 in the following…

A: O2 present in excess while Si2H6 is limiting reagents.

Q: For the reaction whose balanced equation is as follows, find how many grams of zinc phosphate will…

A: The balanced chemical equation for the reaction is given as: 3 ZnCl2 + 2 (NH4)3PO4 → Zn3(PO4)2 + 6…

Q: Liquid octane (CH (CH, CH; reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…

A: The given data is as follows: The mass of octane = 60.5 g The mass of oxygen gas = 424 g The…

Q: In the following reaction, 2H2 (g) + O2 (g) → 2 H20 (g), how many moles of oxygen (O2) would be…

A: Given data contains, Moles of hydrogen is 17.8 moles.

Q: carbon monoxide (g) + oxygen (g) carbon dioxide (g

A: The limiting reagent is the reactant that is used up completely. The balanced chemical equation of…

Q: A chemist needs to add 3.5 moles NaClNaClto a reaction. How much NaCl should she measure out in…

A: Given: No. of mole of NaCl = 3.5 Molar mass of NaCl = 58.44g/mol Number of mole(n) = (mass of…

Q: 0.120 moles of C is reacted with 0.117 moles of O₂ to form CO and CO₂. 3C(s) +20₂(g) → CO₂(g)…

A: The limiting reagent is the compound which is completely consumed during the reaction. It can be…

Q: Gaseous methane (CH4) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂)…

Q: Consider the following chemical reaction HCl (aq) + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0…

A: Given: Mass of HCl=20.0 g Mass of HgNO3=30.0 g Percentage yield=78.4% To find: Reagent in excess…

Q: The synthesis of nitrous oxide gas (n2o) for anesthetic uses can be done by combining ammonia and…

A: The objective of the question is to determine the amount of oxygen needed to react completely with…

Q: For the reaction Ca(s)+Cl2(g)→CaCl2(s) calculate how many grams of the product form when 21.4 gg…

A: Given reaction is Ca(s)+Cl2(g)→CaCl2(s) We have to calculate how many grams of CaCl2 form when 21.4…

Q: Liquid hexane (CH3 (CH₂) CH3) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide…

A: Given -> Weight of hexane = 4.31 gm Weight of O2 = 27.8 gm Actual yield of CO2 = 7.66 gm

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

If 125.5 grams of CO2 are calculated to be produced by a reaction using 70.1 grams
of O2 but only 78.8 grams of CO2 are actually produced, what is the percent yield?
Round your answer to 1 decimal place.
Your Answer:
Answer
units

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1 : Solution ;

VIEW

Step 2 : Solution :

VIEW

Step by step

Solved in 2 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

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.
Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 0.689g of water is produced from the reaction of 1.1g of octane and 2.1g of oxygen gas, calculate the percent yield of water. Round your answer to 2 significant figures.
The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if the scientist concluded that % yield of the reaction ended up to be 77%.
Gaseous butane (CH3(CH2)2 CH3) reacts with gaseous oxygen gas (①2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). What is the theoretical yield of carbon dioxide formed from the reaction of 31.4 g of butane and 59.5 g of oxygen gas? Round your answer to 3 significant figures.
In a laboratory experiment, 5.0 g of aluminum metal is exposed to 23.2 g of chlorine gas which resulted to aluminum chloride. (atomic masses: Al = 26.98 g/mol; Cl = 35.45 g/mol) Round your answer in 2 decimal places. Which is the excess reactant? How much product is formed?
10. Ferrocene, synthesized in 1951, was the first organic iron compound with Fe-C bonds. An understanding of the structure of ferrocene gave rise to new ideas about chemical bonding and led to the preparation of many useful compounds. In the combustion analysis of ferrocene, which contains only Fe, C, and H, a 0.9437 g sample produced 2.233 g of CO2 and 0.457 g of H₂O. What is the empirical formula of ferrocene.
A student synthesizes alum starting with 4.924 grams of scrap aluminum. When the reaction is complete, 71.54 grams of alum are collected. What is the percent yield of this reaction? I know percent yield is actual / theoretical multiplied by 100% but I'm not sure how to identify which is theoretical or actual. Thank you for helping me!
Ammonia is produced by the balanced chemical reaction: 3H2lg) + N2g) → 2NH3(g) How many grams of ammonia can be produced from 22.7g of hydrogen with excess nitrogen present? (Hint: This is a limiting reagent question. Do not forget your significant digits and your units.) How many grams of ammonia can be formed from 36.3g of nitrogen with excess hydrogen present? (Hint: This is a limiting reagent question. Do not forget your significant digits and your units.) This is a limiting reactant problem: How many grams of ammonia can be produced from 22.7 g of hydrogen and 36.3 g of nitrogen? (Hint: This is a limiting reagent question. Do not forget your significant digits and your units. Also note that this question should be easy of you have answered Part A and Part B successfully.)
In a combustion reaction, 457 grams of C8H18 are reacted with 256 grams of O2. The reaction produced 160.1 grams of CO2. Determine the percent yield for this reaction. Provide your answer to 1 decimal place.
An amount (in grams) of nitrogen gas is reacted with excess hydrogen, according to the balanced reaction shown below. If 104 g of NH3 is recovered, giving a percent yield of 42%, what was the mass of the nitrogen (in grams) that reacted? N2 (g) + 3 H2 (g) --> 2 NH3 (g) Report your answer as an integer, that is as a number with zero decimal places, and with no units. Do NOT use scientific notation.
The theoretical yield of product for a particular reaction is 37.06 g. A very careless student obtained only 35.47 g of product after carrying out this reaction. What is the percent yield that this student obtained? Enter a number only; do not spell Include the correct number of significant figures for your answer Answer: % yield
Fernando is doing his pre-lab homework for Chemistry. He is asked to predict how many grams of CO, are produced if 2.09 mol of HCl are reacted according to this balanced chemical equation shown. CaCO3 +2 HCI → CaCl2 + CO2 + H20 He performs the following calculation. 1molEo, 2 metHCT 2.09 motHCI x 44.01 g CO. = 46.0 g CO, 1molEo, of the balanced On the day of the lab his group obtains 31.21 grams of CO2 as their experimental result. What is their percent yield in standard notation?