If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr,Methanol (CH4O) is converted to bromomethane (CH3B1) as follows:21.CH40 + HBr→ CH3B1 + H2Ogwhat is the percentage yield?a.40.9%b.82.6%2MSOс.100.%d.121%е.245%

Given: 12.23g bromomethane produced by reaction of 5.00gmethanol with excess HBr To find: percentage…

If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, Methanol (CH4O) is converted to bromomethane (CH3Br) as follows: CH4O + HBr → CH;Br + H20 what is the percentage yield? 40.9% a.

If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, Methanol (CH4O) is converted to bromomethane (CH3Br) as follows: CH4O + HBr → CH;Br + H20 what is the percentage yield? 40.9% a.

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: 1. The following is an important industrial reaction used to make methanol (CH3OH):…

Q: How many grams of CaCl2 can be produced by reacting 1.34 moles of CaO and 2.47 moles of HCL by the…

A: We are given a reaction., CaO+2HCL= CaCl2 + H2O Now from the reaction we can say that 1 mole of CaO…

Q: Ozone, O3 is formed in vehicle exhaust by the reaction NO2(g) + O2(g) —-> NO(g) + O3(g). What is the…

A: Given:mass of NO2 =2.0gAlso we know,Molar mass of NO2 = 46gMolar mass of O3= 48g

Q: Equation: HC2H3O2 + CaCO3 calcium acetate + H20 + carbon dioxide B. Calculation: If 9.02 x 1024…

A: The reaction taking place is given as, => HC2H3O2 + CaCO3 → Ca(C2H3O2)2 + H2O + CO2 Given: Number…

Q: Given - 1P4 (s) + 5O2 (g) —> 1 P4O10 (g) a) calculate the mass of P4 (s) required to produce…

A: Consider the reaction equation: 1P4(s) + 5O2(g) —> 1 P4O10(g) Molecules of P4O10 = 3.22×1023…

Q: Potassium metal reacts with water according to the following balanced equation. 2 K(s) + 2 H₂O(1) →→…

A: The objective of the question is to understand the stoichiometry of the given chemical reaction and…

Q: 15.50 g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.50 g AgCl is produced. What is…

A: The balanced reaction taking place is given as, => NH4Cl + AgNO3 ------> AgCl + NH4NO3 Given…

Q: Calculate the amount in grams of carbon dioxide from the amount of sodium bicarbonate that you used…

Q: A reaction mixture of 18.215g Na2CO3 and 10.938g HCl react according to the following balanced…

A: The mole ratio between HCl and Na2CO3 is 2 : 1 . First, identify the limiting reactant, Moles…

Q: Give the percent yield when 2.816 g of CO 2 are formed from the reaction of 45.69 g of C 8H 18 (MM =…

A: The percent yield is calculated by applying mole-mole analysis on given reaction.

Q: When 46.19 g NH3 reacts by the following balanced equation, 27.98 H₂O are formed. 4NH3(g) +502(g)…

A: Step 1: Given the information.When 46.19 g NH3 reacts with the following balanced equation, 27.98 g…

Q: If 4.50 g of HCI are reacted with 15.00 g of CaCO3, according to the following balanced chemical…

Q: 1.) If 6.0 grams of CaCO3 reacts with excess HCI, what mass of water should be formed? The balanced…

A: Since you have asked multiple type questions, we will solve only first questions for you. If you…

Q: Urea is prepared by reacting ammonia with carbon dioxide as shown in the reation equation image. In…

A: The objective of this question is to calculate the mass of urea formed when 637.2g of ammonia reacts…

Q: How many moles of water are produced when 6.33 moles of CH4 react? CH4 (g) + 2O2 (g) --> CO2 (g) +…

Q: 10.) The reaction of limestone with hydrolic acid is CaCO3 + 2HCl → CaCl₂ + CO₂ + H₂O If the…

Q: Calculate the mass of H2O formed by burning 4.00 g of C2H5OH. The reaction is C2H5OH (l) + 3O2 (g)…

Q: if 3 mol Al reacts with excess O2. How many moles of Al2O can be formed?

A: HE REACTION WILL BE AS FOLLOW: 4Al(s) + O2(g)----------->2Al2O(s)

Q: When 12.4 g of CH4 is reacted with excess O2, a mass of 20.8 g of CH4O is recovered. What is the %…

A: The number of moles of a compound can be determined as: Number of moles=Given massMolar…

Q: A reinforced steel cylinder is filled with 21.0 moles of hydrogen and 12.0 moles of oxygen. The…

A: Given: Moles of Hydrogen: 21.0 mol Moles of Oxygen: 12.0 mol To Calculate: The theoretical yield in…

Q: Calculate the percent yield for the reaction if 76.8 g of H2O reacted completely with nitrogen…

Q: Suppose 6.0 g of each reactant was used in the balanced reaction: 2Al (s) + 3Cl2 (g) = 2AlCl3 (s)…

A: Number of moles can be determined as follows: No.of moles of Al=massmolarmass=6.0 g26.98 g/mol=0.22…

Q: Draw the major organic product of the reaction shown below. HO Hox + HCI • You do not have to…

A: For given nucleophilic reaction determine major product when alcohol reacts with HCl

Q: For the following reaction, if I start this reaction with 153.0 grams of hydrobromic acid and an…

Q: Macmillan Learning Polychlorinated biphenyls (PCBs), which were formerly used in the manufacture of…

A: We have to calculate moles and grams needed/produced for the given reaction

Q: Tetraphosphorus hexaoxide (molar mass = 219.9 g/mol) is formed by the reaction of phosphorus with…

Q: Nitrogen and hydrogen react to form ammonia according to the following balanced equation: N2(g) +…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Determine the limiting reactant in the reaction. Calculate the amount in grams of CO2 from thew…

Q: In a reaction, 0.77 kg of V,O; are reacted with 0.88 kg of Ca as the following chemical Equation:…

A: This a question based on stoichiometric calculations of a reaction. Which can be solved step by…

Q: The following two-step process has a 30.0 % yield for each step. CH4 + 4 Cl2 + CCL + 4 HCI CC4 + 2…

A: Given that: The % yield of each step = 30.0% Moles of CH4 used= 4.00 mol.

Q: In the reaction below, 7.0 mol of NO 5.0 mol O2 are reacted together. The reaction generated 3.0 mol…

A: The formula for percent yield calculation is - Percent yield = (actual yield of product/theoratical…

Q: According to the balanced reaction below, calculate the moles of NO2 that form when 5.20 x 10-3 mol…

Q: What mass in grams of NaNs is required to produce 50.2 Lof N2 gas (density = 1.25 g/L ) according to…

A: Given that 50.2 L of N2 and density is 1.25g)l

Q: For the reaction represented by the equation CH4+2O22-->2H2O+CO2 calculate the percentage yield of…

A: Percentage yield of carbon dioxide

Q: The following precipitation reaction is perfomed using 3.785 g of FeCk and 2.258 g of NaOH. FeCk…

A: The highest product amount produced in any chemical change is denoted as its "theoretical yield". It…

Q: For the following balanced reaction: 2H2 + O2 = 2 H2O How many grams of H2O (Molar mass: 18g/mol)…

A: For the following balanced reaction: 2H2 + O2 = 2 H2O

Q: If 50.0 g of water is combined with 155.3 g of PCl3, PCl3(l) + 3H2O (l) --> H3PO4 (aq) + 3HCl (aq)…

Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr,
Methanol (CH4O) is converted to bromomethane (CH3B1) as follows:
21.
CH40 + HBr
→ CH3B1 + H2O
g
what is the percentage yield?
a.
40.9%
b.
82.6%
2MSO
с.
100.%
d.
121%
е.
245%

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

For the reaction: 2C2H5COOH + 7O2 -> 6CO2 + 6H2O Calculate the number of moles of O2 required to react with 29.616 grams C2H5COOH.
An intermediate step in the industrial production of nitric acid, HNO3, involves the reaction of ammonia, NH3, with oxygen gas, O2, to form nitrogen monoxide, NO, and water, H2O. 4 NH3 (g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) Molar masses (g mol-1) NH3 = 17.03 O2 = 32.00 NO = 30.01 H2O = 18.02 (a) Assuming excess O2, how many grams of nitrogen monoxide, NO, (i.e., the theoretical yield of NO) can be formed by the reaction of 46.00 g of ammonia, NH3 b. Assuming excess NH3, what is the theoretical yield of NO if we start with 73.00 grams of O2? c.If we start with 8.0 moles of NH3 and 8.0 moles of O2, how many moles of NO will we produce? d. If we have 36.00 g of NH3 and 72.00 g of O2, what is the theoretical yield of NO
How many moles of lithium hydroxide would be required to produce 50.5g of LizCOs in the following chemical reaction? 2 LIOH(s) + CO:(g) Li:CO:(s) + H2O(I)
Given the equation: 4 NH3 + 7 O2 ----> 4 NO2 + 6 H2O (a) How many moles of NH3 must react if 24.8 moles of water are produced? (b) Determine the number of moles of H2O that would be formed from the combustion of86.0 grams of NH3.
Consider the reaction between HCl and O2: 4HCl(aq) + O2(g) -> 2H2O(l)+2Cl2(g) When 15.4 g of HCl reacts with 18.2 g of O2, 14.3 g og Cl2 are collected a) Determine the limiting reactant b) Deteremine the theoretical yield of Cl2 c) Determine the % yield of Cl2
4. An old antacid commercial claimed that each tablet of their product could "neutralize 47 times its mass in stomach acid". The active ingredient in the antiacid tablet, NaAl(OH)₂CO3, reacts with HCl in stomach acid according to this balanced reaction: NaAl(OH)₂CO3 + 4 HCl →→ NaCl + AlCl³ + 3 H₂O + CO₂ How many moles of HCl can a 1.03 g of antiacid tablet neutralize if the tablet contains 0.246 g of the active ingredient? If stomach acid has a concentration of 0.14 M HCl, assuming the density of stomach acid to be similar to that of water (1.00 g/mL), what is the mass of stomach acid that the 1.03 g of antiacid tablet can neutralize? Does this number support the claim in the commercial?
How many moles of HNO3 will be produced from the reaction of 41.5 g of NO, with excess water in the following chemical reaction? 3NO2(g) + H20 (1) → 2 HNO,(g) + NO(g)
2. Balance the equation below for the reaction of benzil with sodium borohydride. ○ O C-C + BH4 + H₂O HH C-C- | | OH OH + 3. Calculate the number of moles of sodium borohydride and benzil used in the experiment. Considering the balanced equation, which of these is the limiting reactant? B(OH)4
In the combustion of pentanol according to the equation: 2C5H11OH + 15 O2 → 10CO2 + 12H2O How many molesof CO2 are produced if 2.28 mole of H2O are produced
What does the mechanism of this reaction look like? Please include arrows, lone pairs, and formal charge
For the reaction represented by the equation SO3+H2O-->H22SO4 how many grams of sulfuric acid (H22SO4) can be produced from 197 g of water and 460g of sulfer trioxide?
According to the balanced reaction below, calculate the quantity of moles of NH, gas that form when 4.20 mol of N,H, liquid completely reacts: 3 N,H,(1) → 4 NH,(g) + N,(g)