Answered: What mass of oxygen is needed to react…

What mass of oxygen is needed to react with 5.37 g of acetylene (C2H2) accor to the following balanced equation? 2 C,H2 + 502 → 4 CO2 + 2 H2O Express your answer to 2 decimal places. Your Answer:

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 40PS

See similar textbooks

Related questions

Q: how to calculate moles of NaHCO3 and moles of CO2 from Mass of NaHCO3= 0.081g Volume of CO2=5ml…

A: We can determine the moles of substance from the mass as below : Moles of substance = ( mass of…

Q: 1. Calculate the GFW of chromium (III) carbonate, Cr2(CO3)3, to four significant figures. From…

Q: Given the following reaction : 4NH3(g) + 3 O2 (g) > 2N2 (g) + 6H2O (I) Calculate ∆G° 298

A: The standard thermodynamic data for the given reactants and products at given temperature is, 4NH3…

Q: When the following equation is balanced using the smallest possible integers, what is the number in…

A: In the given reaction, the Bold typed is NO2 which reacts with water form nitric acid and NO.

Q: An explosive reaction between butane and oxygen occurs as follows. 2 C4H10 (g) + 13 O2 (g) --> 8…

A: An explosive reaction between butane and oxygen occurs as follows. 2 C4H10 (g) + 13 O2 (g) --> 8…

Q: How many moles of NH3 are produced when 0.45 moles of H2 gas react with N2 gas? N2 + 3H2 -->2 NH3…

A: The balanced reaction taking place is given as, => N2 + 3 H2 -----> 2 NH3

Q: After you balance the following equation: n-octene (C8H16) + Potassium permanganate + sulfuric acid…

A: The chemical equation for the given reaction is: C8H16 + KMnO4 + H2SO4 → CO2 + H2O +…

Q: 15.00g of aluminum sulfide and 10.0g of water react until the limiting regeant is used up:…

A: Given information, AI2S3+6H2O=2AI(OH)3+3H2S 15.00g of aluminum sulfide and 10.0g of water

Q: What mass of oxygen is needed to react with 5.37 g of acetylene (C2H2) according to the following…

A: Given : Mass of C2H2 = 5.37g

Q: BASIC STOICHIOMETRY The reaction between pyrite (FeS2) and oxygen gas can be used to produce SO2 gas…

Q: reactions 3 What is the coefficient of CO, in the balanced equation for complete combustion of…

A: We will write the coefficient of CO2

Q: Two reactions take place in the reactor following the stoichiometry shown below: 2 A → 5 C and A →…

Q: In the following reaction, C5H12(1) + 8 02 (g) – 6 H20 (g) + 5 CO2 (g), how many moles of water…

A: C5H12 (l) + 8 O2 (g) -------> 6 H2O (g) + 5 CO2 (g) According to Stoichiometry of reaction; 8…

Q: Sulfuric acid can be manufactured using the reaction: 2S(s) + 3 O2(g) + 2 H2O(l) -> 2 H2SO4 (aq)…

A: We have to calculate the mass of sulphuric acid produced.

Q: Given the following decomposition reaction, calculate the moles of water produced from 6.21 mol of…

A: Moles of water produced from 6.21 mol of H2O2 in the following reaction 2H2O2(l)⟶2H2O(l)+O2(g)

Q: A container holds 100. g of P₄ and 150g of O₂.The following reaction occurs: P₄ + 3O₂ → P₄O₆. Which…

A: When a chemical reaction between the reactants occurs, they combine in a specific stoichiometric…

Q: Using the following equation, calculate the grams of V formed when 1540g of V2O5 reacts with 1960g…

A: Data given: Mass of V2O5 = 1540 g Mass of Ca = 1960 g Mass of V formed = ?

Q: In the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide and water.…

A: The given reaction is,

Q: Octane burns in air to give carbon dioxide and water. CH18(9) +- 0,(9) - co,(g) + H,O(g) Which of…

A: Given that, Octane burns in air to give carbon dioxide and water according to the equation :…

Q: HgI2+ 2KI + 2H2O —> K2[HgI4].2H2O 1 g of each reactant is weighed and the reactian is inserted and…

A: The reaction taking place is given as, => HgI2 + 2 KI + 2 H2O -------> K2[HgI4].2H2O Given :…

Q: Balance the following imaginary equation using the principles you would use for a real equation…

A: According to the Law of conservation of mass " all atoms of different elements must be equal on both…

Q: 4. In the background reading, it was pointed out that heroin can be produced from morphine in a…

A: The Density of Acetic anhydride is 1.08 g/cm3, then the mass of Acetic anhydride is - Mass of Acetic…

Q: How many grams of CO2 are produced from burning one gallon of biodiesel (3,311 g of biodiesel)?…

Q: Given the following reaction. 2Na2S + __Na2CO3 + __SO2(g) __Na2S2O3 + CO2(g) DH =-1025kJ A.…

A: We will calculate mass of CO2

Q: Show your work: Balance the following chemical equation: C7H16 + O2 ---> CO2 + H2O

A: Given Reaction : C7H16 + O2 ---> CO2 + H2O C7H16 + O2 ---> CO2 + H2O

Q: How many moles of O2 will form when 1.818 moles of CO2 react with 3.583 moles of KO2? Enter your…

A: According to the given chemical equation, the number of moles of KO2 (s) needed to react completely…

Q: How many grams of water would be formed from 96.0 g NH3 in a reaction represented by the balanced…

A: The reaction takes place in the stoichiometric ratio.

Q: For the balance equation shown below, how many moles of SO3 will react with 0.7727 moles of C4H8S2?…

Q: Methanol (CH3OH) burns in air according to the equation: 2CH3OH + 3O2 ---> 2CO2 + 4H2O If 231 g…

A: Combustion :- The process of buring a substance in excess of air or oxygen is known as combustion…

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

A: Percentage yield of carbon dioxide

Q: what are the coefficients missing on the following equation?_Ag2S--->_Ag+_S5 O (5,5,0) O (0,5,0) O…

A: Note : In the given equation it is written as S5, but in the terms of writing an equation in a right…

Q: Using the Haber-Bosch process: H2 + N2 → NH3 what is the excess and limiting reactant? what…

A: Given, H2 + N2 NH3 The balanced chemical reaction of…

Q: SO2(g) + Cl2 → SO2Cl2(g) SO2Cl2 + 2H2O → H2SO4 + 2HCl H2SO4 + Ca(OH)2…

A: the balanced chemical reaction for the above process is SO2(g) + Cl2 → SO2Cl2(g)SO2Cl2 + 2H2O →…

Q: in a reaction, 4.0g of sodium oxide was formed from 13.8g of sodium. Calculate the percentage yield

A: given. Experimental yield of Na2O = 4 gram given amount of sodium = 13.8 gram

Q: Toluene reacts with nitric acid to form ortho nitro toluene and water. After carrying out the…

A: In a chemical reaction, the amount of product formed is based on the amount of reactants that react.…

Q: If 6.3 kg of CO₂ are produced during a combustion reaction, how many molecules of CO₂ would be…

A: mass of CO2 = 6.3 kg = 6300 g molar mass of CO2 = 44 g/mol we need to find out the moles of CO2…

Q: Bismuth (III) sulphate reacts with ammonium hydroxide in a double displacement reaction. If 64.3 g…

A: Given, Bismuth (III) sulphate reacts with ammonium hydroxide in a double displacement reaction. Mass…

Q: Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum…

A: Answer :- Theoretical yield of Manganese (Mn) = 89 g…

Q: A container holds 100g of P₄ and 150g of O₂. The following reaction occurs: P₄ + 3O₂ → P₄O₆. What is…

A: The number of moles is equal to the ratio of mass to the molar mass of the substance. It is denoted…

Q: Adipic acid, H2C6H8O4, is used to produce nylon. It is made commercially by a controlled reaction…

A: Percentage yield is defined as the ratio of actual yield by theoretical yield multiplied by 100.…

Q: In the following balanced chemical reaction, what is the value of b (use only real number)? aCsH;OH…

A: The chemical reaction follows the law of conservation of mass. According to the law of conservation…

Q: What mass of oxygen is needed to react with 5.37 g of acetylene (C2H2) accord o the following…

A: Given : Mass of acetylene = 5.37g

Q: Part A. How many moles of O2, are needed to react with 1.40 mol of C2H2? Part B. How many moles of…

A: Given reaction 2C2H2 + 5O2 -> 4CO2 + 2H2O Moles of O2 =? Moles of C2H2 = 1.40mol

Q: For each of the following reactions, calculate the grams of indicated product when 25.0 gg of the…

A: (a) The equation is as follows: 2SO2 (g) + O2(g) → 2SO3 (g) No of moles of SO2 = 25.0g/(64.1gmol-1)…

Q: For the following balanced equation: CH4 + 4 Cl2 ==> CCl4 + 4 HCl Determine the number of moles of…

A: Number of moles formed depend balance reaction

Q: For the following balanced equation: CH4 + 4 Cl2 ==> CCl4 + 4 HCl Determine the number of moles of…

Q: Glucose oxidation is a chemical process that provided energy for an organism to carry out all of its…

Q: In the atmosphere, nitrogen dioxide reacts with water to produce NO and nitric acid: NO2 (g) + H2O…

A: Given unbalanced equation for the reaction of nitrogen dioxide with water to produce NO and HNO3 is…

Q: The equation shows the combustion of acetylene (C2H2) in an arc welder. 2C2H2+5O2⟶4CO2+2H2O…

A: Balanced chemical equation for the combustion of acetylene: 2C2H2 + 5O2…

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

I need a quick solution within 15 minutes With my best wishesTon.

What mass of oxygen is needed to react with 5.37 g of acetylene (C2H2) according
to the following balanced equation?
2 C2H2 + 5 02 → 4 CO2 + 2 H20
Express your answer to 2 decimal places.
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.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

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

About 5 billion kilograms of benzene, C6H6, are made each year. Benzene is used as a starting material for many other compounds and as a solvent (although it is also a carcinogen, and its use is restricted). One compound that can be made from benzene is cyclohexane, C6H12. C6H6() + 3 H2(g) C6H12() rH = 206.7 kJ/mol-rxn; rS = 361.5 J/K mol-rxn Is this reaction predicted to be product-favored at equilibrium at 25 C? Is the reaction enthalpy- or entropy-driven?
When methane is combusted, how many moles of oxygen gas are needed to react to form 2.19 moles of water? Use the equation below, round to the nearest 0.01, and remember to include units (properly abbreviated) and substance in your answer! CH4 + 2 O2 -> CO2 + 2 H2O
When a hydrocarbon such as butane (C4H10) is combusted, it produces water vapor and CO2 given in the reaction below: 2 C 4 H 10 + 13 O 2 ⟶ 8 C O 2 + 10 H 2 O If 404 g of butane are burned, how many grams of CO2 are produced? Round to the nearest whole number.
The equation for the complete combustion of ethene (C2H4 ) is: C2H4(g)+3O2 (g)>2CO2 (g)+2H2O(g) If 75.76 grams C2H4 reacts with 201.6 grams O2 , how many grams CO2 are produced? (Answer to one decimal place) grams CO2 What is the limiting reagent ? C2H4or O2 show all work
Calculate: 1. Mass of CO2 produced from the burning of 1.0 g CH4 . 2. Mass of O2 needed to react completely with 1.0 g CH4 . 3. Mass of CO2 produced if there is 1.0 g O2 . Note: Express your answers in 2 significant figures.
Octane, C8H18, can be used as a representative compound for gasoline.a. Is the combustion of octane a source or sink of a GHG? Explain.b. Write and balance the chemical equation for the combustion of octanec. Calculate the mass of carbon dioxide produced from the completecombustion of 1.0 gallon of gasoline, assuming the fuel is only octane.• Things to think about: How will you start this problem? Notice that youare not given grams initially, you are given 1.0 gallon. What conversionwill you use to get between gallons and grams? There are 3.785 litersin a gallon. Use 0.703 g/mL as the density of octane.
A common way to determine the catalyst: limiting reactant ratio in a catalytic reaction is to report the amount of catalyst used in mol%. For example, 5 mol% catalyst means that the reaction uses 5% as much catalyst as the limiting reactant. Showing all your work, calculate the mol% of Pd used in this reaction where R and R’ = H.
2.) Using the following equation for the combustion of octane, calculate the amount ofenergy released from 100.0 g of octane.2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ
Two reactions take place in the reactor following the stoichiometry shown below: 2 A → 5 C and A → 2 D If 135.2 mol of A is fed into the reactor, 29.0 mol of A is leaving the reactor at the end of the process and 97.0 mol of C is produced, calculate the percent yield of C. (Report in % format using two decimal figures, e. g. 99.99%)
The following equation represents the combustion reaction of octane (C8H18), which is the primary component in gasoline. 2C8H18(l) + 25 O2(g) --> 16CO2(g) + 18H2O(l) The molar mass of octane is 114.22 g/mol and its density is 0.69 g/mL. If 1.0 L of octane is completely combusted in excess of oxygen, how many kilograms of CO2 gas is released into the atmosphere?
3. Syngas is a mixture of carbon monoxide, carbon dioxide, and water vapor that is used for making fertilizer, methanol, and other products. It is produced by heating fossil fuels under low-oxygen conditions to promote incomplete combustion. Write an equation for the complete combustion of the gasoline component cyclopentane, C5H10 (l) and the incomplete combustion of cyclopentane with 20% of the carbon appearing as CO(g).
One method used in the production of H2 gas is to put the coal into an incomplete combustion reaction with air and water vapor in the combustion chamber (water gas production). A simplified reaction can be written as:2C + 1 H2O + a (O2+3.76N2) = 1C0 + 1CO2 + 1H2 + 3.76·a·N2 Here, 02+3.76N2 represents the amount of air and is multiplied by the coefficient "a".a) The value of the coefficient "a" for this reaction b) The amount of air to be used for 1 kg of pure carbon (C) (total amount of 02 and N2) (kg-air/kg-carbon) Hint: Consider how many kilograms 1 kmol "C" weighs.