BookPrinterencesEnter your answer in the provided box.Calculate the number of g of C,Hg required to produce 31.5 g of H₂O using the following balancedequation:C3H8(g) +502(g) →→→3CO2(g) + 4H₂O(g)g C₂HgGL

First calculate the number of moles for H2O. Then use mol to mol ratio to calculate the mass of C3…

Answered: Enter your answer in the provided box.…

Enter your answer in the provided box. Calculate the number of g of C,H, required to produce 31.5 g of H₂O using the following balanced equation: C3Hs(g) +502(g) →→3C02(g) + 4H₂O(g) C₂H₂

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: A chemist plans to react 2.1 moles of aluminum with excess water according to the following…

A: Aluminium reacts with water to form aluminium hydroxide and hydrogen gas. The equation for the…

Q: How many moles of CO2 can be made from this reaction? CH4(g)+2O2(g)→CO2(g)+2H2O(g) Suppose 2.8…

A: Balanced Reaction CH4 (g) + 2O2 (g) ---> CO2 (g) + H2 O(g) Moles of methane=2.8mol Moles of…

Q: Balance the following chemical equation (if necessary) for the combustion reaction of propane:…

A: The combustion reaction of propane is given as, => C3H8 (g) + O2 (g) -------> CO2 (g) + H2O(g)…

Q: Consider the following reaction between sulfur trioxide and water: SO3(g)+H2O(l)→H2SO4(aq) A…

Q: In the reaction below the percent yield of Iron is 74.6% Fe (s) + CO₂ (g) Fe₂O3(s) + CO (g) →…

Q: 4. Given: H₂O 1 CH + 1 HNO3 → 1 CH₂NO₂ + 1 6 If a student wishes to make at least 6.66 x 10 24…

A: Avogadro's number = 6.022 × 1023 Number of molecules in 1 mol of a substance equals Avogadro's…

Q: Consider the following balanced chemical equation: 2Cu2O(s) + O2(g) → 4CuO(s) Determine…

A: From the reaction it is clear that 2 moles of Cu2O reacts with one mole of O2 to give 4 moles of…

Q: When copper(II) sulfate pentahydrate (CuSO4·5 H2O) is heated, it decomposes to the dehydrated form.…

Q: A mixture of 9.275 g of iron (II) oxide and 8.435 g of aluminum metal is placed in a crucible and…

A: To solve this problem we will use the given chemical equation .

Q: In the following reaction, identify the limiting reactant: C3H8 (g) + 5 O2 (g) → CO2 (g) + 2 H2O…

A: The reactant that is totally consumed in the reaction is known as limiting reactant. The amount of…

Q: Determine the theoretical yield of carbon dioxide, in grams, when 14.32 grams of O2 reacts…

A: A numerical problem based on mole concept that is to be accomplished.

Q: Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l)…

A: Mole of a substance or a mole of a particles is defined as exactly 6×10^23 particles which may be…

Q: How many moles of Al are necessary to form 29.2 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) →…

Q: Balance the following chemical reaction using the combination of a smallest possible set of whole…

A: In Balanced chemical equation number of atoms of each species are equal on both reactant and…

Q: Balance the following ng chemical equation (IT ecessary): 10 CSH10(g) + 15 O2(g) → 10 H2O(g) + 10…

A: The question is based on balancing the given equation. we have to systematically balance the atoms…

Q: Consider the balanced equation SiO2(s)+3C(s)→SiC(s)+2CO(g) Complete the following table showing the…

A: The balanced chemical reaction is given below.

Q: Use the balanced equation, 4K + O₂ 2 K₂O, to answer the following question. How many grams of K are…

A: mass of O2 = 19.1 gmolar mass of O2 = 32.00 g/molAtomic mass of K = 39.10 g/mol

Q: The Haber-Bosch process involves the combination of nitrogen and hydrogen at high temperatures in…

A: Answer:Reagent that exhuast first in the chemical reaction and decides the yield of product is…

Q: AlI3(s)+3K(s)->3KI(s)+Al(s) Consider the reaction of solid aluminum iodide and potassium metal to…

A: Given :- AlI3(s)+3K(s)->3KI(s)+Al(s) amount of Al produced = 131.75 g To calculate :- Amount…

Q: Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce…

A: The objective of the question is to determine the amount of ammonia produced, the limiting reactant,…

Q: A student combines 15.0 g FeS, with excess 02, which react according to the balanced equation shown…

A: Now, mass of one reactant is given and other reactant is present in excess. The amount of product…

Q: For the chemical equation given below (not balanced), the percent yield of the reaction is 65.0%.…

Q: Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the…

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

A: Thereotical yield : The maximum amount of product formed in given reaction is called as theoretical…

Q: One method used in the eighteenth century to generate hydrogen was to pass steam through red-hot…

A: Given that, a reaction is 3Fes+4H2Og→Fe3O4s+4H2g. The molar masses are Fe = 55.845 g/mol, H2O =…

Q: A sample of 8.61 g8.61 g of liquid 1‑propanol, C3H8O,C3⁢H8O, is combusted with 64.6 g64.6 g of…

A: It's a multiple part question. Given information, Mass of 1-propanol = 8.61 g Mass of oxygen gas =…

Q: Hydrogen cyanide, a highly toxic compound, is made by the following reaction: 2 CH4(g) + 2 NH3(g) +…

Q: Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When…

A: Given : Mass of Mg ribbon = 2.58 g Mass of oxygen = 8.70g

Q: an iron nail has a mass of 1.12 g, what mass of rust would form

A: Number of moles = mass / molar mass Number of moles of Fe = mass of Fe /55.845gmol-1

Q: Starting with the partially balanced equation, CH₂COOH(1) + O2(g) →?CO2(g) + 2H₂O(l) what…

A: Since, Balanced reaction means that both side number of atom present in equal number. Thus,

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: How many moles of Al are necessary to form 50.2 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) →…

A: Given Reaction 2Al(s) + 3 Br2(l) → 2 AlBr3 Mass of AlBr3 = 50.2 gram Number of mole of Al…

Q: A sample of 1.527moles of methane (CH4) is mixed with 1.32 moles of chlorine. What is the…

A: Methane reacts with chlorine to form carbon tetrachloride and hydrogen chloride. The equation for…

Q: Washing soda, a compound used to prepare hard water for washing laundry, is a hydrate, which means…

Q: summarizes the experimental quantities of reactants an specific batch. N2 (8) + 3 H2 (g) --> 2 NH3…

A: % Yield = Obtained mass x 100/Calculated mass

Q: Aspirin (C9H8O4) is synthesized by reacting salicyclic acid (C7H6O3) with acetic anhydride (C4H6O3).…

Q: Determine the mass (in grams) of carbon dioxide obtained when 7.04 g of C6H5OH reacts with 2.80 g of…

A: Below attached file showing the details answer. All the best.

Q: What is the mass in grams of CO₂ that can be produced from the combustion of 4.06 moles of butane…

Q: Lead ions can be precipitated from solution with KCl according to the reaction: Pb²+ (aq) + 2KCl(aq)…

A: Solution :-“Since you have posted multiple questions, we will provide the solution only to the…

Q: magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. When 10.1 g of…

A: Balance chemical equation is defined as which has equal number of atoms or ions in both sides…

Q: number of grams of C₄H₁₀

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

Book
Print
erences
Enter your answer in the provided box.
Calculate the number of g of C,Hg required to produce 31.5 g of H₂O using the following balanced
equation:
C3H8(g) +502(g) →→→3CO2(g) + 4H₂O(g)
g C₂Hg
GL

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: Approach to the problem

VIEW

Step 2: Moles calculation

VIEW

Step 3: Calculation of mass

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 4 images

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

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
Chloroform, CHCl3, reacts with chlorine, Cl2, to form carbon tetrachloride, CCl4, and hydrogen chloride, HCl. In an experiment 25 grams of chloroform and 0.36 mol of chlorine were mixed. Which is the limiting reactant? The equation is given as CHCl3 + Cl2 = CCl4 + HCl
What is the mass in grams of CO₂ that can be produced from the combustion of 6.54 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)
[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.
Determine the theoretical yield of water, in grams, when 19.66 grams of O2 reacts according to the reaction below. Use two decimal places for your molar masses and use the abbreviation for the unit. C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g)
According to the chemical reaction below, two atoms of sodium are required to react with a molecule of chlorine in order to form sodium chloride. How many grams of sodium metal are required to react completely with 2.00 grams o chlorine gas. 2 Na(s) + Cl2(g) → 2 NaCl(s)
Butane, C4H10C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atmatm and 23 ∘C∘C, what is the volume of carbon dioxide formed by the combustion of 2.00 gg of butane?
The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: N₂(g) + O₂(g) → 2 NO(g) If 5.220 g N₂ is mixed with 9.660 g O₂, calculate the theoretical yield (g) of NO produced by the reaction. g
Determine the grams of ammonia produced when 1.15 g of hydrogen H is reacted with 3.75 g of nitrogen N to produce ammonia (NH) according to the following chemical equation: 3H + N → 2NH
Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol
Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) Calculate the number of grams of NO produced as a byproduct of the reaction of 118.17 grams of Ag with excess HNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol
Consider the following equation: 4NH3(g) + 5 O2(g) → 4 NO(g) + 6 H₂O(1). 25 g of NH3 and 25 g of O₂ are allowed to react. How many grams of which reactant remains left over when the reaction goes to completion. 14.4 g NH3 left. 14.4 g 0₂ left. 10.6 g NH3 left. 10.6 g 0₂ left. 000 0.