### Sodium and Chlorine Reaction to Form Sodium Chloride**Equation:**\[ 2 \, \text{Na}(s) + \text{Cl}_2(g) \rightarrow 2 \, \text{NaCl}(s) \]**Part A:****Question:**What is the theoretical yield of sodium chloride for the reaction of 55.4 g Na with 69.3 g Cl\(_2\)?**Options:**- 141 g NaCl- 57.1 g NaCl- 228 g NaCl- 114 g NaCl**Instruction:**Select the correct theoretical yield from the options given.*Note:* Make use of stoichiometry and molar mass calculations to determine the yield.**Additional Links:**- To better understand the concept, you can refer to Section 4.4 (Page).- Video resources: [KCV 4.4](#) and [IWE 4.6](#).**Feedback:**For any queries or additional help, please use the "Provide Feedback" option.

Answered: Image /qna-images/answer/714fbfea-055e-4ea5-a602-4ccaafc76618.jpg

Sodium and chlorine react to form sodium chloride: 2 Na(s) + Cl2(g) →2 NaCl(s) ▼ Part A What is the theoretical yield of sodium chloride for the reaction of 55.4 g Na with 69.3 g Cl₂? O 141 g NaCl O 57.1 g NaCl O228 g NaCl O 114 g NaCl

Sodium and chlorine react to form sodium chloride: 2 Na(s) + Cl2(g) →2 NaCl(s) ▼ Part A What is the theoretical yield of sodium chloride for the reaction of 55.4 g Na with 69.3 g Cl₂? O 141 g NaCl O 57.1 g NaCl O228 g NaCl O 114 g NaCl

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: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: Consider the given reaction is as follows; 2 NO (g) + O2 (g) → 2 NO2 (g) Moles of NO2 generated =…

Q: What is the mass in grams of H₂ that can be formed from 54.6 grams of NH3 in the following reaction?…

A: Given that the mass of ammonia is 54.6 g which decomposes to form nitrogen gas and hydrogen gas. The…

Q: What is the mass in grams of H2 that can be formed from 54.6 G of NH3 in the following reaction? 2…

A: From the stoichiometry, we can easily calculate , the problem.

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: The balanced reaction taking place is given as, => 2 NO (g) + O2 (g) → 2 NO2 (g) Given: Moles of…

Q: Based on the following chemical equation: 2 H2 + O2 2 H2O: Identify the limiting reactant when 32.0…

A: The balanced chemical equation given - The ratio between H2 gas and O2 gas is 2:1 mole ratio. We…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given : Mass of sucrose = 35.4 gram Molar mass of sucrose = 342 gm/mole

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: According to the chemical equation, the number of moles of oxygen required to produced 13.0 mol of…

Q: Carbon disulfide is produced by the reaction of Carbon and Sulfur dioxide. 5C (s)…

A: Percentage yield: It is the ratio of actual yield to the theoretical yield multiplied by 100.

Q: What is the mass in grams of H₂ that can be formed from 47.2 grams of NH₃ in the following reaction?…

A: A question based on stoichiometry, which is to be accomplished.

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: Percent yield = actual yield / theoretical yield x 100%.

Q: A 7.50 g sample of hydrogen peroxide decomposes according to the reaction b 2 H2O2(aq) - 2 H20(1) +…

Q: Only 4.00 g of O 2 were actually produced by the reaction below; this represents a 65.0% yield. How…

Q: How many moles of NO₂ would be produced from 6.2 mol of O₂ in the reaction below assuming the…

A: Given percent yield = 57.0 % => Actual YieldTheoretical Yield*100 = 57.0 The question asks to…

Q: How many grams of H₂ can be formed from 54.6 grams of NH₃ in the following reaction? 2 NH₃(g) → 3…

A: Given that the mass of ammonia is 54.6 g which decomposes to form nitrogen gas and hydrogen gas. The…

Q: What is the theoretical yield when 38.2 g Al reacts with 14.8 g O2 according to the following…

Q: What is the mass in grams of H₂ that can be formed from 31.6 grams of NH₃ in the following reaction?…

A: The number of moles, nNH3, of NH3 equivalent to 31.6 g of NH3 is; nNH3=mNH3MMNH3=31.6 g17.03…

Q: If you react 6.7g of iron oxide with 4.5g of aluminium, what is the theoretical yield of aluminium…

A: Given, Mass of iron oxide = 6.7g. Mass of aluminium = 4.5g. The moles of iron oxide and aluminium…

Q: What is the mass in grams of H₂ that can be formed from 34.0 grams of NH₃ in the following reaction?…

A: Mass of NH3 = 34.0 g Mass of H2 = ?

Q: Determine the theoretical yield of HCl

A: Number of moles = mass/molar mass Mass of HCl = moles of HCl × molar mass of HCl

Q: What is the mass in grams of H₂ that can be formed from 70.4 grams of NH₃ in the following reaction?…

A: Given, 70.4 grams of NH₃

Q: Consider the combustion of methane. CH4(g)+2O2(g)→CO2(g)+2H2O(g) Suppose 2.5 mol of methane are…

A: Given:Moles of CH4 = 2.5 mol.Moles of O2 = 3.5 mol.

Q: Nitrogen monoxide (NO), alongside water vapor, can be formed from the reaction between ammonia and…

A: In a chemical reaction, the amount of product formed depends on the amount of reactant that takes…

Q: The combustion of liquid ethanol (C2H5OH) produces carbon dioxide and water. After 4.62 mL of…

A: The balanced reaction of ethanol combustion is given as - C2H5OH + 3O2 -----> 2CO2 + 3H2O It…

Q: Al4C3 (s) + 12 H2O (l) → 4 Al(OH)3 (s) + 3 CH4 (g) In this reaction, 0.3455 mol of…

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: Balanced chemical equation is as follows: It is given that 84.9% of the theoretical yield is equal…

Q: What is the mass in grams of H₂ that can be formed from 43.6 grams of NH₃ in the following reaction?…

A: Molar mass of NH3 = Atomic mass of N + H x 3 = 14 g/mol + 1 g/mol x 3…

Q: Answer the questions about the balanced reaction 3 A + 2 B → 1 C + 100. cal The molar…

A: Given- A+2B->1C+100 cal Molar mass of A=10 gram Molar mass of B=20 gram Molar mass of C=70…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given - Un - Balanced Chemical equation is - C₁₂H₂₂O₁₁(s) + O₂(g) → CO₂(g) + H₂O(l) The balanced…

Q: Consider the reaction: 2 KCIO3 (s) → 2 KCI (s) + 3 O2 (g) How many electrons does an atom of…

A: Applying concept of oxidation state change due to electron .

Q: For the reaction Ti(s)+2F2(g)→TiF4(s)Ti(s)+2F2(g)→TiF4(s) compute the theoretical yield of the…

A: Determine number of moles of each reactant: From the balanced equation, it is clear that 1 mol Ti…

Q: Calculate the quantity of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below…

A: Given, actual yield of NO2 = 13.0 mol percent yield = 81.9 % we know, => percent yield of NO2 =…

Q: Nitrogen monoxide (NO), alongside water vapor, can be formed from the reaction between ammonia and…

Q: When 25.1 g NaCl and 27.2 g H 2SO 4 are mixed and react according to the equation below, how much…

Q: Lithium reacts with nitrogen to form lithium nitride. 6 Li(s) + N2(g) → 2 Li3N(s) In one experiment…

A: The % yield of the reaction is 25%.Explanation:

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

Q: What is the mass in grams of H₂ that can be formed from 55.6 grams of NH₃ in the following reaction?…

A: Mass of NH3= 55.6gm Mole of NH3= 55.6÷17= 3.27 Apply mole-mole relationship. Mole of H2=3.27×3/2=…

Q: The equation for the production of glucose through photosynthesis is: 6 CO₂ + 6 H₂O → C₆H₁₂O₆ + 6 O₂…

A: 1 mol = 6.022 x 1023 molecules/ions/entity Mass of 1 mole = molar mass Amount of product formed can…

Q: If the oxidation reaction below has a theoretical yield of 21.9 g H2O, what is the percent yield if…

A: The reaction given is 4 NH3 + 5 O2 → 4 NO + 6 H2O

Q: When 24.5g of NH 3 reacts, the actual yield of H 2O is 26.5g. What is the percent yield? 4NH 3(…

A: The percentage yield is the ratio of actual yield to that of theoretical yield whole multiplied by…

Q: For the chemical reaction given, how many grams of sulfuric acid, HS2O4, are needed to react…

A: Given, mass of sodium hydroxide(NaOH) reacted = 72.5 gwe know, molar mass of sodium hydroxide(NaOH)…

Q: quantity

Q: When 85.0 g of CH 4 are mixed with 160. g of O 2 what is the maximum amount of CO 2 that can be…

A: Mass of methane, CH4 = 85.0 g Mass of oxygen, O2 = 160. g Molar mass of methane, CH4 = 16.0 g/mol…

Q: Given that the reaction below has a yield of 84.36%, If you needed to create 26.29 g of SbCl3…

Q: How many grams of NO are required to produce 145 g of N₂ in the following reaction? 4NH3 + 6NO →→…

A: This can be explained as:

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

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: Determine the given values

VIEW

Step 2: Determination of limiting reagent

VIEW

Step 3: Determine the theoretical yield of NaCl

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

When 15.0 g of NH3 reacts, the actual yield of N2 is 6.50 g. What is the percent yield? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l) Group of answer choices 30.8% 21.1% 20.6% 31.1 %
What is the mass in grams of NO that will be produced from 22.9 g of NO, reacted with excess water in the following chemical reaction? 3 NO2(g) + H,0(1) → 2 HNO3(g) + NO(g) 2 ΗΝΟ:
Consider the reaction between sodium sulfide and copper(Il) sulfide: NazS (aq) + CuS04 (aq) -> Na2SO4(aq) + CuS (s) A chemist allows 16.7 g of Na,S and 35.0 g of CUSO, to react. Determine the theoretical yield of NazSO4 for the reaction. 31.1 20.5 30.4 O 21.0
How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming the reaction has only 69.8% yield? 2 NO (g) + O₂ (g) → 2 NO₂ (g)
What is the mass in grams of H₂ that can be formed from 54.4 grams of NH₃ in the following reaction? 2 NH₃(g) → 3 H₂(g) + N₂(g)
How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming the reaction has only 66.3% yield? 2 NO (g) + O₂ (g) → 2 NO₂ (g)
Balance each reaction, then suppose exactly 13.3 g of each reactant is taken. Indicate which reactant is the limiting reagent. Calculate the mass of each product that is expected. Al(s) + Cl2(g) → AlCl3(s)limiting reagent AlCl2 AlCl3 produced
The reaction of a 4.35-g K sample with excess oxygen (O2) yielded 4.82-g K20. What is the percent yield of this reaction? 4 K(s) + O2(g) – 2 K20(s) K 39.10 g/mol 02 32.00 g/mol K20 94.20 g/mol
For this reaction, 4.76 g hydrogen gas reacts with 50.3 g iodine. hydrogen (g) + iodine (s) hydrogen iodide (g) What is the maximum mass of hydrogen iodide that can be formed? What is the FORMULA for the limiting reagent? X What mass of the excess reagent remains after the reaction is complete? x g X 9
What is the percent yield if 28.16 g of CO2 is collected from a reaction with a theoretical yield of 225.3 g of CO2? 20.00% 50.00% O 25.00% O 12.50%
For the following reaction, how many moles of oxygen gas are required to react with 4.5 moles of Mg? 2 Mg (s) + O2(g) → 2 MgO (s)
What is the mass in grams of H₂ that can be formed from 47.0 grams of NH₃ in the following reaction? 2 NH₃(g) → 3 H₂(g) + N₂(g)