Use the balanced chemical formula below to answer the following problem using dimensional analysis. Report answers with unit, substance, and corre number of significant figures. Use mol for moles and g for grams. 3 Mn + Al.(CO.), --> 2 Al + 3 MNCO, How many moles of manganese are needed to react with 12.2 moles of aluminum carbonate?

Use the balanced chemical formula below to answer the following problem using dimensional analysis. Report answers with unit, substance, and corre number of significant figures. Use mol for moles and g for grams. 3 Mn + Al.(CO.), --> 2 Al + 3 MNCO, How many moles of manganese are needed to react with 12.2 moles of aluminum carbonate?

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: N но What is the chemical formula for the limiting reactant in the reaction shown? chemical formula:…

A: Limiting reactant is the reactant which limits the extent of reaction or the reaction proceed…

Q: What mass of AgCl will be produced when 20.8 g of AgNO, and 8.20 g of CaCl, are reacted? Grams…

A: Given reaction equation; 2AgNO3 + 1CaCl2 ----> 1Ca(NO3)2 + 2AgCl Molar mass; AgNO3 =…

Q: Sodium nitrate, manganese (II) sulfate, potassium sulfate, and water is formed from the reaction of…

A: Given: grams of sodium nitrite (NaNO2) used= 47.68 g grams of potassium permanganate ( KMnO4 )…

Q: What mass, in grams, of KO2 will react with 287 g of CO2? Enter your answer to the ones place. Do…

Q: For the reaction Ti(s) + 2 F2 (g) ➡️ TiF4(s) compute the theoretical yield of the product (in grams)…

A: The reaction given is, => Ti (s) + 2 F2 (g) ➡️ TiF4 (s) Given : Mass of Ti taken = 6.0 g And mass…

Q: In parentheses you will see that the products is not balanced .*first we will have to balance the…

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

Q: Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4 Fe(s) +30,(g)-2 Fe,O,(s)…

A: We have to predict limiting reactant, theoretical yield and percentage yield.

Q: before performing any calculations. 1) What is the percent yield of iron (III) oxide if, when 250 g…

A: To solve this problem first we calculate the theoretical yield of iron oxide then we will calculate…

Q: With the aid of the following balanced equation and molar masses (MM), determine the answer for the…

A: Given - Molar mass of C6H10= 82.2 g/mol Molar mass of O2= 32 g/mol Molar mass of CO2= 44g/mol Molar…

Q: 8 In this experiment as long as 1.3g NaHCO3 or less is used it will be the limiting reactant.…

A: 8 ) we need to calculate moles of NaCl

Q: 9.) Answer the following for the balanced equation: P4+6Cl2---> 4PCl3 (this question is in 4 parts)…

A: The question is based on the concept of reaction stoichiometry. we need to identify limiting and…

Q: Use the balanced chemical formula below to answer the following problems using dimensional analysis.…

A: 1. Given that : Number of moles of aluminium carbonate = 7.46 mol Also given that Mn is in excess,…

Q: Use the References to access important values if needed for this question. An iron nail rusts when…

A: This problem is based on mole concept.Here we have to first write down the balanced equation then…

Q: Consider the following unbalanced equation ____Na2SiF6 + ____ Na ---------> ____Si +…

Q: Which of the equalities below is true for the following equation? Select ALL that apply. TICI4(s) +…

A: The given chemical equation: TiCl4 + 2 Mg → Ti + 2 MgCl2 1 mol 2 mol 1 mol 2 mol The…

Q: For the following reaction, 19.3 grams of sulfur dioxide are allowed to react with 10.3 grams of…

A: Given mass of SO2 = 19.3 gram Molar mass of SO2 = 64.066 gram/mole Given mass of H2O = 10.3 gram…

Q: Be sure to answer all parts. Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide…

A: Limiting Reagent is the reactant which is completely consumed when a reaction goes to completion.

Q: Determine the limiting reactant: 2H2 (g) + O2 (g) --> 2H2O (g) (balanced) 5 moles of oxygen gas…

A: Since we know that the reactant which are completely consumed in a chemical reaction is known as…

Q: CS2+302 CO₂+2SO₂ If 6.0mol of CS2 and 6.0 mol of O₂ react to form moles of the products. You can…

A: Given that, a chemical reaction is CS2 + 3O2 → CO2 + 2SO2. Also, given that, 6.0 moles of CS2 is…

Q: What is the mass in grams of CO₂ that can be produced from the combustion of 3.91 moles of butane…

A: We will use simple mole concept to answer the question. however, we have to use the balanced…

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

Use the balanced chemical formula below to answer the following problems
using dimensional analysis. Report answers with unit, substance, and correct
number of significant figures. Use mol for moles and g for grams.
3 Mn + Al:(CO.), --> 2 Al + 3 MNCO,
How many moles of manganese are needed to react with 12.2 moles of aluminum
carbonate?
How many moles of manganese(Il) carbonate will be produced when 85.61 g Mn
is reacted with excess aluminum carboante?

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 with 2 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

Using the equation below, find how many grams of tin (Sn) can be produced from 13.32 g of H2. Round to the nearest 0.01 and remember to include both units and substance. SnO2 + H2 --> Sn + H2O
In parentheses you will see that the products is not balanced .*first we will have to balance the products . Pls Help and write neatly so I can understand thank you!!!
Q.1: If 42.1 g of C4H10 0 react with 73.0 g of 02 according to the reaction Equation : C4H10 0 + 02 CO2 + H20 a) Write the balanced equation for the reaction. b) Determine the moles of given reactants b) Find the limiting reagent, c) calculate the mass of CO2 formed, d) If the actual yield of CO2 is 55.8 g, what is the percent yield? Given that: C= 12 g/ mol. , 0 = 16 g/ mol., : H = 1 g/ mol.
Consider the stoichiometry of the reaction provided in the question(s) below. a. A laboratory student started with 0.0812 grams of Reactant A (benzaldehyde, m.w. 106.12 g/mol). How many millimoles of Reactant A did the student add to the reaction mixture? b. A laboratory student started with 0.162 grams of Reactant B (sodium chromate, m.w. 161.97 g/mol). How many millimoles of reactant B did the students add to the reaction mixture? c. Which of the reactants is the limiting reagent? d. After running the reaction, the student isolated 0.0733 grams of signal product (benzoic acid, m.w. 122.12 g/mol). How many millimoles pf product did the student isolate? e. calculate the % yield of this reaction
Im stuck on the last three questions
Use the References to access important values if needed for this question. For the following reaction. 5.63 grams of iron(III) oxide are mixed with excess aluminum. The reaction yields 2.88 grams of aluminum oxide. Fe₂O₂ (s) + 2Al(s) Al₂O, (s) 2Fe (s) (1) What is the theoretical yield of aluminum oxide? (2) What is the percent yield for this reaction? % grams
fill in blanks and solve using the emthod shown! please
Q.1: If 42.1 g of C4H10 0 react with 73.0 g of 02 according to the reaction Equation : C4H10 0 + 02 CO2 + H20 a) Write the balanced equation for the reaction. b) Determine the moles of given reactants b) Find the limiting reagent, c) calculate the mass of C02 formed, d) If the actual yield of CO2 is 55.8 g, what is the percent yield? Given that: C= 12 g/ mol. , O = 16 g/ mol., : H = 1 g/ mol.