42.9 g of Aluminum nitrite and 97.2 g of ammonium chloride react to form aluminum chloride, nitrogen, and water. How many grams of the excess reagent remain after the reaction? Enter to 1 decimal place.

42.9 g of Aluminum nitrite and 97.2 g of ammonium chloride react to form aluminum chloride, nitrogen, and water. How many grams of the excess reagent remain after the reaction? Enter to 1 decimal place.

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 132E: DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a...

See similar textbooks

Related questions

Q: For the following reaction, 4.41 grams of carbon (graphite) are allowed to react with 15.8 grams of…

A: To calculate the amount of carbon dioxide that can be formed we need to know its molecular mass and…

Q: For the following reaction, 28.9 grams of sulfur dioxide are allowed to react with 6.29 grams of…

Q: Use 1 decimal point for all atomic masses. 12.1 g of C2H4(g) are reacted with 0.924 g of HCl(g) by…

A: Determine limiting reagent:From the balanced chemical equation, 1 mol of C2H4 and 1 mol of HCl…

Q: ximum amount of sulfur trioxide that can be formed? grams PRMULA for the limiting reagent? of the…

A: Given, Balanced chemical reaction, 2SO2(g) + O2(g) ---> 2SO3(g) Mass of SO2 = 28.8 g Moles of…

Q: miting reagent? of nitrogen mon

A: Balanced chemical reaction, N2(g) + O2(g) ----> 2NO(g) Moles of N2 = 0.174 mol Moles of O2 =…

Q: Through several successive reactions, a chemist uses carbon, CaO, HCl, and H₂O to produce C₆H₄Cl₂…

Q: Mass of sample (g ) 1.94g Mass of empty crucible (g) 84.248g Crucible and sample after heating…

A: Mass of sample = 1.94 g Mass of empty crucible (g) = 84.248 g Crucible and sample after heating (g)…

Q: If you are given 2.50 g C2H4 and 2.75 g of O2 to conduct the combustion reaction written below: C2H4…

Q: Balance the following equation. What are the missing coefficient? ___NH3(g) +____O2 (g)---> ____N2…

A: Here ammonia is oxidised in presence of oxygen and converted to nitrogen.

Q: For the following reaction, 6.65 grams of oxygen gas are mixed with excess hydrogen sulfide. The…

A: The theoretical yield of the reaction can be calculated by calculating the yield of water produced…

Q: Determine the mass of CaSO4 in the sample based on the following data to two decimal places mass of…

A: When the sample is heated the water present in the sample is evaporated and anhydrous CaSO4 is…

Q: For the following reaction, 0.271 moles of nitrogen gas are mixed with 0.565 moles of hydrogen gas.…

A: To find limitng reagent mole-mole analysis is applied on balanced chemical reaction.

Q: Part A(already solved): 2NO (g) +O2 (g) --> 2NO2 (g) Part B: You are provided with 2.56 mol of…

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

Q: If a solution containing 111.49 g of silver nitrate is allowed to react completely with a solution…

A: Given that : The mass of silver nitrate = 111.49 g The mass of lithium bromide = 10.39 g The molar…

Q: Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and…

Q: You run the reaction with two unknown quantities of copper sulfide and nitric acid and capture all…

Q: In the following reaction, 2H2 (g) + O2 (g) → 2 H20 (g), how many moles of oxygen (O2) would be…

A: Two moles of hydrogen gas reacts with one mole of oxygen gas to form two moles of water.

Q: A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands…

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: Al reacts with hydrochloric acid according to the following balanced equation: 2 Al + 6 HCl ==> 2…

A: 2 Al + 6 HCl ==> 2 AlCl3 + 3 H2

Q: How many grams of H₂O are formed when 89.6 g of Si₂H6 reacts with excess O2 in the following…

A: O2 present in excess while Si2H6 is limiting reagents.

Q: 9.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Given data 9.00g of a certain Compound X molecular molar mass of 60.g/mol Co2=13.20g water=5.40g…

Q: carbon monoxide (g) + oxygen (g) carbon dioxide (g

A: The limiting reagent is the reactant that is used up completely. The balanced chemical equation of…

Q: A chemist needs to add 3.5 moles NaClNaClto a reaction. How much NaCl should she measure out in…

A: Given: No. of mole of NaCl = 3.5 Molar mass of NaCl = 58.44g/mol Number of mole(n) = (mass of…

Q: Butane gas burns in oxygen to produce carbon dioxide, water and energy. If you have 10 liters of…

Q: 4. A mixture of glucose and oxygen reacts in aeroblo respiration. The right-hand box below shows a…

A: The given reaction is, C6H12O6 + O2 → CO2 + H2O + O2

Q: Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution…

Q: A major component of gasoline is octane (C8H18). When octane is burned in air, it chemically reacts…

A: In this question we have to explain that what mass of oxygen is consumed by reaction of 8.24 g of…

Q: How many grams of NH3 will be required to react with 32.7 grams of pbo based on the balanced…

Q: Given the reaction of 4 g of CaCN2 and 4 g of H20 forming CaCO3 and NH3, determine the mass (in g)…

Q: Consider the following unbalanced reaction: P4 + O2 → P4O6 If 3.28 g of P4 is reacted with 9.55 g of…

A: Applying concept of limiting reagent and reaction of inorganic chemistry.

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

42.9 g of Aluminum nitrite and 97.2 g of ammonium chloride react to form aluminum chloride,
nitrogen, and water. How many grams of the excess reagent remain after the reaction? Enter
to 1 decimal place.

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: Determine the given values

VIEW

Step 2: Determination of mass of excess reagent left after the reaction

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.
ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.
In a blast furnace at high temperature, iron(III) oxide in ore reacts with carbon monoxide to produce metallic iron and carbon dioxide. The liquid iron produced is cooled and weighed. The reaction is run repeatedly with the same initial mass of iron(III) oxide, 19.0 g, but differing initial masses of carbon monoxide. The masses of iron obtained arc shown in this graph. (a) Write the balanced chemical equation for this reaction. (b) Calculate the mass of CO required to react completely with 19.0 g iron(III) oxide. (c) Calculate the mass of carbon dioxide produced when the reaction converts 10.0 g iron(III) oxide completely to products. (d) From the graph, determine which reactant is limiting when less than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (e) From the graph, determine which reactant is limiting when more than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (f) Calculate the percent yield if 24.0 g iron(III) oxide reacted with 20.0 g carbon monoxide to produce 15.9 g metallic iron. (g) Calculate the minimum mass of additional limiting reactant required to react with all of the excess of nonlimiting reactant from part (f).
One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.
please make sure the answer has the correct number of significant digits
For the following reaction, 28.8 grams of sulfur dioxide are allowed to react with 6.14 grams of oxygen gas . sulfur dioxide ( g ) + oxygen ( g ) → sulfur trioxide ( g ) What is the maximum amount of sulfur trioxide that can be formed?|| grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams Submit Answer Retry Entire Group 4 more group attempts remaining
Given the reaction of 4 g of CaCN2 and 4 g of H2O forming CaCO3 and NH3, determine the mass (in g) of the excess reactant that is left after a complete reaction. Write the final answer with 3 decimal places and correct units.
Aluminum carbide reacts with water to form aluminum hydroxide and methane. If 3.30 g of aluminumcarbide is reacted with 3.60 g of water, how many grams of the excess reagent will be left after the reactionis complete?
9.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 60./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 13.20g water 5.40g Use this information to find the molecular formula of X.
[Review Topics] [References] Use the References to access important values if needed for this question. For the following reaction, 15.9 grams of nitrogen monoxide are allowed to react with 6.06 grams of oxygen gas. L nitrogen monoxide(g) + oxygen (g) nitrogen dioxide(g) What is the maximum amount of nitrogen dioxide that can be formed? g What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? g Submit Answer Retry Entire Group 8 more group attempts remaining Previous