2.) Striking a match stick on the matchbox involves thereaction of potassium chlorate and red phosphorus withthe following equation:10 KCIO3 (s) +3 Р4(s) ---> 3 РАО10 (s) + 1О КСІ (5)(A) How much reactant (KCIO3) will be needed to produce105.8 g of P4010?(B) How much reactant (P4) will be needed to produce 105.8g of P4010?Molar Masses:1 mole of KCIO3 = 122.55 grams of KCIO3%3D1 mole of P4 = 123.88 grams of P4%3D1 mole of P4010 = 283.88 grams of P4010Ratio:10 mole of KCIO3 = 3 mole of P40103 mole of P4 = 3 mole of P4O10

Stoichiometry gives the relationship between the amount of reactants and products in a balanced…

2.) Striking a match stick on the matchbox involves the reaction of potassium chlorate and red phosphorus with the following equation: 10 KCIO3 (s) + 3 P4 (s) ---> 3 P4O10 (s) + 10 KCI (s) (A) How much reactant (KCIO3) will be needed to produce 105.8 g of P4O10? (B) How much reactant (P4) will be needed to produce 105. g of P4010? Molar Masses: 1 mole of KCIO3 = 122.55 grams of KCIO3 1 mole of P4 = 123.88 grams of P4 1 mole of P4O10 = 283.88 grams of P4010 Ratio: 10 mole of KCIO3 = 3 mole of P4010 3 mole of P4 = 3 mole of P4010

2.) Striking a match stick on the matchbox involves the reaction of potassium chlorate and red phosphorus with the following equation: 10 KCIO3 (s) + 3 P4 (s) ---> 3 P4O10 (s) + 10 KCI (s) (A) How much reactant (KCIO3) will be needed to produce 105.8 g of P4O10? (B) How much reactant (P4) will be needed to produce 105. g of P4010? Molar Masses: 1 mole of KCIO3 = 122.55 grams of KCIO3 1 mole of P4 = 123.88 grams of P4 1 mole of P4O10 = 283.88 grams of P4010 Ratio: 10 mole of KCIO3 = 3 mole of P4010 3 mole of P4 = 3 mole of P4010

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: The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In…

Q: Consider the generic chemical equation:A + 3 B------->C

A: "Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: Ozone, O3 is formed in vehicle exhaust by the reaction NO2(g) + O2(g) —-> NO(g) + O3(g). What is the…

A: Given:mass of NO2 =2.0gAlso we know,Molar mass of NO2 = 46gMolar mass of O3= 48g

Q: Reactant and Theoretical Yield; Read Section 4.4. You can click on the Review link to access the…

Q: The reaction for producing glucose in plants, called photosynthesis, is 6CO2+6H2O−→−−light…

A: 6CO2 +6H2O −→ light + C6H12O6 + 6O2 Number of moles of C6H12O6 produced = 7.01 mol

Q: how many grams of water will be formed

A: Given :- mass of Fe2O3 = 27.2 g To calculate :- mass of H2O (in g)

Q: An organic liquid is either methyl alcohol (CH3OH), ethyl alcohol (CH3CH2OH) o a mixture of the two.…

A: The combustion reaction of methyl alcohol and ethyl alcohol:

Q: Balance each reaction, then suppose exactly 13.3 g of each reactant is taken. Indicate which…

A: Dear student since you have posted multiple questions we will solve the first question for you if…

Q: Arsenic reacts with oxygen according to the following equation: 4 As (s) + 3 O2 (g) → 2 As2O3 (s)…

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: This question will walk you through the steps of determining which reactant is limiting based on a…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the…

Q: If a reaction vessel initially contains 9 mol A and 8 mol B,how many moles of A, B, and C will be in…

A: The reactant which is completely consumed in a chemical reaction and limits the product formation is…

Q: The combustion of propane may be described by the chemical equation C,H,(g) + 50,(g) → 3 CO,(g) + 4…

Q: Balance the following chemical equation Fe3O4(s) +H2(g)-----> Fe(s) +H2O(1)

Q: When hydrobromic acid reacts with chlorine, bromine and hydrochloric acid are obtained: 2 HBr (aq) +…

A: We have to calculate the theoretical yield and percentage yield.

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: 7 = 8. HE 9. 10. Br "Nice Snce₂ нзой B. Сег Alles O 25 -NH₂ major product only

A: The question is based on organic reactions. we need to identify the product formed and explain…

Q: A nail in a board is completely turned to rust. Oxygen has combined with the iron in the nail (4Fe +…

A: A limiting reagent is the one that is present in lesser amount and that limits the amount of product…

Q: Hydrobromic acid dissolves solid iron according to the followiaung reaction: Fe(s)+2HBr(aq)→…

A: The reaction of iron and hydrobromide is given by equation 1.So, from equation (1) one mole of iron…

Q: What mass of HCI, in grams, is required to react with 0.840 g of Al(OH)3? Al(OH)₂ (s) + 3HCl(aq) →…

Q: Aluminum metal reacts with bromine according to the following unbalanced equation: Al (s) + Br₂ (1)→…

A: 4. Recall the given unbalanced equation, Al s + Br2 l → AlBr3 sWant to…

Q: In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following…

A: Limiting reagent of a reaction is the compound which is completely consumed during the reaction. The…

Q: Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching…

A: Mass of phosphoric acid = 2.0 x 10 3 g

Q: The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In…

A: As per the given chemical reaction2 moles of MnCO3 yields 2 moles of MnO2. In the second reaction 3…

Q: Limestone (CaCO3) is used to rem heated to form lime (CaO), which 74.2% yield in the overall…

A: The reaction involved are., CaCO3 ---> CaO + CO2 CaO + SO2 ---> CaSO3 S + O2 --> SO2

Q: 29. Consider the unbalanced equation for the reaction of solid lead with silver nitrate: Pb(s) +…

Q: ead (II) ions can be removed from solution with KCl according to the reaction: Pb2+ (aq) + KCl (aq)…

A: Firat we would balance the given chemical reaction. Then to calculate limiting reagent, we would…

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: Which of the following compounds are trans-1-bromo-3-methylcyclohexane? A I and III B II and III C…

A: Thank you.

Q: Mercury can be obtained by reacting mercury(II) sulfide (show below) with calcium öxide. It you…

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

Q: 13. Consider the following reaction. CaCl2(aq) + 2AGNO3(aq) 2A9C((s) + Ca(NO3)2(aq) Suppose that you…

A: Given data/information Reaction : CaCl2 (aq) + 2 AgNO3 (aq) → 2 AgCl(s) + Ca(NO3)2 (aq)…

Q: Here is the organic chemical equation for the reaction of an inorganic compound B with a big organic…

Q: According to the following reaction, how many grams of water will be formed upon the complete…

A: The balanced reaction given is, 4 HCl (aq) + O2 (g) ------> 2 H2O (l) + 2 Cl2 (g) Given : Mass…

Q: The reaction for producing glucose in plants, called photosynthesis, is…

A: Given, moles of C6H12O6 = 9.76 molThe reaction for producing glucose in plants is: 6 CO2 + 6 H2O →…

Q: 2 C3H18 (1) + 25 O2 (g) --> 16 CO2 (g) + 18 H2O (g) determine the mass in grams of carbon dioxide…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

2.) Striking a match stick on the matchbox involves the
reaction of potassium chlorate and red phosphorus with
the following equation:
10 KCIO3 (s) +3 Р4(s) ---> 3 РАО10 (s) + 1О КСІ (5)
(A) How much reactant (KCIO3) will be needed to produce
105.8 g of P4010?
(B) How much reactant (P4) will be needed to produce 105.8
g of P4010?
Molar Masses:
1 mole of KCIO3 = 122.55 grams of KCIO3
%3D
1 mole of P4 = 123.88 grams of P4
%3D
1 mole of P4010 = 283.88 grams of P4010
Ratio:
10 mole of KCIO3 = 3 mole of P4010
3 mole of P4 = 3 mole of P4O10

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

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 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

If 35g of LiCl mixes with 25g of Ca(OH)2, (a) which is the limiting reactant? (b) what is the theoretical yield? LiCl + Ca(OH)2 → LiOH + CaCl2
Book Print Limestone (CaCO3) is used to remove acidic pollutants from gases inside smokestack flues. It is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 78.1% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 9.3 x 104 kg of coal that is 0.49 mass % sulfur? x 10 g Caco3
11)
Black smokers are found in the depths of the oceans. Thinking that the conditions in these smokers might be conducive to the formation of organic compounds, two chemists in Germany found the following reaction could occur in similar conditions. 2 CH, SH + CO - CH, COSCH, + H;S If you begin with 14.0 g of CH, SH and excoss CO, what is the theoretical yield of CH, COSCH, ?. 9 CH;COSCH, If you isolate 6.40g of CH, COSCH, what is the percent yleld of CH, COSCH, ?
7) The reaction HNO3(aq) + NaOH(aq) NaN03(aq) + H2O() is an example of A) an acid-base reaction B) a precipitation reaction C) a combustion reaction 8) Which is the correct balanced reaction for the combustion of octane? A) C8H18(g) + 12.502(g) → 8CO2(g) + 9H2O(g) B) C8H18(g) + 250(g) → 8CO2(g) + 9H2O(g) C) 2C8H18(g) + 2502(g) → 16CO2(g) + 18H2O(g)
6.) What is the maximum mass of H20 that Can be produced by Combining 66.4g of each reactant. 4NH3 (g) + 5O₂ (g) → 4NO(g) + 6 H ₂ O (g)
The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo
In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compounds in the equation are as follows; PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol What is the limiting reagent in this scenario? Your answer should be an explanation! You're not solving anything. Note! Make an accurate claim: The limiting reagent in this scenario is _____. Provide additional details and use subject specific language. Cite evidence from what's given to you in the problem that supports your answer, hint: look at that equation!. Lastly! Fully connect the evidence to the claim/your answer to the question. Include subject specific language in your reasoning. The two images attached are examples of how your response SHOULD look.
1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? c) Which of the reactants is the limiting reagent? Justify your answer. d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction? f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container? please answer d, e and f
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. (c) NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l)limiting reagent? NaOHCO2 Na2CO3 produced g H2O produced g
In the reaction CrCl3 (aq) + 3 AgNO3 (aq) --> Cr(NO3)3 (aq) + 3 AgCI (s) 4.4 moles of CrClą are reacted with 1 moles of AgNO3. Determine the theoretical yield in mols of the product, silver chloride.
Balance and complete the following combustion reaction. Give the sum (one number only) t e t r a c a r b o n h e x a h y d r i d e ( g ) + o x y g e n ( g ) ⟶ ?