For the unbalanced equation, Al + O_2 \to Al_2O_3, a) If 21.0 moles of oxygen gas react, how...
Question:
For the unbalanced equation, {eq}Al + O_2 \to Al_2O_3, {/eq}
a) If {eq}21.0 {/eq} moles of oxygen gas react, how many moles of aluminum will react with this oxygen?
b) If we use {eq}3.0 {/eq} grams of aluminum, how many grams of aluminum oxide will be produced when enough oxygen gas is present?
Stoichiometric Ratio:
Stoichiometry ratio is used to determine the amount of one chemical species, either product or reactant, relative to the amount of other chemical species. The stoichiometric ratio is simply the theoretical ratio of chemical species based on balance chemical reaction.
Answer and Explanation:
Become a Study.com member to unlock this answer! Create your account
View this answer
To calculate the (a) moles of aluminium that will react with oxygen, and (b) the mass of aluminium oxide generated, the reaction must first be...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Stoichiometry: Calculating Relative Quantities in a Gas or Solution
from
Chapter 9 / Lesson 4
30K
Learn how to find the molarity of a solution or the moles of gas in a given volume using stoichiometry. See examples of calculating moles from molarity.
Related to this Question
- How many moles of Al will be consumed when 0.400 moles of Al_{2}O_{3} are produced in the following equation?
- Calculate the mass of Al2O3 formed when 4.7 grams of aluminum completely reacts with excess oxygen. Al + O2 arrow Al2O3
- What is the mass of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with enough amount of carbon according to the following chemical reaction? Al_2O_3 + 3 C \rightarrow 2 Al
- In the following reaction, 35.6 grams of Al was given to react with 39.4 grams of O2. How many grams of Al2O3 will be produced? 4Al(s) + 3O2(g) arrow 2Al2O3(s)
- Given the equation 3BaO+2Al=3Ba+Al_2O_3, what is the mole ratio of Aluminum to Aluminum Oxide? How many moles of Barium will be produced from 5.25 moles of Aluminum?
- Calculate the mass of Al_2O_3 that can be produced if the reaction of 55.1 g of aluminum and sufficient oxygen has a 80.0% yield. Express your answer with the appropriate units.
- How many moles of oxygen are produced when 8 moles of AL are produced?
- What is the sum of all the stoichiometric coefficients in the balanced chemical equation for the reaction of aluminium with platinum (IV) nitrate where platinum solid and aluminium nitrate are produced? a. 16 b. 14 c. 13 d. 12 e. 15 f. 11 g. 10
- What is the theoretical yield in grams of aluminum oxide when 40.0 g of aluminum react with 50.5 g of oxygen gas?
- The molten metal reaction below begins with 27.0 g of manganese (IV) oxide (86.94 g/mol) and 11.6 g of aluminum (26.98 g/mol). Convert these quantities to moles and use the stoichiometric ratios (from the coefficients) to determine which reactant is limit
- Calculate the mass of aluminum oxide (Al 2 O 3 ) produced if 25.00 g of Aluminum (Al) is reacted completely.
- A thermite reaction occurs between solid aluminum and iron III oxide (rust) to form molten iron metal and aluminum oxide. 2 Al (s) + Fe2O3 (s) → 2Fe (l) + Al2O3 (s) How many grams of iron are produced for every 1.50 moles of iron III oxide tha
- Which substance is in excess when 6.00 moles of aluminum are reacted with 12.00 moles of oxygen
- Aluminum reacts with chlorine gas according to the following equation shown below. How many moles of C l 2 are required to react with 0.081 mol of A l ? 2 A l ( s ) + 3 C l 2 ( g ) 2 A l C l 3 ( s )
- Consider the unbalanced equation below. Cu + O_2 \to CuO If 101 grams of copper are used, how many moles of copper (II) oxide will be formed?
- In this reaction, 0.35 moles of oxygen are mixed with 0.500 moles of phosphorous. How many moles of phosphorous(III) oxide form? 4P(s) + 3O2(g) arrow 2P2O3(s)
- What is the total number of grams of O2(g) needed to react completely with 0.50 moles of C2H2(g) for the balanced equation below? 2C2H2(g) + 5O2(g) arrow 4CO2(g) + 2H2O(g)
- Balance the chemical equation. Al2O3 + Fe --%3E Fe3O4 +Al
- Balance the equation below and answer the question. Fe + O2 arrow Fe2O3 How many grams of Fe2O3 are produced when 2.93 x 1011 molecules of O2 are reacted?
- Write balanced equations for the following reaction: molten aluminum oxide is decomposed into its elements by electrolysis.
- In the following stoichiometry problem, How does 4.5 moles of H2O cancel out 2 moles of H20 once the problem is set up? How many moles of O2 is used when 4.5 moles of water is produced according to t
- How many moles of O_2 are produced from 0.177 moles KClO_3 according to the reaction below Hint: must balance the reaction \rule{0.5cm}{0.1mm}\ KClO_3 (s) \rightarrow\ \rule{0.5cm}{0.1mm}\ KCl (s) +\ \rule{0.5cm}{0.1mm}\ O_2 (s)
- In the aluminothermic reaction between Manganese and Aluminium. Find the redox reaction between MnO2 and Al using stoichiometry, and calculate the molar mass ratio of the reaction.
- For decomposition chemistry, predict the products for the following decomposition reaction. Write the complete balanced molecular equation for the reaction. Aluminum chlorate is strongly heated with a catalyst.
- For the following balanced equation, indicate how many moles and grams of each reactant and product are needed/produced in the reaction if 10.0 grams of FeS2 reacts. 4FeS2 + 11O2 arrow 2Fe2O3 + 8SO2
- Aluminum carbide is a solid that reacts with water to form aluminum hydroxide and methane gas. The reaction can be represented by the following chemical equation. Al4C3(s) + 12H2O(l) arrow 4Al(OH)3(s) + 3CH4(g) If 0.327 moles of Al4C3 completely reacts wi
- In the following balanced chemical equation, how many atoms (total) of oxygen are found on the reactant side?
- Consider the reaction 4Al + 3MnO2 rightarrow 3Mn + 2Al2O3. If 22 grams of Al react with 13 grams of manganese(IV) oxide, how much excess reactant remains after the reaction has run to completion?
- According to the following reaction, how many moles of mercury will be formed upon the complete reaction of 23.2 grams of mercury(II) oxide? 2HgO(s) \to 2Hg(l) + O2(g)
- For the balanced equation shown below, if 7.15 grams of P4 were reacted with 16.6 grams of O2, how many grams of P4O10 would be produced? P4 + 5O2 P4O10
- If 5 moles of hydrogen gas and 5 moles of oxygen react what is the limiting reactant? How many moles of water are formed?
- Explain the need for coefficients when balancing the following reaction. Al + Fe2O3 arrow Fe + Al2O3
- For the reaction represented by the equation 2H2 + O2 --> 2H2Oo, what is the mole ratio of H2 to H2O?
- For the reaction 2S (s) + 3O_2 (g) to 2SO_3 (g) If 6.3 g of S is reacted with 10.0 g of O_2, which one will be the limiting reactant?
- Consider the reaction where aluminum (Al) reacts with chlorine (Cl_{2}) to form aluminum chloride (AlCl_{3}). What is the number of chlorine molecules needed so that 1 mole of aluminum will be consumed by the reaction? a. Avogadro's number b. Half of Av
- For the following reaction, calculate how many moles of each product are formed when 0.356 moles of PbS completely reacts. Assume there is an excess of oxygen. 2PbS(s) + 3O2(g) arrow 2PbO(s) + 2SO2(g)
- What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? C2H6O(l) + O2(g) arrow CO2(g) + H2O(g)
- Aluminum reacts with Hydrochloric acid to produce hydrogen gas and aluminum chloride salt. a. Formula for aluminum chloride: AlCl_3. Meaning we need one mole of Aluminum and 3 moles of Chloride to form Aluminum chloride. b. Equation of the reaction: 2Al
- Given the equation 2Mg + O2 --> 2MgO, how many moles of MgO are produced for every mole of O2 used up?
- How many grams of O2 are needed to produce 0.400 mole of Fe2O3?
- 2NO(g) + O2(g) arrow 2NO2(g) You are provided with 3.88 mol of nitrogen monoxide gas. Using the balanced chemical equation, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen
- How many moles of oxygen gas react to yield 0.100 mol of water?
- 2KClO_3 to 2KCl + 3O_2. How many moles of O_2 are produced when 4.0 moles of KCl are produced?
- In the reaction given below, for every two moles of iron(III) oxide consumed, how many moles of iron are produced? 2 Fe2O3 4 Fe + 3 O2
- Using the equation 4fe + 3O2 2Fe2O3, if 6 moles of oxygen and an excess of iron were available, how many moles of iron (III) oxide would be produced?
- In using the thermite reaction, 144 grams of Al are reacted with 155 grams of iron (lll) oxide. How much of excess reagent is left at the end of the reaction?
- If the molten metal reaction below begins with 25.0 grams of manganese(IV) oxide and 10.0 grams of aluminum, determine which reactant is limiting. Then determine the mass of aluminum used and the mass of manganese created. 3MnO2 + 4Al arrow 3Mn + 2Al2O3
- How many moles are in 16 grams of oxygen?
- a) Write a balanced equation for the reaction of tin (IV) phosphate with sodium carbonate to make tin (IV) carbonate and sodium phosphate. b) If 36 grams of tin (IV) phosphate is mixed with 7.3 grams of sodium carbonate, how many grams of tin (IV) carbona
- Calculate the mass in grams of aluminum iodide(AlI_3) when 22.20 g of aluminum (Al) reacted completely with iodine (I_2) according to this equation: 2Al + 3I_2 \to 2AlI_3. a. 167.7 g \\b. 335.4 g \\c. 456.7 g \\d. 313.0 g
- Suppose 7 grams of aluminum metal is reacted with 11 grams of hydrogen sulfate and produces 3.4 grams of aluminum sulfate and hydrogen gas. Calculate the percent yield of this reaction.
- Reaction: Aluminum chloride is mixed with Hydrogen gas to produce Hydrochloric acid and Aluminum metal. If you are given 5 grams of Hydrogen and 50 grams of Aluminum chloride, how many grams of Aluminum can be produced if the reaction is 35% efficient? a.
- Consider the following reaction: 4 PH3 + 8 O2 to P4O10 + 6 H2O a. How many grams of PH3 are required to react with 100 g of O2? b. How many grams of P4O10 are produced when 100 g of O2 react? c. How many moles of water are produced when 100 g of O2 react?
- Given 14.0 g of O2, how many grams of the product Cr2O3 could be produced?
- How many moles of magnesium oxide are produced by the reaction of 1.82 g of magnesium nitride with of 17.73 g of water? Mg_3N_2 + 3H_2O \to 2NH_3 + 3MgO
- In the reaction: 2KClO3(s) 2KCl(s) + 3O2(g), what mass of potassium chlorate, KClO3, would be required to produce 957 L of oxygen, O2, measured at STP?
- Using the following reaction: C5H12 + O2 right arrow CO2 + H2O; answer the questions below. a) Balance the equation. b) How many moles of oxygen are needed to react with 4.25 moles of C5H12? c) How many grams of water can be produced from 6.18 moles of
- Use the following equation: 4Fe(g) + 3O_2 (g) \to 2Fe_2O_3(s) If 32 moles of Fe and 27 moles of O_2 are reacted, which is the limiting reagent?
- 6.32 g of potassium chlorate reacts according to the following incorrectly balanced reaction. (Make sure to properly balance the equation before completing your calculations.) 2 KClO3(s) 2 KCl(s) + O2(g) Determine the quantity of oxygen produced by the re
- How many moles of carbon dioxide are produced when 3.00 mol of oxygen react completely in the following equation? C_3H_8 + 5 O_2 rightarrow 3 CO_2 + 4 H_2O
- When 14.387 g of aluminum (26.982 g/mol) are reacted with 127.657 g of copper(II) sulfate (159.609 g/mol), solid copper and aluminum sulfate are formed. Which reactant(s) is/are the limiting reactant(s)? a) Copper is the limiting reactant. b) Aluminum i
- A solid piece of aluminum is reacted with hydrochloric acid. How many moles of aluminum are required to react with 283 mL of 2.3 mol/L hydrochloric acid?
- 15.00 g Al2S3 and 10.00 g H2O react until the limiting reagent is used up. The equation for the reaction is: Al2S3 (s) + H2O (l) to Al(OH)3 (s) + H2S (g). (A) Give a balanced equation for the reaction. (B) Which is the limiting reagent? Show your calculat
- Calculate the limiting reactant if 1.50 mol Fe_2O_3 reacts with 2.50 mol Al
- How many moles of O2 are needed to react completely with 4.80 mol of C2H2?
- Consider the following balance equation: 2Fe_2O_3 + 3S \to 3SO_2 + 4Fe. How many moles of sulfur dioxide are made if 12 moles of iron III oxide are used?
- Unbalanced reaction: Fe + O_{2} \rightarrow FE_{2}O_{3}. \Delta H = -1652 kJ a. How much heat is involved when 100. g of iron reacts? b. How much heat is involved when 100. g of Fe_{2}O_{3} is produced? c. How many grams of oxygen did you start with when
- Find the number of moles of oxygen that will react with 5.00 grams of butane. C4H10 + O2 arrow CO2 + H2O
- Consider the equation: 2H2O(l) 2H2(g) + O2(g) If 9 g of H2O decomposes according to the reaction shown above, how many moles of hydrogen gas are produced? a) 0.5 mol b) 1 mol c) 2 mol d) 4 mol
- Suppose the reaction occurs at RTP. How many cm^3 of chlorine would be needed to react with 25 grams of aluminium?
- What are coefficients in stoichiometry?
- How many moles of HCl are produced when 75.1 grams of AlCl3 reacts with excess H2SO4? 2AlCl3 + 3H2SO4 arrow Al2(SO4)3 + 6HCl
- How many moles of ethane (C2H6) would be needed to react with 62.3 grams of oxygen gas?
- Calculate the theoretical yield of AlCl3 when 15.0 g of Al reacts with 55.0 g of Cl2 in the reaction below. 2 Al (s) + 3 Cl2 (g) arrow 2 AlCl3 (s).
- How many moles of magnesium oxide are produced by the reaction of 1.82 g of magnesium nitride with 17.73 g of water?
- H2(g) + O2(g) arrow H2O(g) 1) How many moles are needed of oxygen to completely react with 6.02 grams of hydrogen? 2) How much water is produced if we have 502 grams of oxygen with plenty of hydrogen? 3) If 24.3 moles of water was produced, how many gram
- Niobium is element 41. It can be obtained from its oxides by reaction with aluminum. For example: 3Nb_2O_5(s) + Al(s) 6Nb(s) + 5Al_2O_3(s) For each 10.0 grams of niobium(V) oxide that reacts, what mass, in grams, of aluminum oxide is formed?
- If 500g of aluminum reacted with an excess of sulfuric acid, how many liters of H2 at STP would be produced in this reaction? 2Al(s)+3H2SO4(aq) \to Al2(SO4)3(aq)+3H2(g)
- For the following balanced chemical equation, calculate the number of moles of products that would be produced if 0.628 mol of the first reactant would react completely. CO2 + 4 H2 -------> CH4 + 2
- Consider the equation: A (g) + 3 B (g) to 4 C(g) If 3.0 moles of A is reacted with 6.0 moles of B, which of the following is true after the reaction is complete? O A is the leftover reactant because, for every 1 mole of A, 4 moles of C are produced. O A
- How many moles of aluminum sulfate, Al2(SO4)3, are there in 0.6076 grams of aluminum sulfate?
- If you are given 5 grams of Hydrogen and 50 grams of Aluminum chloride, how many grams of Aluminum can be produced if the reaction is 35% efficient?
- Consider the following reaction and answer the following questions. 2Mg + O2 arrow 2MgO a. How many moles of oxygen gas are needed to react with 12.3 moles of magnesium? b. How many moles of magnesium are needed to react with 30.2 grams of O2?
- Write and balance the chemical equation upon the combustion of sucrose. Determine the moles of H_2 O produced from the combustion of 5 moles of sucrose and 39 moles of oxygen? Which chemical is in excess and how many moles remain after the reaction is com
- What mass of iron(III) oxide would be required to produce 2250g of iron metal? How many moles of carbon monoxide would be used during this reaction?
- How many moles of oxygen gas is consumed in a hydrogen sulfide reaction that produces 295 g of SO_2?
- Aluminum hydroxide reacts with sulfuric acid to produce aluminum sulfate and water. How many grams of aluminum hydroxide are necessary to produce 108 grams of water?
- Given the reaction for the decomposition of hydrogen peroxide into water and oxygen, how many moles of water can be produced from 26.0 g of hydrogen peroxide?
- Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many liters of hydrogen gas would be formed if 25.0 g of H2SO4 completely reacted with aluminum? 2Al(s) + 3H2SO4(aq) arrow Al2(SO4)3(aq) + 3H2(g) a) 5.71 L b) 290 L c) 45
- _____NH_{3} + _____O_{2} \rightarrow _____N_{2} + _____H_{2}O a. 20 moles of NH_{3} are needed to produce _____ moles of H_{2}O. b, How many moles of N_{2} will be produced if 3.5 moles of O_{2} react?
- Silver nitrate and aluminum chloride react with each other by exchanging anions. 3AgNO3(aq) + AlCl3(aq) arrow Al(NO3)3(aq) + 3AgCl(s) What mass of precipitate is produced when 4.22 grams of silver nitrate reacts with 7.73 grams of aluminum chloride in sol
- Phosphorus and oxygen combine to form tetraphosphorus decoxide. a) Write a balanced reaction and determine the limiting reactant and the mass of P4O10 formed if 15.0g of P4 and 30.0g of O2 are used. b
- During a complete combustion of C_4H_8 How many moles of oxygen are consumed for every one mole of C_4H_8?
- 2H2(g) + O2(g) 2H2O(g) + Heat. If 25.0 grams of H2(g) is mixed with 197 grams of O2(g), how many grams of H2O(g) is produced? (The molar mass of hydrogen is 1.01 g/mol and oxygen is 16.00 g/mol)
- In the decomposition of 1.2 moles of dinitrogen pentaoxide, how many moles of oxygen would be formed?
- How many molecules of O2 are produced when 35.3 grams of KClO3 decomposes as shown in the reaction below? 2KClO3 arrow 2KCl + 3O2
- The equation for the decomposition of potassium chlorate is written as: 2KClO3(s) to 2KCl(s) + 3O2(g) When 48.2 g of KClO3 is completely decomposed, what is the theoretical yield, in grams, of O2?
- How many moles of CO_{2} are produced when 3.01 * 10^{23} molecules of C_{3}H_{6} react completely in the following equation? 2C_{3}H_{6} + 9O_{2} \rightarrow 6CO_{2} + 6H_{2}O
- A student in a chemistry lab mixes 13.8 g of aluminum sulfate with 2.04 g calcium hydroxide to produce aluminum hydroxide and calcium sulfate. The unbalanced reaction is: Al2(SO4)3 + Ca(OH)2 Al(OH)3+ CaSO4. a) Which reactant is limiting? b) What mass of a
- 2C6H6 + 15O2 arrow 12CO2 + 6H2O Suppose you have 2.92 g of C6H6 and 9.95 g of O2. What mass of the reactant is present in excess after the reaction is complete?
Explore our homework questions and answers library
Browse
by subject