How many moles of MnOs are produced when 4.30 kg of oxygen gas completely reacts according to the balanced chemical reaction: 2 Mn(s) + 3 0:(g) - 2 MnO:(s)
Q: When 6.8 g al Aluminum reacts with excess oxygen according to the following balanced equation and…
A: Aluminium reacts with oxygen to form aluminium oxide as per the reaction, => Al (s) + O2 (g)…
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Q: The formation of aluminum chloride can be described by the balanced chemical equation. 2 Al + 3 Cl,…
A: Balanced equations: 2Al + 3Cl2 -----> 2AlCl3 Number of moles of Cl2 = (3 x number of moles of…
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Q: he number of moles of oxygen gas needed to react with 4.0 moles of Mg is
A: We have to apply general maths
Q: Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The unbalanced…
A: Given: Mg(s)+O2→MgO(s) Mass of Mg=10.1 gMass of O2=10.5 gMass of MgO=11.9 g To determine: Limiting…
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A: Dear student , since you have posted multiple questions we are allowed to solve only first question…
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A: Given, mass of H2 = 11.3 g we know, molar mass of H2 = 2.016 g/mol molar mass of HI = 127.911 g/mol…
Q: How many grams of oxygen gas are produced when 2.43 x 10-g of KCIO: are completely reacted according…
A: Stoichiometry involves the calculation of concentration of solutions in the given conditions of…
Q: How many moles of MnO, are produced when 4.30 kg of oxygen gas completely reacts according to the…
A:
Q: How many moles of MnO₃are produced when 4.30 kg of oxygen gas completely reacts with according to…
A: We have to find the moles of MnO3 produced in a balanced chemical reaction.
Q: Consider the following reaction at STP: 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g) 11. Determine the…
A: actual amount of products formed from Balanced chemical equation is known as theoretical yield.
Q: Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write a…
A: The chemical formula of Aluminium suffide=AL2S3The chemical formula of water=H2OThe chemical…
Q: Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum…
A: The reaction between MnO2 and Al –metal is shown as: Here, MnO2 and Al react in 3:4 ratio. Given…
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A: The chemical equation for given reaction is as follows,
Q: if 6.7x10^25 molecules of co2 are produced in a combustion reaction how many liters of co2 is…
A: Since moles = number of molecules / Avogadro's number Avogadro's number = 6.022 X 1023 => moles…
Q: 7.0 mol of NO and 5.0 mol of O2 are reacted together. The reaction generates 3.0 mol of NO2. What is…
A: Given that the moles of NO and O2 are 7.0 mol and 5.0 mol respectively. The reaction of yields…
Q: limiting reactant
A:
Q: Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into…
A: NH4NO3(s) → N2(g) + O2(g) + H2O(g) Mass of ammonium nitrate = 1.29 g To calculate the mass of…
Q: How many moles of MnO3 are produced when 4.30 g of oxygen gas completely reacts according to the…
A: Given data: The amount of oxygen gas reacted is = 4.30 g Molar mass of O2 is = 32.00 g
Q: How many moles of MnO₃ are produced when 4.30 kg of oxygen gas completely reacts…
A: moles of reactant reacting / coefficient of that reactant in reaction = moles of product forming /…
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A: Chemical Reaction :- 2C₄H₁₀ (g) + 13O₂ (g) → 8CO₂ (g) + 10H₂O (g) O2 is excess reagent. So, C4H10…
Q: identify the limiting reactant, and calculate the theoretical yield. c) If 3.52 g of Cisplatin is…
A: Number of moles = mass / molar mass Percent yield = (actual yield/theoritical yield) x 100
Q: Given the balanced equation representing a reaction: F2(g) + H2(g) ? 2HF(g) What is the mole ratio…
A:
Q: How many moles of MnO, are produced when 4.30 kg of oxygen gas completely reacts according to the…
A: Step : 1 The required answer for the above question is follows as :
Q: How many moles of MnO3 are produced when 4.30 kg of oxygen gas completely reacts according to the…
A: Balanced chemical equation: 2Mn (s) + 3O2 (g) -----> 2MnO3 (s) Number moles of MnO3 = (2 x…
Q: Aluminum sulfide reacts with water to form aluminumhydroxide and hydrogen sulfide. (a) Write the…
A: a. The balanced chemical equation of the above process is as follows : Al2S3 + 6H2O ------------>…
Q: The (fictitious) element Unobtainium can be easily oxidized by oxygen gas to produce Unobtainium…
A: Given data contains, Moles of oxygen inside the reaction vessel is 10.9 mol. The given chemical…
Q: How many moles of MnO3 are produced when 4.30 kg of oxygen gas completely reacts according to the…
A: The moles of the product formed from a specified amount of reactant can be obtained by looking at…
Q: How many grams of sodium sulfate are produced when 15 moles of copper sulfate are used? 2NaOH +…
A: Given chemical equation is : 2NaOH + CuSO4 → Cu(OH)2 + Na2SO4Sodium…
Q: How many moles of MnO, are produced when 4.30 kg of oxygen gas completely reacts according to the…
A: Given, the balanced chemical reaction as follows,2 Mn(s)+3O2 →2 MnO2(s)amount of oxygen gas (O2) for…
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A: Ag2O + 2HCl = 2AgCl + H2O Molar mass of ; Ag2O : 107.87×2 + 16 = 231.7 g/mol HCl : 1 + 35.45 =…
Q: What mass of magnesium chloride is produced from the reaction of 20.7 g of Mg? Balance the equation:…
A: This can be done as
Q: How many grams of barium sulfate are produced if 25.34mL of o.113M BaCl, completely react given the…
A: Balanced Equation BaCl2 (aq) + Na2SO4(aq) → BaSO4 (s) + 2NaCl (aq) From above, clearly 1 mol BaCl2…
Q: How many grams of oxygen gas are produced when 2.43 x 10 g of KCIO, are completely reacted according…
A: Given: Mass of KClO3 reacted = 2.43 x 10-4 g The balanced chemical equation of the reaction is given…
Q: How many moles are produced when 4.30 kg of oxygen gas completely reacts according to the balanced…
A: The reaction given is 2 Mn (s) + 3 O2 (g) ------------> 2 MnO3 (s) Given : mass of oxygen…
Q: For the following balanced reaction: 2H2 + O2 = 2 H2O How many grams of H2O (Molar mass: 18g/mol)…
A: For the following balanced reaction: 2H2 + O2 = 2 H2O
Q: A sample of 108.2 g of Calcium oxide was obtained by heating 258 g of calcium carbonate. What is the…
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A:
Q: If ammonia can be produced from calcium oxide and ammonium chloride according to the following…
A: Ammonia can be produced from calcium oxide and ammonium chlorideaccording to the following…
Q: What mass in grams of oxygen gas are produced when 2.43 x 10g of KCIO, are completely reacted…
A:
Q: How many grams of magnesium oxide (MgO) are created when 25.0 grams of magnesium (Mg) react with…
A: The chemcal reaction is 2 Mg + O2 = 2 MgO. Hence, 2 moles of Mg reacts with 1 mole of O2 to produce…
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A:
Q: How many moles of nitrogen gas would be produced if 7.19 moles of copper(II) oxide were reacted with…
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Q: 1. In a reaction, 50.0g of manganese (IV) oxide reacts with 25.0g of aluminum. Identify the limiting…
A: Given data,Mass of MnO2=50gMass of Al=25.0g Balance chemical equation: 3MnO2+4Al→2Al2O3+3Mn
Q: According to the following balanced reaction how many moles of NO are formed from 8.44 moles of NO2…
A: Given, Moles of NO2 = 8.44 mol The balanced reaction is given as : 3 NO2 (g) + H2O → 2 HNO3 (aq) +…
Q: How many moles of nitrogen gas would be produced if 4.08 moles of copper II ) oxide were reacted…
A: Moles of copper oxide= 4.08mole
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A: According to the given balanced chemical equation, 2 moles of HgO reacts to produce exactly 1 mole…
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- A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.4.90 Iron metal can be refined (rom the mineral hematite (Fe2O3). One way of converting the mineral to iron is to react it with carbon monoxide, as shown below: Fe2O3+3CO2Fe+3CO2 Because the hematite is obtained from various ores, it is usually not in a pure form. Suppose an iron manufacturer has 2.00 X 105 kg of ore available, and the ore is 93% Fe2O3 by mass. (There is no iron in the remaining 7% of the ore.) How many moles of Fe2O3are present in this ore? How many kg of pure iron could be obtained from this sample of ore? Assume that the process has a 100% yield and that excess CO is available.A Boron and hydrogen form an extensive family of compounds, and the diagram below shows how they are related by reaction. The following table gives the weight percent of boron in each of the compounds. Derive the empirical and molecular formulas of compounds A-E.
- When calcium carbonate is heated strongly, it evolves carbon dioxide gas. CaCO3(s)CaO(s)+CO2(g) 25 g of CaCO3 is heated, what mass of CO2would be produced? What volume would this quantity of CO2 (CU at STP?When solid silicon tetrachloride reacts with water, solid silicon dioxide and hydrogen chloride gas are formed. (a) Write a balanced equation for the reaction. (b) In an experiment, 45.00 g of silicon tetrachloride are treated with 45.00 mL of water (d=1.00g/mL). What is the theoretical yield of HCI (in grams)? (c) When the reaction is complete, 17.8 L of HCl gas (d=1.49g/L at the conditions of the experiment) are obtained. What is the percent yield? (d) How much of the reactant in excess is unused?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.
- 4.17 Phosgene is a highly toxic gas that has been used as a chemical weapon at times in the past. It is now used in the manufacture of polycarbonates, which are used to make phone cases and plastic eyeglass lenses. Phosgene is produced by the reaction, CO+Cl2COCl2 . Given an excess of carbon monoxide, what mass of chlorine gas must be reacted to form 4.5 g of phosgene?Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
- When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?4.21 Ammonium nitrate, NH4NO3, will decompose explosively to form N2, O2, and H2O, a fact that has been exploited in terrorist bombings. What mass of nitrogen is formed by the decomposition of 2.6 kg of ammonium nitrate?How many grams of oxygen gas are produced when 2.43 × 10⁻⁴ g of KClO₃ are completely reacted according to the following chemical equation: 2KClO₃(s)→2KCl(s)+3O₂(g)