If 10.0 moles of O: are reacted with excess NO in the reaction below, and only 5.5 mol of NO2 were collected, then what is the percent yield for the reaction? 2 NO (g) + O2 (g)→2 NO2 (g)
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.6 mol of NO₂ were…
A: Nitrogen monoxide reacts with oxygen to form nitrogen dioxide. The balanced equation is as follows:…
Q: Ammonia gas can be prepared by the reaction of a metal oxide such as calcium oxide with ammonium…
A: 1) Molar mass of CaO, MM = 1 x MM(Ca) + 1 x MM(O) = 1 x 40.08 + 1 x 16.0 = 56.08 g/mol…
Q: If 10 moles of o2 are reacted with excess no in the reaction below and only 6.4 mil of No2 were…
A: Percent yield: The percentage of ratio between actual and theoretical yield of a reaction.
Q: When HgO is heated, it decomposes into elemental mercury and molecular oxygen. If 10.0 g of Hg is…
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Q: When HgO is heated, it decomposes into elemental mercury and molecular oxygen. If 60.0 g of Hg is…
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Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…
A: According to the chemical equation, the number of moles of oxygen required to produced 13.0 mol of…
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.0 mol of NO₂ were…
A: Information given: Moles of oxygen = 10.0 mol Moles of NO2 formed = 4.0 mol
Q: a) What is the limiting reactant when 0.200 mol of P4 and 0.200 mol of O2 react according to the…
A: Stoichiometry of a reaction is important to determine the amount of reactant required or the amount…
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.5 mol of NO₂ were…
A:
Q: When HgO is heated, it decomposes into elemental mercury and moecular oxygen. If 60.0g og Hg is…
A: % Yield = 100 x Obtained mass/calculated mass
Q: what is the percent yield of the reaction of 3.75 g of NO are formed?
A: Number of moles = mass/molar mass Mass = moles × molar mass Percent yield = (actual…
Q: Sodium borohydride (NaBH4) is used industrially in many organic syntheses. One way to prepare it is…
A: Sodium borohydride is an inorganic compound which can be prepared by reacting sodium hydride with…
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 8.9 mol of NO₂ were…
A: The balanced chemical equation for the given reaction is, 2NOg+O2g→2NO2g The moles of oxygen are 10.…
Q: How many moles of nitrogen gas would be produced if 6.03 moles of copper(II) oxide were reacted with…
A: Stoichiometric calculation means the calculation of masses of reactant and product involved in a…
Q: What is the percent yield for the reaction?
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Q: How much is the excess reactants? if the given is Al(OH)3 If 10.0 g of Al2(SO3)3 is reacted with…
A: Answer :- The mass of excess reactants (NaOH) = 1.84 g…
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.4 mol of NO₂ were…
A: Use Mole- mole ralationahip Percent yield= actual×100÷theoritical yield
Q: If 10.0 moles of O2 are reacted with excess NO in the reaction below, and only 3.9 mol of NO2 were…
A: For the reaction: O2 (g)+ 2NO (g)→ 2NO2 (g) 1 mol 2 mol 2 mol Given moles of O2 =10 mol…
Q: 3. Use the balanced equation below to answer questions a-d. 4 NH + 3 Ozg) → 2 N2 + 6H2O@ a. How many…
A: a) Given, 4NH3(g) + 3O2(g) ➝ 2N2(g) + 6H2O(g) Moles of O2 are needed to react with 28.0g of NH3 =?…
Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…
A: Balanced chemical equation is as follows: It is given that 84.9% of the theoretical yield is equal…
Q: Silicon nitride (Si3N4) is made by combining Si and nitrogen gas at a high temperature. How much (in…
A: Answer is explained below.
Q: According to the reaction below you are supposed to produce 1 mol of SigN4 ,Silicon Nitride each…
A: Given, The reaction: 3Si(s) + 2N2(g) ---------> Si3N4(g) The produced moles of Si3N4 =0.743…
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.3 mol of NO₂ were…
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Q: how many grams of nitrogen dioxide will be formed
A: Balanced chemical equation: 2NO(g)+O2(g)= 2NO2(g)
Q: Sodium borohydride (NaBH4) is used industrially in many organic syntheses. One way to prepare it is…
A:
Q: If 10.0 moles of O_{2} are reacted with excess NO in the reaction below, and only 4.9 mol of N*O_{2}…
A: Given data: The moles of O2 reacted= 10.0 mole. The moles of NO2 obtained=4.9 mol. Given reaction: 2…
Q: Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for…
A: The reaction given is SO2(g) + 2 Cl2(g) → SOCl2(g) + Cl2O(g)
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.2 mol of NO₂ were…
A: The balanced chemical equation between nitrogen oxide and oxygen and its theoretical yield are…
Q: Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3NH3, according to the…
A: The reaction is written below. 3H2(g)+N2(g)→2NH3(g) According to the reaction, 3 moles of H2 reacts…
Q: Ammonia gas (NH3) reacts with hydrochlorix acid (HCl) to form ammonium chloride (NH4Cl). If 3.0 g of…
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Q: Question is attached herewith
A: The balanced reaction is: Ca3PO42 + 3 H2SO4 → 3 CaSO4 + 2 H3PO4 Moles of Ca3(PO4)2 = Mass/Molar mass…
Q: Quicklime, CaCO, and water can be produced by heating calcium hydroxide, Ca(OH) 2. What is the…
A: The balanced reaction taking place is given as, => Ca(OH)2 (s) -------> CaO (s) + H2O (l)…
Q: Calcium carbonate reacts with hydrochloric acid solution to form calcium chloride solution, water…
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Q: Given the following: 2 Ca (s)+ O2(g) -> 2 CaO (s) if 150. g of O2 react with 150. g of Ca 1) how…
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Q: When HgO is heated, it decomposes into elemental mercury and molecular oxygen. If 10.0 g of Hg is…
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Q: Calcium hypochlorite, Ca(OCl)2, is used as a bleaching agent. It is produced from sodium hydroxide,…
A: Limiting reagent is the reactant of the reaction which is present in limited amount and will…
Q: n the reaction below, 7.0 mol of NO and 5.0 mol of O₂ are reacted together. The reaction generates…
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Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.2 mol of NO₂ were…
A: GIVEN: Reaction: 2 NO (g) + O₂ (g) → 2 NO₂ (g) To Solve: percent yield for the reaction=?
Q: 3. Given the balanced equation: 2 H2 + CO ? CH;OH , how тапy moles of CH;OH will be produced if 12.6…
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Q: If 10.0 moles of O2 are reacted with excess NO in the reaction below, and only 7.0 mol of NO2 were…
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Q: How many moles of nitrogen gas would be produced if 3.24 moles of copper(II) oxide were reacted with…
A: The given reaction is: 2 NH₃(g) + 3 CuO (s) → 3 Cu(s) + N₂(g) + 3 H₂O(g)
Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…
A: To solve this problem first we calculate theoretical yield of NO2 Then we calculate the number of…
Q: According to the following balanced reaction, how many moles of CaOCaO are required to exactly react…
A: The amount of product formed in a chemical reaction depends upon the amount of limiting reactant and…
Q: If the percent yield for the following reaction is 75.0%, and 30.0 g of NO2 are consumed in the…
A: The balanced chemical reaction is given below. The number of moles of NO2 (g) consumed can be…
Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 8.7 mol of NO₂ were…
A: To calculate the percentage yield of the reaction the no. of moles of reactant and the molecular…
Q: Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high…
A: The balanced chemical reaction is 2NH3 + 3CuO → N2 + 3Cu + 3H2O First, we will have to identify the…
Q: If 10.0 moles of O, are reacted with excess NO in the reaction below, and only 7.6 mol of NO, were…
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Q: How many moles of nitrogen gas would be produced if 4.06 moles of copper(II) oxide were reacted with…
A: The law of conservation of mass Matter can change the form, but cannot be created or destroyed.…
Q: 5. When N2 and 5.00 g H2 are mixed, the reaction produces 16.0 g NH3. a) What is the percent yield…
A: 5) we have to calculate percentage yield and actual yield
Q: If 10.0 moles of O₂ are reacted
A: Given reaction is 2 NO (g) + O₂ (g) →…
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- Solve the 3 questions below 1. How many grams of the excess reagent are left over when 6.00 g of CS gas react with 10.0 g of Cl gas in the following reaction: CS2 (g) + 3 Cl2 (g) -> CCl4 (l) + S2 Cl2(l) 2. Given the following reaction: 2 Fe + 3 I2 → 2 FeI3, if 0.229 mol of iron (Fe) and 0.318 moles of I2 are available, which would be the limiting reactant? 3. 0.329 g of Fe3O4 and 0.812 g of Al are available for the following reaction: 3 Fe3O4 + 8 Al → 4 Al2O3 + 9 Fe. What would be the limiting reactant?When benzene (C6H6) reacts with bromine (Br)2, bromobenzene(C6H5Br) is obtained:C6H6 + Br2-------->C6H5Br + HBr(a) When 30.0 g of benzene reacts with 65.0 g of bromine, whatis the theoretical yield of bromobenzene? (b) If the actual yieldof bromobenzene is 42.3 g, what is the percentage yield?Complete combustion of 4.5892 a particular compound that contains only carbon, hydrogen and oxygen produces 10.4324 g of CO2 and 4.2705 g of H2O. The empirical formula of the compound is given by C H O (indicate "1" if there is only one atom of a given type in the empirical formula.) The molar mass of the compound is found to be 116.16 g/mol in a different experiment. What is the molecular formula of the compound? C H O
- When elemental copper is strongly heated with sulfur, a mixture of CuS and Cu2Sis produced. with CuS predominating. :math>Cu(s)+S(s)CuS(s)2Cu(s)+S(s)Cu2S(s) at is the theoretical yield of CuS when 31.8 g of Cu(s) is heated with 50.0 g of S? (Assume only CuS is produced in the reaction.) What is the percent yield of CuS if only 40.0 g of CuS can be isolated from the mixture?4-66 Benzene reacts with bromine to produce bromoben zene according to the following equation: If 60.0 g of benzene is mixed with 135 g of bromine, (a) Which is the limiting reagent? (b) How many grams of bromobenzene are formed in the reaction?Ammonia reacts with a limited amount of oxygen according to the equation 4NH3(g)+5O2(g)4NO(g)+6H2O(l)(a) How many moles of NO are obtained when 3.914 moles of oxygen are used? (b) How many moles of oxygen are required to react with 2.611 moles of ammonia? (c) How many moles of water are obtained when 0.8144 moles of ammonia are used? (d) How many moles of oxygen are required to produce 0.2179 mol of water?
- 11. In mining, roasting is the oxidation of metal sulfides to produce metal oxides and sulfur dioxide, a typical example is zinc sulfide: 2 ZnS + 3 O2 - 2 ZnO + 2 SO2 When 100.0 g of zinc sulfide reacts with 70.0 g of oxygen according to the above reaction, determine: The limiting reagent for the above reaction is? A) ZnS B) ZnO C) SO2 D) O2 E) None of the aboveBalance the following chemical equation, then answer the following question. C8H18(g)+O2(g)→CO2(g)+H2O(g)C8H18(g)+O2(g)→CO2(g)+H2O(g) How many grams of oxygen are required to react with 16.0 grams of octane (C8H18C8H18) in the combustion of octane in gasoline?NH3 (g) + O2 (g) ---> NO (g) + H2O (I) (Balance equation) For the following reaction, if 0.503 mole NH3 reacts with 0.356 mole O2, Which is the limiting reagant for the product NO? For the previous equation, if 2.3 g of NH3 reacts with 4.5 g O2, how much NO is produced?
- Given the balanced chemical equation below, 2 NO(g) + 5 H2 (g) --> 2 NH3(g) + 2 H2O(g) 1. There are 4.00 moles of NO in a reaction vessel that has EXCESS H2. How much NH3should be produced in moles? In grams? 2. There are 4.00 moles of NO in a reaction vessel that has EXCESS H2. How much H2O should be produced in moles? In grams? 3. There are 4.00 moles of NO and 14.00 moles of H2 in a reaction vessel, how much NH3 should be produced in moles? In grams? 4. For the previous reaction that began with 4.00 moles of NO and 14.00 moles of H2 in a reaction vessel, what is the limiting reactant? How many moles of the reactant in excess will be left over? How many grams of the reactant in excess will be leftover?Xanthotoxin, a photosensitizer compound found in parsnips, contains only C, H, and O. Combustion of 1.000 g of xanthotoxin produces 2.443 g of CO₂ and 0.3334 g of H₂O. Determine the molar mass of the compound if it is between 175.0 and 250.0 g/mol. Provide an answer to four significant figures.Imagine that you are working on ways to improve the process by which iron ore containing Fe2O3 is converted into iron. In your tests you carry out the following reaction on a small scale: Fe2O3 (s) + CO (g) ---> Fe (s) + CO2 (g)(a) If you start with 150 g of Fe2O3 as the limiting reagent, what is the theoretical yield of Fe? (b) If the actual yield of Fe in your test was 87.9 g, what was the percent yield?