Methanol is used in racing cars because it is a clean fuel. It can be synthesized according to the following reaction, What is the percent yield if 5.0 x 103 g of hydrogen gas reacts with an excess of carbon monoxide to produce 3.5 x 104 g of methanol? CO(g) + 2H2(g) ----- CH3OH(l) A) 90.3 % B) 43.8 % C) 56.2 % D) 87.5 %

Q: What is the percent yield for this reaction?

A:

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: If 103.1 g of PCl5 are formed from the reaction of 61.3 g Cl2 with excess PCl3, what is the percent…

A: .P(1319) + Cl₂ lg)puslg)since Plusis presentinexcessSOCl2the Limiting Reactant.Given Massof ų (g) =…

Q: What is the percent yield for the reaction PCI3(3) if 44.2 g of PCls (M = 208.2 g/mol) are formed…

A: Given, PCl3(g) + Cl2(g) ➝ PCl5(g)  Mass of PCl3 reacts = 49.7 g Molar mass of PCl3 = 137.3 g/mol Cl2…

Q: A sample of 0.49 g of carbon dioxide was obtained by heating 1.24 g of calcium carbonate. What is…

A: The first step in calculating the percent yield is to determine the molar mass of the reactants and…

Q: What is the percent yield of a reaction if the product recovered is 21.2 g and the theoretical yield…

A: The correct options are as follows:

Q: A sample of 10.0g NH3 on oxidation produces 6.0 g of NO. calculate the percent yield. Reaction :…

A:

Q: A fuel mixture used in the early days of rocketry contained hydrazine (N2H4) and dinitrogen…

A: Given;

Q: What is the theoretical yield of sodium chloride when 8.3 g of sodium is reacted with 4.5 g of…

A: We have to calculate theoretical yield of NaCl ,that means we have to calculate how much NaCl has…

Q: Starting with 1.34 g of potassium chlorate (molar mass 122.55 g/mol), a student determined that the…

A:

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 common laboratory method for preparing oxygen gas involves decomposing potassium chlorate…

A: Given that,Decompose of potassium chlorate is

Q: Iron metal reacts with chlorine gas giving iron (III) chloride. The balanced chemical equation for…

A: Percentage yield can be calculated by dividing actual yield by theoretical yield and multiplying by…

Q: A container holds 75.0 g of CuO and 5.00 g of H₂. The following reaction occurs: CuO + H₂ --> Cu +…

A:

Q: What is the theoretical yield when 38.2 g Al reacts with 14.8 g O2 according to the following…

A:

Q: A student obtained 11.4 g of PbSO4 from the following reaction. The student added 15 g of Lead (II)…

A:

Q: in this reaction 2VS3+9O2–> 2VO3+6 SO2 if we were to use 25.4 g of VS3 and 25.2 g of O2, and…

A:

Q: When 15.0 g of NH3 react, the actual yield of N2 is 13.5 g. What is the percent yield? 4 NH3 (g) +…

A: Given; 4 NH3 (g) + 6 NO (g) ⟶ 5 N2 (g) + 6 H2O(l) Mass of NH3 = 15.0 g Actual yield of N2 gas = 13.5…

Q: A fuel mixture used in the early days of rocketry contained hydrazine (N2H4) and dinitrogen…

A: Given  Balanced reaction  2N2H4(l)  + N2O4(g)   →  3N2(g)  +  4H2O(g) Number of mole of N2H4 = 9.15…

Q: A reaction of 34.3 g of Na and 38.9 g of Br₂ yields 47.5 g of NaBr. What is the percent yield? 2…

A: A question based on general chemistry that is to be accomplished.

Q: When 12.4 g of CH4 is reacted with excess O2, a mass of 20.8 g of CH4O is recovered. What is the %…

A: The number of moles of a compound can be determined as: Number of moles=Given massMolar…

Q: A sample of 0.52 g of carbon dioxide was obtained by heating 1.28 g of calcium carbonate. What is…

A:

Q: Calculate the percent yield for the reaction if 76.8 g of H2O reacted completely with nitrogen…

A:

Q: What is the actual amount of magnesium oxide produced when excess carbon dioxide reacts with 44.8 G…

A: The chemical reaction is- 2Mg(s)+CO2(g)→2MgO(s)+C(s) The mass of Magnesium metal = 44.8 g The molar…

Q: If the theoretical yield of a reaction is 0.102 gg and the actual yield is 9.40×10−2 gg , what is…

A:

Q: How much aluminum oxide and how much carbon are needed to prepare  673  g of aluminum by the…

A: As per balanced chemical reaction provided, 2 mol of Al2O3 reacts with 3 mol of carbon. The products…

Q: What is the percent yield (to four significant figures) of this reaction if 153.97 g iron (III)…

A: Given information is as follows: 6HCl(aq) + Fe2O3(s) → 3H2O(l) + 2FeCl3(aq) The mass of iron (III)…

Q: Determine the limiting reactant (LR) and the Theoretical Yield (in g) of nitrogen that can be formed…

A:

Q: How many grams of carbon dioxide are produced when 17.680 moles of the following substance is…

A: Solution

Q: When ethane, C₂H6, reacts with chlorine, Cl₂, the main product is C₂H5CI, but other products…

A: Given ,

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 of oxygen with Carbon forms Carbon Monoxide, a toxin that causes many health problems…

A: The balanced chemical reaction is the reaction in which all the elements present in the reactant are…

Q: How many grams of CO2 can you produce by reacting 10.85 g of Fe:Os with excess CO according to the…

A: No. of moles of Fe2O3 is calculated using given mass as follows: No. of moles = massmolar massof…

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: Ethyl alcohol (C2H6O) is prepared by the reaction of ethylene (C2H4) with water; C2H4 (g) + H2O (l)…

A: Molar mass of ethylene is 28.05 g/mol.          Molar mass of ethyl alcohol is 46.07 g/mol

Q: Combustion of 8.45 mg of an unknown substance yields 14.0 mg CO2 and 7.08 mg H20. The unknown…

A: We have to calculate the % of each element in substance.

Q: 9.87 g of ammonia, NH3, react completely according to the reaction: 2 NH3 + CO₂ -> CN₂OH4+ H₂O If…

A: The given mass of ammonia = 9.87 gThe experimental yield of urea = 13.74 gThe percent yield of the…

Q: For the reaction: Na2CO3 + CuCl2 --> CuCO3 + 2 NaCl  If 25.7 grams of NaCO3 are required to form…

A: The balanced reaction is: Molar mass of Na2CO3 = 105.98 g/mol Molar mass of NaCl = 58.44 g/mol…

Q: A sample of 108.2 g of Calcium oxide was obtained by heating 258 g of calcium carbonate. What is the…

A: The percent yield is the ratio of the amount of products actually obtained and the theoretically…

Q: When 11.0 mol of NO reacts, the actual yield of N2 is 8.63 mol. What is the percent yield? 4NH3(g)…

A: According to balanced chemical equation, 6 moles of NO gives 5 moles of N2. Hence, Moles of N2 that…

Q: When 15.0 g of NH3 reacts, the actual yield of N2 is 6.50 g. What is the percent yield?…

A: We Know   Molecular Weight of NH3= 17g Mole of NH3 given= 15/17=.882

Q: Nitric Oxide can be made from the oxidation of ammonia as shown below. A reaction between 8.5 g of…

A: We have to calculate the percent yield of the reaction.

Q: When 24.5 g of NH3 reacts, the actual yield of H20 is 26.5g. What is the percent yield? 4NH3(g) +…

A: Given  mass of NH3    = 24.5 gram  Actual yield     =   26.5 gram  ℅ yield            =   ?

Q: If 14.0 g of C₂H4 react completely to form 7.84 g of water, as shown below, the percent yield in the…

A: We can solve this problem by using this equation %yield = (observed yield / theoretical yield)× 100

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".