Q: For the following reaction, 0.126 moles of iron are mixed with 0.429 moles of oxygen gas. iron(s) +…
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Q: what is the theoretical and percent yield of the reaction?
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Q: Lead(III) sulfide reacts with calcium chloride to produce lead(III) chloride and caleium sulfide. If…
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Q: The theoretical yield of aluminum is 1.16 moles. If only 1.03 moles of aluminum were collected, what…
A: Given, Theoretical yield = 1.16 moles Actual yield = 1.03 moles % yield = ?
Q: According to the following reaction, how many moles of bromine trifluoride are necessary to form…
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Q: According to the following reaction, how many moles of calcium carbonate are necessary to form 0.360…
A: The given reaction is, Calcium carbonate (s) ----> calcium oxide (s) + carbon…
Q: For
A: 2Fe(s) + 3Cl2(g) ------> 2FeCl3(s)
Q: Hydrogen gas and nitrogen gas react to give ammonia gas. How many moles of hydrogen are needed to…
A: In a chemical reaction, when number of atoms of each element present in reactants are equal to…
Q: If 1.7 moles of ammonium phosphate reacts with zinc nitrate, what will be the actual yield (in…
A: 2(NH4)3PO4 + 3Zn(NO3)2 → Zn3(PO4)2 + 6NH4NO3 From this Balanced chemical equation we get that ;…
Q: Solid potassium chloride and oxygen gas are products of heated solid potassium chlorate. How many…
A: Given: Moles of potassium chlorate= 0.083 mol Moles of oxygen= ? In order to calculate the moles of…
Q: How many molecules (not moles) of NH3 are produced from 2.21*10^-4g of H2?
A: Given:Mass of H = 2.21 X 10-4 g of H2We need to find the number of molecules (not moles) of NH3 are…
Q: According to the following reaction, how many moles of iodine are necessary to form 0.224 moles…
A: Hydrogen (g) + iodine (s) → Hydrogen iodide (g) H2 (g) + I2 (g) → 2 HI (g) Moles of Hydrogen…
Q: 2. What would be the limiting reactant of sodium reacted with 10 mol of chlorine to form 10 mol of…
A: Sodium reacts with chlorine to form sodium chloride. The equation for the balanced chemical reaction…
Q: How many molecules of magnesium hydroxide are produced from 0.960 mole of magnesium oxide?
A: One mole of compound contains Avogadro number of its molecules. Avogadro Number = 6.022 × 1023
Q: How much methane is required to produce 55.0 g of carbon dioxide, when burned in excess oxygen?
A: Dear student , since you have posted multiple questions we are allowed to solve only first question…
Q: How many molecules (not moles) of NH3 are produced from 7.42×10−4 g of H2?
A: To obtain the number of molecules, first of all the reaction for the production of NH3 should be…
Q: If you had excess chlorine, how many moles of aluminum chloride could be produced from 22.0 g of…
A: If excess chlorine is present, then number of moles of aluminium chloride that could be produced…
Q: Calculate the moles ammonium perchlorate needed to produce 0.090 mol of oxygen.
A: Decomposition equation of ammonium perchlorate is NH4ClO4 --------> NH3 + HClO4 HClO4----->…
Q: What is the total number of moles of aluminum oxide that can be formed when 4 moles of aluminum…
A: Answer:- This question is answered by using the simple concept of writing the balanced chemical…
Q: chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 3…
A: According to the reaction, 1 mole of NaHCO3 is reaction with 1 mole of HCl. Therefore, 3 moles of…
Q: How many moles of KCl can be produced from 7.08mol KClO3 ?
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Q: How many molecules (not moles) of NH3 are produced from 5.01×10−4 g of H2?
A: Calculate the number of moles of hydrogen gas. The molar mass of hydrogen gas is 2g/mol.
Q: Carbon dioxide can be created by burning carbon in oxygen: C+ O2 → CO2 Approximately how many moles…
A: Given : C + O2 → CO2 Mass of C reacts with excess O2 = 24 g To calculate : No.of moles of CO2…
Q: How many moles of Ag can be obtained from 1.01 moles Cu using the following balanced reaction? Use…
A: Balanced reaction : 2AgNO3 + Cu .....> Cu(NO3)2 + 2Ag Moles of Cu = 1.01 moles
Q: , what is the limiting reactant and the theoretical yield of water?
A: Number of moles = mass/molar mass Molar mass of O2 = 31.999 g/mol Molar mass of H2 = 2.0159 g/mol…
Q: s the formula for the limiting reagent? s the maximum amount of bromine monochloride that can be…
A: Br2(g) + Cl2(g) ---> 2BrCl(g) Moles of Br2 = 0.299 moles Moles of Cl2 = 0.251 moles So, moles of…
Q: How many moles of potassium chloride are formed when 6.0 moles of chlorine are reacted with…
A: Reactants - 1) Chlorine 2) Potassium bromide Products - 1) Bromine 2) Potassium chloride Moles…
Q: How many grams of sodium hydroxide are produced from 5g of sodium carbonate and 10g of iron…
A: Given information: Mass of Na2CO3 = 5.0 g Mass of Fe(OH)3 = 10.0 g Molar mass of Na2CO3 = 105.988…
Q: According to the following reaction, how many moles of calcium carbonate are necessary to form 0.434…
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Q: A. How many grams of methyl alcohol can be produced from 147 g of CO with excess hydrogen present?
A: Number of moles = mass/molar mass Molar mass of CO = 28 g/mol Molar mass of H2 = 2.0 g/mol Molar…
Q: Choose the key item that must be determined experimentally in order to calculate the percent yield…
A: The percent yield is calculated using the following formula:
Q: Phosphorus pentachloride reacts with water to produce phosphoric acid and hydrochloric acid. How…
A: Given :- Phosphorus pentachloride + water → phosphoric acid + hydrochloric acid Number of moles of…
Q: How many moles of water can be produced from 0.61 moles of Sodium Hydroxide, assuming there will be…
A: Here we are given that sodium hydroxide in present in limited amount and so it is the limiting…
Q: How many grams of calcium chloride will be produced when 31.0 g of calcium carbonate is combined…
A: Number of moles can be determined as follows: No.of moles of…
Q: b. If the percentage yield of sodium chloride is 67%, what is the actual yield of sodium chloride?
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Q: According to the following reaction, how many grams of calcium carbonate are necessary to form 0.483…
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Q: What does the term stoichiometrically equivalent molar ratiomean, and how is it applied in solving…
A: A chemical reaction is essentially a system which involves a large collection of particles (atoms,…
Q: Given the following chemical equation: 2 Mg(s) + 3 N2 (g) --> 2 MgN3 (s) How many grams of MgN3 will…
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Q: According to the following reaction, how many grams of hydrogen iodide will be formed upon the…
A: Hydrogen gas reacts with iodine to form hydrogen iodide. The equation for the balanced chemical…
Q: How many grams of potassium chloride are produced if 25.0 grams of potassium chlorate decompose?
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Q: How many moles of iron(III) oxide can be produced from the reaction of 10.980 moles of iron reacting…
A: Given: Moles of Fe = 10.980 moles
Q: According to the following reaction, how many moles of carbon dioxide will be formed upon the…
A: Law of Conservation of Mass:- The law of conservation of mass states that mass can neither be…
Q: For a theoretical yield of 5 g and percent yield of 53.7015%, calculate the actual yield for a…
A: Given :- Theoretical yield = 5 g Percent yield = 53.7015% To calculate :- Actual yield (in g)
Q: What would be the limiting reactant if 6 mol of sodium reacted with 3 mol of chlorine to form sodium…
A: Limiting reactant :- A reactant which is present in lesser number of moles than required as per…
Q: how many moles of CO2 would be produced from 7.123 moles of O2according to 2C2H6+7O2=4CO2+6H2O
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Q: 44 grams of carbon dioxide was formed after combustion of 12 grams of methane gas. Calculate…
A: Given that : Mass of CO2 formed = 44g Mass of methane = 12g Combustion Reaction of methane CH4(g)…
Q: How many moles of carbon dioxide are produced if 2.78 moles of octane react with excess oxygen gas?
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Q: If 250. grams of sodium azide undergoes decomposition, how many molecules of nitrogen gas are…
A: We have to predict the molecules of nitrogen gas Produced.
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- Although many sulfate salts are soluble in water, calcium sulfate is not (Table 7. 1). Therefore, a solution of calcium chloride will react with sodium sulfate solution to produce a precipitate of calcium sulfate. The balanced equation is :math>CaCl2(aq)+Na2SO4(aq)CaSO4(s)+2NaCl(aq) a solution containing 5.21 g of calcium chloride is combined with a solution containing 4.95 g of sodium sulfate, which is the limiting reactant? Which reactant is present in excess?Classify each of the following statements as true or false: a Coefficients in a chemical equation express the molar proportions among both reactants and products. b A stoichiometry problem can be solved with an unbalanced equation. c In solving a stoichiometry problem, the change from quantity of given substance to quantity of wanted substance is based on masses. d Percentage yield is actual yield expressed as a percentage of ideal yield. e The quantity of product of any reaction can be calculated only through the moles of the limiting reactant. f rH is positive for an endothermic reaction and negative for an exothermic reaction.Consider the unbalanced equation for the combustion of propane: :math>C3H8(g)+O2(g)CO2(g)+H2O(g) rst, balance the equation. Then, for a given amount of propane, write the mole ratios that would enable you to calculate the number of moles of each product as well as the number of moles of O2that would be involved in a complete reaction. Finally, show how these mole ratios would be applied if 0.55 mole of propane is combusted.
- Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion, hcpLcnc reacts with oxygen to produce carbon dioxide and water. What is the mole ratio that would enable you to calculate the number of moles of oxygen needed to react exactly with a given number of moles of heptene? What mole ratios would you use to calculate how many moles of each product form from a given number of moles of heptene?4.37 The theoretical yield and the actual yield for various reactions are given below. Determine the corresponding percentage yields. Theoretical Yield Actual Yield Reaction 1 35.0 g 12.8 g Reaction 2 9.3 g 120 mg Reaction 3 3.7 metric tons 1250 kg Reaction 4 40.0 g 41.0 gLead(II) carbonate, also called “white lead,” was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer he used in paints intended for residential homes. Lead(II) carbonate is prepared industrially by reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced equation is :math>Pb(C2H3O2)2(aq)+H2O(l)+CO2(g)PbCO3(s)+HC2H3O2(aq) ppose an aqueous solution containing 1.25 g of lead(II) acetate is treated with 5.95 g of carbon dioxide. Calculate the theoretical yield of lead carbonate.
- Consider a reaction represented by the following balanced equation :math>2A+3BC+4D u find that it requires equal masses of A and B so that there are no reactants left over. Which of the following is true? Justify your choice. l type='a'> The molar mass of A must be greater than the molar mass of B. i>The molar mass of A must be less than the molar mass of B. i>The molar mass of A must be the same as the molar mass of B.Consider the balanced chemical equation :math>A+5B3C+4D en equal masses of A and B are reacted, which is limiting, A or B? Justify your choice. If the molar mass of A is greater than the molar mass of B, then A must be limiting. If the molar mass of A is less than the molar mass of B, then A must be limiting. If the molar mass of A is greater than the molar mass of B, then B must be limiting. If the molar mass of A is less than the molar mass of B, then B must be limiting.Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.
- The gaseous hydrocarbon acetylene, C2H2, is used in welders’ torches because of the large amount of heat released when acetylene burns with oxygen. :math>2C2H2(g)+5O2(g)4CO2(g)+2H2O(g) w many grams of oxygen gas are needed for the complete combustion of 150 g of acetylene?For the chemical reaction Sb2S3+6HCl2SbCl3+3H2S write the conversion factor that would be needed to do each of the following one-step conversions. a. Moles of SbCl3 to moles of H2S b. Moles of Sb2S3 to moles of HCl c. Moles of H2S to moles of HCl d. Moles of Sb2S3 to moles of SbCl3Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.