Q: Calculate the mass of limestone (CaCO,) that must be decomposed to produce 475 g of lime (CaO). The…
A: Mass of CaO = 475 g Molar mass of CaO = 56.077 g mol-1 Molar mass of CaCO3 = 100.087 g mol-1
Q: Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium…
A: Answer: This question is based on the stoichiometric calculation of the reaction that we have…
Q: f the reaction of 30 grams of calcium carbonate (CaCO3) produces 15 grams of calcium oxide (CaO),…
A: CaCO3 decompose to give CaO and CO2. Reaction is as follows: CaCO3 ---------> CaO + CO2 Mass of…
Q: Define the terms theoretical yield, actual yield, and percent yield?
A: Theoretical yield is defined as the yield which is the maximum yield of products, which is…
Q: What does it mean to say a reactant is present “in excess” in a process? Can the limiting reactant…
A: Limiting reactant: In a chemical reaction the substance which is totally consumed is known as…
Q: 1.1127 g of chromium (II) nitrate was mixed in water with 0.5437 g of sodium phosphate A solid…
A: a) The balanced chemical reaction is, 3Cr(NO3)2(aq) + 2Na3PO4(aq) ---> Cr3(PO4)2(s) + 6NaNO3
Q: Calculate the percent yield of a reaction?
A: Yield is the measure of the quantity of moles of product formed in relation to the product consumed…
Q: For a theoretical yield of 2.54 g and percent yield of 82.8583%, calculate the actual yield for a…
A: Given data, Theoretical yield = 2.54 g % yield = 82.8583% Then, Actual yield = ?
Q: If the theoretical yield of a reaction is 0.118 g and the actual yield is 0.104 g, what is the…
A: The given data contains, Theoretical yield = 0.118 g. Actual yield = 0.104 g.
Q: 1.51 g H2 is allowed to react with 10.0 g N2, producing 2.01 g NH3 .
A: Welcome to bartleby !
Q: Why is the actual yield in a reaction almost always less than the theoretical yield?
A: THEORETICAL YIELD Theoretical yield is the amount produced from the correct computations.…
Q: The theoretical yield of a product in a reaction is determined by the limiting reactant. O True…
A: 1.Theoretical Yield is the amount of product formed from a given balanced equation. 2. Actual yield…
Q: The actual yield is 4.951 What is the percentage yield of the reaction ?
A: Percent yield is the percent amount of product actually formed with reference to that of theoretical…
Q: The limiting reactant is the reactant that has the lowest coefficient in the balanced equation. O…
A: Limiting reactant in a chemical reaction is a reactant that will be consumed completely. Consider…
Q: Calcium bromide reacts with silver nitrate to form calcium nitrate and silver bromide. If an aqueous…
A: Limiting reactant :- A reactant which is present in lesser number of moles than required as per…
Q: 3.86 Why is the theoretical yield of a reaction determinedonly by the amount of the limiting…
A: Limiting reagent is the reagent which is consumed in the chemical reaction completely. It decides…
Q: For a theoretical yield of 6.7 g and actual yield of 4.57426 g, calculate the percent yield for a…
A: We have to predict the percentage yield.
Q: The theoretical yield of product for a particular reaction is 32.03 g. A very meticulous student…
A: Percent yield = practical yield ×100theoretical yield = 31.87×10032.03…
Q: If the theoretical yield of the reaction below corresponds to 74.8 gg and the actual yield was 57.4…
A: The percent yield is the ratio of actual yield to theoretical yield, which is expressed as…
Q: If the percent yield for a reaction is 100% and the theoretical yield is 88 g. What is the actual…
A: Actual yield is defined as quantity of a product received from a chemical reaction.
Q: A reaction has a theoretical yield of 76.5 grams of a product, and a percent yield of 32.5 %. What…
A: A numerical problem based on percent yield, which is to be accomplished.
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: Solutions containing 5.03g of calcium chloride and 2.78g of silver nitrate are combined to from 1.00…
A: NOTE : Since it is not mentioned that which product is having 1 g yield. Hence we can assume it to…
Q: Theoretical yield
A:
Q: A reaction has a theoretical yield of 55.8 g. When the reaction is carried out, 37.2 g of the…
A: Percent yield is the percent ratio of actual yield to the theoretical yield. It is calculated to be…
Q: The theoretical yield of a reaction is 75.0 grams of product and the actual yield is 42.0 g. what is…
A: Given as The theoretical yield of a reaction is 75.0 gram and actual yield is 42.0 g % yield has to…
Q: If 18.2 kg NH3 is produced by a reaction mixture that initially contains 6.00 kg H2 and an excess of…
A:
Q: Calculate the percent yield of a reaction if the theoretical yield of the reaction is 2.70 moles,…
A:
Q: For a theoretical yield of 21 g and actual yield of 12 g, calculate the percent yield for a chemical…
A: The theoretical yield is = 21 g The actual yield is = 12 g The percent yield of the given chemical…
Q: Calculate the percent yield of a reaction if the theoretical yield of the reaction is 1.43 moles,…
A: ans: 80.41% % yield = Actual yield /theoretical yield x 100 given theoretical yield=1.43 moles…
Q: Balanced Chemical Equation Reaction Type: At completion of reactions: Grams of nitrogen Grams of…
A: All your calculations so far are correct. N2(g) is the limiting reactant.
Q: What mass of H2O is formed when H2 reacts with 284 g of O2?
A:
Q: If 1.00g of hydrogen reacts and 4.50g of NH3 are collected, what is the precent yield?
A: Given: Mass of Hydrogen= 1.00 g Mass of NH3 formed (Actual Yield) =4.50g To calculate: Percent yield…
Q: what is the percent yield?
A: The ratio between the actual yield and the theoretical yield multiply by 100 is known as percent…
Q: Consider the reaction of solid P₄ and chlorine gas to form gaseous phosphorus trichloride. The…
A: Percent yield of any reaction is given in terms of product as
Q: A 1.897 g sample of pure Mg(HCO3)2 was heated and decomposed. When the sample cooled, it weighed…
A: Any reaction's percent yield gets computing by taking ratio of its actual yield with its calculated…
Q: ate the percent yield ог а reaction e theoretical yield of the reaction is 2.2 oles, but only 2.65…
A: Percent yield is the percent ratio of actual yield to theoretical yield and it is expressed as…
Q: For the reaction Ti(s) + 2 F2 (g) → TIF4(s) compute the theoretical yield of the product (in grams)…
A:
Q: Aqueous hydrochloric acid (HCI) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium…
A:
Q: What is the maximum amount, in grams, of CO2 produced when 6.00grams of carbon are reacted with…
A: The chemical equation for given reaction is as follows,
Q: If 24 molecules of H2 and 18 molecules of N2 are mixed and allowed to react, how many molecules of…
A: Recall the reaction between H2 and N2 to obtain NH3 N2+3H2→2NH3According to stoichiometry…
Q: If 15.0 g potassium metal are reacted with 15.0 g oxygen gas to yield 14.3 potassium oxide, what is…
A: Reaction occurs as: Moles can be given as: n: Number of moles. m: Mass of the reactants or…
Q: In the reaction Cl2 (g) + I2 (s) --> 2 ICI (g) 22.1 grams of chlorine are reacted in the presence of…
A:
Q: Determine the limiting reactant and the percent yield of this reaction. How many molecules of…
A:
Q: if 15.0 mol of iron combines with excess chlorine gas, and 12.2 mol of FeCl3 is produced. what is…
A: Given Number of mole of iron = 15 mole Number of mole of FeCl3 = 12.2 mole % yield = ?
Q: 1.65 g H2 is allowed to react with 10.0 g N2, producing 1.79 g NH3. What is the theoretical yield in…
A: The reaction between H2 and N2 is as follows,
Q: Mass of product (g) 3.516 Theoretical yield (g) Product percent yield
A:
Q: 16. 2K + Br, 2KBR 71.1g Br, is reacted, and 64.1g KBr is produced. What is the percent yield for the…
A: The given chemical reaction is: 2K+Br2→2KBr. Then, 1g of Br2 formed --- 64.1g of KBr. Calculate the…
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- 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?Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
- 4.70 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) identify the limiting reactant, and explain how the pictures allow you to do so.The space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l)+O2(g)CO2(g)+H2O(l) If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
- 4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(II) sulfate can be prepared in the laboratory by reaction of copper(II) oxide with sulfuric acid. The unbalanced equation is :math>CuO(s)+H2SO4(aq)CuSO4(aq)+H2O(l) 2.49 g of copper(II) oxide is treated with 5.05 g of pure sulfuric acid, which reactant would limit the quantity of copper(II) sulfate that could be produced?3.75 The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A atoms are shown in blue and B atoms in white). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reac- tion has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
- Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.3.105 Nitric acid is often sold and transported as a concentrated 16 M aqueous solution. How many gallons of such a solution would be needed to contain the roughly 2.1109 pounds of HNO3 produced annually in the United States?Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain. l type='a'> Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B. Choose the reactant with the smallest mass given. So in this case, the limiting reactant is The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.