What is the amount of limiting reactant consumed in Procedure 1? Calcium phosphate is used as an antacid, supplement, and/or a source of calcium and phosphate in toothpaste.In a laboratory setup calcium hydroxide can be reacted with phosphoric acid to produce calcium phosphate with water as by-product.In an experimental process, there are three procedures to deal with in the production of calcium phosphate.Procedure 1: 846.0 grams of calcium oxide and 264.0 grams of water are combined in order to produce a single product, calciumhydroxide.Procedure 2: 979.0 grams of diphosphorus pentoxide and 323.0 grams of water are combined in order to produce a single product,phosphoric acid.Procedure 3: Actual mass of isolated calcium hydroxide from Procedure 1 and actual mass of isolated phosphoric acid fromProcedure 2 are combined in order to produce calcium phosphate with water as by-product.It is also noted that each procedure had the following percent yields:Procedure 1: 53.58% yield on calcium hydroxide.Procedure 2: 59.26% yield on phosphoric acid.Procedure 3: 31.41% yield on calcium phosphate.

Answered: Image /qna-images/answer/ffc33807-660e-4c93-b0f0-03da987a9b8c.jpg

Answered: rocedure 1: 846.0 grams of calcium…

rocedure 1: 846.0 grams of calcium oxide and 264.0 grams of water are combined in order to produce a single product, calcium droxide.

Chemistry for Today: General, Organic, and Biochemistry

9th Edition

ISBN:9781305960060

Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.81E

See similar textbooks

Related questions

Q: Give me the volume of one mug of milk

A: Volume of a substance is the space occupied by a substance.

Q: If the density of ethanol is 0.789 g/mL, how many cm3 can be produced by the fermentation of 45.4 kg…

A: Ethyl alcohol is formed by enzyme action on sugars and starches by fermentation. C6H12O6 → 2 CO2 + 2…

Q: It requires two sticks of butter to make a batch of 20 cookies. How much butter will it take to make…

A: Simple use of unitary method to solve this problem

Q: The gasoline tank of an automobile contains 59.0 kg of gasoline. The gasoline combines with 236 kg…

A: The reaction of gasoline (isooctane) and oxygen takes place as, 2 C8H18 + 25…

Q: The density of liquid ethanol C2H5OH is 0.789 g/mL. If 505 grams of glucose decomposes, how many…

A: The decomposition reaction of glucose can be expressed as, C6H12O6 (s) -----> 2…

Q: How many grams of Xe are contained in 454 mL?

A: Density of a substance is given as the mass per unit volume. The density is directly proportional to…

Q: Ethanol fuel mixtures have "E" numbers that indicate the percentage of ethanol in the mixture by…

A: Since, E10 is a mixture of 10% ethanol and 90% gasoline.

Q: You weigh a dry flask, and place a chunk of solid into it, then weigh it again. You then fill the…

A: We are given mass of flask = 58.97g Mass of flask + solid = 135.91g We have to find mass of solid

Q: A chemist has two different gasohol mixtures available. One contains 20% alcohol and the other 12%…

Q: 100.0 g of lead(II) nitrate is reacted with 50.0 g of potassium iodide (in plenty of water). How…

Q: The burning of 4.13 g of carbon in oxygen produces 24.22 g of carbon dioxide as the only product.…

Q: A sample of air, upon analysis by an environmentalist showed that it contains 1.4 X 10-18 of mercury

Q: You will need grams of sodium chloride and mL of water.

A: Given :- mass of solution = 184 g % w/w = 3.17 % To be calculated :- mass of NaCl (…

Q: 6. Calculate The scientist repeats the experiment, burning a new sample of steel wool until it is…

Q: If 33.3 grams of hydrogen gas were mixed with 45.55 grams of nitrogen gas, then how many grams of…

A: Nitrogen gas reacts with hydrogen gas to form ammonia. The equation for the balanced chemical…

Q: Oil spreads on the water to form a film 110nm thick. How many square kilometers(Km²) of the ocean…

A: The oil and water are two immiscible liquids which means that the oil cannot be dissolved in water.…

Q: student performs Experiment 7 using copper wire as the initial copper source and obtains the…

A: Given mass of dry beaker is 120.4265 g Given mass of dry beaker + copper wire is 122.4715 g After…

Q: (4€) Carbon reacts with Oxygen to produce Carbon monoxide. If 6.2 grams of Carbon and 2-8grams of…

A: 4 . E) When Carbon reacts with Oxygen , it produces carbon monoxide. The balanced chemical…

Q: A chemist has a 19.50g sample of drinking alcohol (ethyl alcohol). what is the volume ogf the…

A: The relationship between mass and volume is given below.

Q: An underground tank contains 600 kL of decane (C10H22). If the owner of the tank requires 2.52 ×…

A: Given: Volume of tank = 600kL Density = 1.21 g.ml-1 Molecules = 2.52 × 1029

Q: Brass is an alloy that is approximately 67% Cu and 33% Zn, by mass. How many grams of Cu and Zn are…

A: % by mass = Mass of the componentMass of the whole compound X 100 Given that, % by mass of Cu=67% %…

Q: A student add 15g of baking soda to 10g of acetic acid in a beaker. A chemical reaction occurs and a…

A: Baking soda : NaHCO3 ACETIC ACID : CH3COOH

Q: <) is 1.106 amu. Estimate the total bindi

Q: KI, H;PO4 KMNO4, H30* ,G

A: Two reactions whose product is to be determined, individually.

Q: Commercial solvents are commonly sold in 55-gallon drums. What is the weight in pound of the carbon…

A: Volume of the solvent = 55 gallon Volume of solvent in cc = 208198 cm3 (since 1 gallon = 3785.41…

Q: Combustion of hydrocarbons such as methane (CH.) produces carbon dioxide, a "greenhouse gas."…

A: When methane gas is burnt , then Carbon dioxide gas and water vapours are formed. The Balanced…

Q: A 5.00 g mixture of potassium sulfide and potassium chloride contains 2.80 g potassium. What…

A: The mass percentage is calculated using the formula given below: Mass percentage =mass of potassium…

Q: (c) MnO, + SO, Mn* + SOf

Q: 47.9 grams of nitric acid are reacted with 39.3 grams of potassium sulfate. How much nitrate can be…

A: Consider the given information is as follows; Mass of nitric acid HNO3 = 47.9 g Mass of potassium…

Q: Magnesium will burn in air to form both Mg;N2 and MgO. What mass of each product would be found if…

Q: A student determines the calcium content of a solution by first precipitating it as calcium…

A: Given data,Molarity of Ca(NO3)2=0.531MVolume of Ca(NO3)2=34.0mL=0.034L

Q: how many grams of Cu(NO3)2 can be made from 25 grams of copper

A: The reaction involves,

Q: Carbon tetrachloride, CCl4, was a popular dry-cleaning agent until it was shown to be carcinogenic.…

A: 1 mole = 6.022×1023 (Avogadro's number) The mass of one mole of molecules of a substance is known…

Q: Aqueous sulfurlc acid (H,SO will react with solld sodlum hydroxide (NaOH) to produce aqueous sodlum…

A: The balanced chemical equation can be written as follows: H2SO4 + 2 NaOH --> Na2SO4 + 2 H2O 1 mol…

Q: 750 g Oral 237 mL per bottle Potassium 950 g elemental iodine + 1.5 kgs potassium hydroxide…

A: Given that - Potassium iodide ,KI Here only one Compound is given , which is potassium iodide, KI…

Q: w grams of water wc

Q: If 52.4 g of O2 is mixed with 52.4 g of H2 and the mixture is ignited, what is the maximum mass of…

A: Mass of O2 = 52.4 gm Mass of H2 = 52.4 gm Mass of H2O = ?

Q: A 13.0-g sample of X combines with a 34.0-g sample of Y to form the compound X Y 2 . What is the…

A: Law of Conservation of mass: According to the law of conservation of mass, mass can neither be…

Q: You have two distinct gaseous compounds made from element X and element Y. The mass percents are as…

A: For easy calculations in the above question, let us consider one unit of compound A is 100 grams and…

Q: 378 g f) 3.8 x 10 mol x 0.0670 mol h) (2.3 x 10 m) (4.567 x 10 m)= 2.3x100m 230m

A: Here some values are given, we have to find the final answer of this given question. For…

Q: 0.848g of Na2B4O7.10H2O into a crucible. After hearing the sample for a short time and allowing the…

A: Na2B4O7.10H2O is known as borax.It is a hydrated crystal having 10molecules of water of…

Q: Liquid heptane, C,H,6 , burns in oxygen gas to yield carbon dioxide and water. What mass of carbon…

Q: A student is given a 6.216 g mixture of iron filings, calcium chloride, and sand. He separates the…

Q: A 5.00g sample of sand and salt is 75.0%w/w salt. How many grams of salt and sand are in the…

A: Mass percentage can be defined as the parts of a substance (A) per hundred parts of the total by…

Q: Aspirin can be prepared from salicylic acid (C7H;O3), which has a molar mass of 138.12 g/mol, and…

Q: You weigh a dry flask, and place a chunk of solid into it. then weigh it again. You then fill the…

Q: If a chemist were given 2.99 grams of a mixture of sugar and sand which gave 1.35 grams of sand on…

A: Given : Mass of mixture = 2.99 g Mass of sand = 1.35 g

Concept explainers

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".

Question

What is the amount of limiting reactant consumed in Procedure 1?

Calcium phosphate is used as an antacid, supplement, and/or a source of calcium and phosphate in toothpaste.
In a laboratory setup calcium hydroxide can be reacted with phosphoric acid to produce calcium phosphate with water as by-
product.
In an experimental process, there are three procedures to deal with in the production of calcium phosphate.
Procedure 1: 846.0 grams of calcium oxide and 264.0 grams of water are combined in order to produce a single product, calcium
hydroxide.
Procedure 2: 979.0 grams of diphosphorus pentoxide and 323.0 grams of water are combined in order to produce a single product,
phosphoric acid.
Procedure 3: Actual mass of isolated calcium hydroxide from Procedure 1 and actual mass of isolated phosphoric acid from
Procedure 2 are combined in order to produce calcium phosphate with water as by-product.
It is also noted that each procedure had the following percent yields:
Procedure 1: 53.58% yield on calcium hydroxide.
Procedure 2: 59.26% yield on phosphoric acid.
Procedure 3: 31.41% yield on calcium phosphate.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What is the purpose of staggering the start and stop of the reactions?
Explain the meaning of “the reaction goes to less than 100% completion”
This reaction is used to obtain iron from iron ore: Fe2O3(s) + 3 CO(g) —>2 Fe(s) + 3 CO2(g) The reaction of 185 g of Fe2O3 with 95.3 g of CO produces 87.4 g of Fe. Determine the limiting reactant, theoretical yield, and percent yield. (include solution map & steps)
Name the missing reactant for the reaction
Limiting reactants, please double check answer
What was the initial reactant concentration for the reaction described in Part A?
I2 (aq) + CH3COCH3 (aq)  HI (aq) + ICH2COCH3 (aq)Iodine in solution has a yellow-brown color, whereas the acetone and both products are colorless. This means that we can run the reaction using iodine as the limiting reagent, and when we see that the yellow-brown color of the iodine has disappeared, we know that the reaction has stopped and all of the iodine has been consumed. Recall that to calculate a rate of reaction, we would like toknow the change in concentration of a reactant or product during a fixed amount of time. Wewill choose the reactant iodine in this case, because its brown color allows us to determinewhen its concentration has fallen to zero. Rate = –Δ[I2] / Δt = – ([I2]final – [I2]initial) / ([tfinal – tinitial) = – (0 – [I2]initial) / (tfinal – 0) = [I2]initial / tfinal Run several trials at different concentrations of reactants and use themethod of initial rates to obtain values for k, x, y, and z in the rate law. Rate = k [I2]x [acetone]y [H+]z Run the…
I2 (aq) + CH3COCH3 (aq)  HI (aq) + ICH2COCH3 (aq)Iodine in solution has a yellow-brown color, whereas the acetone and both products are colorless. This means that we can run the reaction using iodine as the limiting reagent, and when we see that the yellow-brown color of the iodine has disappeared, we know that the reaction has stopped and all of the iodine has been consumed. Recall that to calculate a rate of reaction, we would like toknow the change in concentration of a reactant or product during a fixed amount of time. Wewill choose the reactant iodine in this case, because its brown color allows us to determinewhen its concentration has fallen to zero. Rate = –Δ[I2] / Δt = – ([I2]final – [I2]initial) / ([tfinal – tinitial) = – (0 – [I2]initial) / (tfinal – 0) = [I2]initial / tfinal Run several trials at different concentrations of reactants and use themethod of initial rates to obtain values for k, x, y, and z in the rate law. Rate = k [I2]x [acetone]y [H+]z Run the…
As the reactant concentration increases, the average kinetic energy of molecules increases. TRUE OR FALSE?
Automobile air bags employ a chemical reaction involving the rapid decomposition of sodium azide (NaN3) into sodium metal and nitrogen gas to inflate in a collision. How much sodium azide is required to decompose to inflate a 20.0 L air bag? Assume that the gas is at standard temperature and pressure, and thus occupies 22.4 L per mole. (AW: Na=23; N=14.007)
At a particular temperature, Kc = 6.0 × 102 for2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g)Calculate Kc for each of the following reactions:(a) NO(g) + H2(g) ⇌ 12N2(g) + H2O(g)
1. If a student loses more than 0.01 g between the first and second heating of sodium bicarbonate, what does this indicate about the decomposition reaction?