Heating a certain pure solid completely decomposes it into a solid and a gas, each ofwhich is also a pure substance. Which of the following is/are reasonable conclusionsregarding these observations?1. The solid is a compound and the gas is an element.2. At least one of the products is an element.3. The original solid is not an element.O1 onlyO 2 onlyO 3 onlyO 1 and 21, 2, and 3 A 7.45 g sample of calcium carbonate completely decomposes into calcium oxide (lime) and carbon dioxidegas when heated. If 4.17 g calcium oxide is produced, what mass of carbon dioxide must have been formed?) 3.28 g31.10 g11.62 g)2.48 g0.56 g

Answer :- 1) only 3 i.e. The original solid is not an element.…

À 7.45 g sample of calcium carbonate completely decomposes into calcium oxide (lime) and carbon dioxide gas when heated. If 4.17 g calcium oxide is produced, what mass of carbon dioxide must have been formed? 3.28 g 31.10 g O 11.62 g 2.48 g 0.56 g

À 7.45 g sample of calcium carbonate completely decomposes into calcium oxide (lime) and carbon dioxide gas when heated. If 4.17 g calcium oxide is produced, what mass of carbon dioxide must have been formed? 3.28 g 31.10 g O 11.62 g 2.48 g 0.56 g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Tin, element 50 on the periodic table, has 10 stable isotopes. 117^Sn makes up 7.687% of naturally…

A: Using the formula moles of Sn117 is calculated as,

Q: A mixture contains both potassium phosphate and potassium chloride. What is the percentage of…

A: The moles of Cu3(PO4)2 in 0.5565 g is, number of moles=given massmolar mass…

Q: When kerosene is burned with oxygen, the products are carbon dioxide and water. If you produce 72…

Q: If 2 moles of water decomposes, the products that will form are 2 moles of hydrogen gas and one mole…

A: Given, Moles of water decomposed = 2 moles.

Q: A container has 5.80 x 1023 molecules (aka atoms) of bromine gas. Calculate the mass (in g) of…

A: Bromine gas = Br2 Molar mass of Diatomic Br2 gas = 159.808 g/mol 6.022 x 1023 molecules mass =…

Q: In a lab experiment, 5.66 g of Mg reacts with sulfur to form 13.13 g of magnesium sulfide. How much…

A: From data find the how much magnesium sulfide would be formed if 5.66 g of Mg were reacted with…

Q: 19.78 mL of bromine contains 6.022 x 1023 bromine molecules. How many bromine atoms are in 3.00 L of…

A: Given -> Volume (V1) = 19.78 ml = 0.01978 L (1L = 1000 ml) Number of bromine molecules in V1=…

Q: Calculate the total number of N atoms in 23.8 g N2O5. O 2.65 x 1023 total N atoms O 9.31 x1023 total…

Q: lithium carbonate contains 18.8 lithium and is used in the treatment of mental illnesses such as…

A: The percent mass composition is also known as the mass percent also called as the percent by weight.…

Q: 5.00 g of copper is reacted with 5.00 g of sulfur in a crucible and a compound composed of copper…

A: Mass percentage of substance is one of the ways to express composition of compounds. Mass percentage…

Q: If you react 5.2 grams of magnesium metals with 2.3 grams of copper (II) bromide, how many total…

A: Given : Mass of magnesium i.e Mg taken = 5.2 g And mass of copper (II) bromide i.e CuBr2 taken = 2.3…

Q: Two elements, R and Q, combine to form two binary compounds A and B. In the compound A, 10.50 g of R…

A: The law of multiple proportions states that if two elements combine with each other to form more…

Q: Two different compounds are obtained by combining nitrogen with oxygen. The first compound results…

Q: When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of FeO and…

A: Amount of iron = 20.00 g Amount of oxygen gas = 11.83 g Atomic weight of iron = 55.847 g We have…

Q: Use the law of conservation of mass to answer the questions. Consider a hypothetical reaction in…

Q: What is the mass of 4.78 x 1024 nitrogen dioxide (NO₂) molecules?

Q: 2.90 grams of phosphorus is burned in the presence of oxygen and forms 5.14 grams of a phosphorus…

A: We can just subtract the mass of the phosphorus from the mass of phosphorus oxide and get mass of…

Q: A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride…

A: Given: mass of P = 12.39 g mass of Cl2 = 42.54 g molar mass of P = 30.97 g/mol molar mass of Cl2 =…

Q: If 50.6 g S is allowed to react as completely as possible with 106.6 g F2 (g), what mass of the…

A: mass of S = 50.6 gatomic mass of S = 32.065 g/molmass of F2 = 106.6 gmolar mass of F2 = 38.00 g/mol

Q: A scientist is trying to discover information about an unknown metal in a compound. The formula for…

A: 1- First calculate the moles of compound XBr3 moles of XBr3 = ( moles of Br ) / 3 moles of XBr3 =…

Q: When methane is burned with oxygen the products are carbon dioxide and water. If you produce 36…

Q: When the substance shown below burns in oxygen, the products are carbon dioxide and water. How many…

Q: 1.The combustion of ammonia in the presence of excets oxygen yields NO, and H20: 4 NH3 (g) + 7 02…

A: 1) Given that : Mass of ammonia = 174 g Mass of oxygen consumed = ?

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: A student is running an experiment in which 48.1 grams of MgBr2 is needed, but the only jar of…

A: Given Mass of MgBr2 needed = 48.1 g

Q: In a laboratory, a 16.1 g of solid aluminum reacts with oxygen gas to produce 37.5 g of Al2O3. After…

A: First balance the chemical equation All step given in Handwritten solution.

Q: Determine the mass in grams of 6.96 × 102¹ atoms of carbon. (The mass of one mole of carbon is 12.01…

A: Mole is defined as mass of substance divide by it's molar mass

Q: A 5.041-g sample of calcium is burned in air to produce a mixture of two ionic compounds, calcium…

A: Given:Calculate the mass of CaO and Ca3N2.

Q: Coal is a leading source of energy for the world. While coal is primarily composed of carbon and…

A: Given:S(s)+O2(g)→SO2(g)

Q: A chemist measures the amount of bromine liquid produced during an experiment. She finds that 658. g…

A: Given: Mass of bromine liquid produced - 658 g To find: number of moles of bromine produced = ?…

Q: 32 g of sulfur will react with 48 g of oxygen to produce 80 g of sulfur troxide. If 20 g of sulfur…

A: Mass of S = 20 gMass of Oxygen(O2) = 100 gMolar mass of S = 32.06 g/molMolar mass of O2 = 32…

Q: There are two gas compounds that are made out of element A and B. This is the mass percentage of…

A: Given: Mass percentage: Compound 1: 30.43% A, 69.57% B Compound 2: 63.64% A, 36.36% B

Q: You wish to prepare 210 grams of 16.3 % Mg(NO3)2 You will need grams of magnesium nitrate and mL of…

A: Given that we have to prepare a 210 grams of 16.3 % MgNO32 solution. Recall the expression of mass…

Q: Solid calcium chloride is formed by the reaction of chlorine gas and solid calcium . Write a…

Q: natural rubidium has the average mass of 85.4678 AMU and is composed of isotopes Rb 85 (mass =…

A: Average atomic mass = ∑i=1XiMiWhere X = mole fraction of the isotope and M is the mass of the…

Q: A nail is coated with a 5.49E-2 cm thick layer of zinc. The surface area of the nail is 8.27 cm2.…

Q: A 0.580 g sample of calsium(Ca) is allowed to burn in 2.530 g of oxygen gas(O2). The sole product is…

Q: Consider the following: 4NH3 + 5O2 → 4NO + 6H2O In an experiment, 5.42 g of NH3 are allowed to…

A: Limiting reagent: It can be defined as by saying that the reagent which used up completely in a…

Q: d) Which of the following substances can be considered chemically pure? • Brass ● ● Seawater Air…

A: Given 5 substances • Brass , • Seawater , • Air , • Apple juice , • A bar of 24-karat gold We…

Q: Two different compounds are obtained by combining nitrogen with oxygen. The first compound results…

A: First we need to calculate the mass ratio of O to N in first and second compound by using the mass…

Q: Determine the mass in grams of 7.75 x 1021 atoms of carbon. (The mass of one mole of carbon is 12.01…

A: Given,the mass of one mole of carbon = 12.01 gNumber of carbon atoms = 7.75×1021 atomsHere, we are…

Q: Dichlorodifluoromethane (CF2CI2) is an Ozone-depleting substance. It belongs to a class of compounds…

A: Atomic Weight of C = 12.01g/mol Atomic mass of Fluorine = 19.0g/mol Atomic mass of Chlorine =…

Q: 15.0 g of iron is allowed to react with air to produce Iron III Oxide. If the reaction is complete,…

A: solution is followed as:

Q: A scientist is trying to discover information about an unknown metal in a compound. The formula for…

A: We have to calculate molar mass of metal and it's identity.

Q: Consider the following table: Substance Density (g/mL) Gold (s) 19.32 Silver (s) 10.49 Lead (s)…

A: Density can be defined as mass divided by volume which is represented as; Density=MassVolume…

Q: In the reaction X + 3 Y 2 Z, the mass of X is 5.0 g and the mass of Z is 14.0 g. If the reaction was…

Q: A student reacted 15.000 g of Lead with 2.325 g Sulfur to form Lead Sulfide. How much grams of Lead…

A: Given: Mass of Pb=15.000 g Mass of S=2.325 g Chemical equation : Pb (s) + S (s) → PbS (s) 1 mol 1…

Question

Heating a certain pure solid completely decomposes it into a solid and a gas, each of
which is also a pure substance. Which of the following is/are reasonable conclusions
regarding these observations?
1. The solid is a compound and the gas is an element.
2. At least one of the products is an element.
3. The original solid is not an element.
O1 only
O 2 only
O 3 only
O 1 and 2
1, 2, and 3

A 7.45 g sample of calcium carbonate completely decomposes into calcium oxide (lime) and carbon dioxide
gas when heated. If 4.17 g calcium oxide is produced, what mass of carbon dioxide must have been formed?
) 3.28 g
31.10 g
11.62 g
)2.48 g
0.56 g

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

SEE SOLUTION Check out a sample Q&A here

Similar questions

What is the mass in grams of 1.75 x 10^24 atoms of silicon? grams How many silicon atoms are there in 32.4 grams of silicon? atoms
A 0.500 g mixture of Cu₂O and CuO contains 0.425 g of Cu. What is the mass of CuO in the mixture? Give 3 sig figs in your answer.
A 1.58 mole sample of a pure unknown substance has a density of 1.87 g/cm3. If the sample occupies a volume of 188. cm3, what is the identity of the substance in the samples? Element Molar Mass Cadmium 112.411 Francium 223.02 Barium 137.327 Terbium 158.925 Molybdenum 95.95 Terbium Molybdenum Cadmium Francium Barium
Use this information to find the molecular formula of x
You wish to prepare 207 grams of 14.7 % Ca(NO3)2. You will need grams of calcium nitrate and mL of water.Assume that the density of water is 1.00 g / ml.
the mass of Cu (63.35 g/mol) used to create Cu2S was 41.95 grams. what theoretical mass of Cu2S (159.16 g/mol) can be produced?
An analytical chemist measures the amount of Elements E₁ and E₂ in four samples of an unknown Substance. sample of E1 1 2 3 mass mass of E2 4 16.0 g 9.1 g 17.1 g 9.8 g 18.5 g 10.6 g 12.0 g 6.9 g It's known that X contains no elements other than E₁ and E₂. Using this information, answer the questions in the table below. Is X a pure substance or a mixture? If you don't have enough information to decide, choose can't decide. If you said X is a pure substance, calculate the mass of Element E₁ the analytical chemist would find in a new 10.0 g sample of X. Round your answer to 2 significant digits. O pure substance O mixture O (can't decide) g
13.0 g of titanium reacted with 60.0 g of bromine. In this reaction, assuming 100% yield, 69.0 g of titanium(IV) bromide were produced and 4.01 g of titanium were left after the reaction. Which reactant was the limiting reactant? Which reactant was the excess reactant? Explain your reasoning using complete sentences.
A student performed an experiment in Lesson 2 (the chemical reaction is shown below). The student's total measured mass of reactants was 14.87 g. Ideally, what should the mass of the products be? Explain your answer using the law of conservation of mass.
When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of FeO and Fe2O3. In a certain experiment, 20.00 g iron metal was reacted with 11.48 g oxygen gas. After the experiment, the iron was totally consumed, and 3.26 g oxygen gas remained. Calculate the amounts of FeO and Fe2O3 formed in this experiment. A, Mass of FeO = B. Mass of Fe2O3 =
One technique used in industry to extract gold from gold sulfide is reacting it with hydrogen gas. In the process, solid gold and hydrogen sulfide gas form. If 337.75 g of gold(III) sulfide is completely reacted in the process, what mass of gold will be produced?
The average mass of one atom of carbon is 2.00 x 10 –23 g. How many carbon atoms are present in a 40.0 g sample of carbon?