Combustion analysis of a hydrocarbon produced 33.01 g CO2 and 13.51 g H2O. Calculate the empirical formula of the hydro- carbon.

Q: A 7.591-g gaseous mixture contains methane (CH₄) and butane (C₄H₁₀). Complete combustion to form…

A: Step-1CH416g + 2O2 → CO2 + 2H2OC4H1058g + 132 O2 → 4CO2 + 5H2O

Q: The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O:…

A: The given reaction is, 4 NH3 (g) + 7 O2 (g)  →   4 NO2 (g)  + 6 H2O (g) The reaction is already…

Q: A compound contains 21.6% Na, 33.3% Cl, and 45.1% O. Write the empirical formula and name the…

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Q: A compound was found to have the following composition by mass: 28.03% Mg, 21.60% Si, 1.16% H, and…

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Q: The molar mass of an alkene is 112.23 g/mol and empirical formula of the alkene is CH2. What is the…

A: The concept used to solve this question is to calculate the molecular formula using the molar mass…

Q: A compound is composed of 73.1 % G e and 26.9 % O. What is the empirical formula?

A: Given : Mass percent of Ge = 73.1 %  And mass percent of O = 26.9 % Since the compound contains only…

Q: 3 FeS2   +  11 O2   →  Fe3O4   +  6 SO3 100 g of iron sulfide was reacted with excess oxygen,…

A: 3 FeS2   +  11 O2   →  Fe3O4   +  6 SO3 Atomic masses Fe=56; S=32, O=16 Molecular mass of…

Q: An unknown hydrocarbon is subjected to elemental analysis. The results of this test show that the…

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Q: By chemical analysis, the composition of potassium phosphate is 55.19% K, 14.63% P, and 30.19% O.…

A: Given data contains, Mass percent of potassium is 55.19%. Mass percent of phosphorus is 14.63%. Mass…

Q: 1. A certain compound is accidentally synthesized by a chemist in a laboratory set-up. He discovers…

A: Number of moles of any substance = mass of substance/molar mass of substance  Mol ratio for…

Q: A compound is decomposed in the laboratory and produces 1.40 g N and 0.20 g H. What is the empirical…

A: The number of moles of N and H present in the compound can be determined as follows: nN = WNMNnN =…

Q: Starting with the following equation, KOH(s) + CO2(g) → K¿CO3(s) + H¿O(1) calculate the mass in…

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Q: The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur…

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Q: Calculate the number of moles of hydrogen peroxide molecules, H2O2, present in a sample containing…

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Q: Calculate the number of moles of propane molecules, C3H8 C 3 H 8 , present in a sample containing…

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Q: Starting with the following equation, Fe₃O₄(s) + CO(g) → Fe(l) + CO₂(g) calculate the mass in grams…

A: Weight of Fe = 575 gm

Q: 1. 84 g of CsH&O6 contains 6.02 x 1023 molecules.

A: Molar mass of C5H8O6 = 5×12 + 8×1+ 6 × 16 = 164 g 1 mol of any substance contains= 6.022×1023…

Q: A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

A: Given,  Mass of CO2 = 2.224 g  H2O = 0.3035 g

Q: What is the Empirical formula of a compound that is 40.0% C, 6.7% H, and 53.3% O

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Q: The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g)…

A: 4 molesNH4 NH3 +702 G4NO24 NO + 6H₂OMy gives a proles Nomole NH₃ gines Imole No.17 g NHg gives 46 gm…

Q: Determine the molecular formula of the compound with an empirical formula of CH and a molar mass of…

A: Given:- Determine the molecular formula of the compound with an empirical formula of CH and a molar…

Q: A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

A: Given: Mass of unknown compound = 1.000 g CO2 formed = 2.224 g H2O formed = 0.3035 g Known: Molar…

Q: compound is 92.2% Carbon and 7.76% Hydrogen. The formula mass of the compound is 78.1 g. Calculate…

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Q: Calculate the molecular formulas of the compounds having the following empirical formulas and molar…

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Q: O CHEMICAL REACTIONS Combustion analysis 6.00 g of a certain Compound X, known to be made of carbon,…

A: Given :  Molar mass of compound X = 78 g/mol  Mass of compound used = 6.00 g  Mass of Carbon dioxide…

Q: What is the empirical formula of a compound that is 40% carbon, 7% hydrogen and 53% oxygen by mass…

A: ANSWER : Option (ii) CH2O is correct answer. Solution: Empirical formula  of a compound = ? that is…

Q: Without using a calculator, arrange these samples in order of increasing numbers of carbon atoms:12…

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Q: 4 KO₂ (s) + 2 CO₂(g) → 2 K₂CO₃(s) + 3 O₂(g) What is the mass in grams of oxygen gas that can be…

A: The balanced reaction given is, => 4 KO2 (s)  + 2 CO2 (g) → 2 K2CO3 (s) + 3 O2 (g) Given: Mass of…

Q: Solve the attached

A: Hello. Since your question has multiple questions, we will solve the first question for you. If you…

Q: Titanium tetrachloride, TiCl4 , is prepared by the reaction below.…

A: Given, Mass of TiO2 = 35g. Mass of Cl2 = 38g. Mass of C = 11g. The balanced reaction for the…

Q: What chemical property of potassium chlorate did you use to design a procedure to determine the…

A: Interpretation-  Tell that chemical property of potassium chlorate which we use to design a…

Q: Caffeine a stimulant found in coffee, tea and chocolate is composed of C, H, N and O. Combustion of…

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Q: The reaction between methanol and oxygen gas produces water vapor and carbon dioxide. 2 CH,OH(1) + 3…

A: From the reaction it is clear that 2 moles methanol and 3 moles oxygen reacts to give 4 moles water…

Q: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 210 g of ammonia consumes __________…

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Q: A compound contains 76.47% Cr and 23.53% O. Calculate the empirical formula. Cr= 52.00 g/mole,  O =…

A: Given :-  Percent composition of Cr = 76.47 %  Percent composition of O = 23.53 %  MM of Cr = 52.00…

Q: What is the empirical formula of the compound?

A: The empirical formula is defined as the lowest whole number ratio of  elements present in a compound

Q: A substance, AzB, has the composition by mass of 60% A and 40%B. What is the composition of AB2 by…

A: Find solution below

Q: 24) Calculate the molar mass of the following compound: ammonia, NH3 A) 15.02 g/mol B) 17.03 g/mol…

A: 24) molar mass of nitrogen = 14.0067 g/mol molar mass of hydrogen = 1.00784 g/mol

Q: A hydrocarbon contains 74.98 % carbon, the remainder hydrogen. Determine the empirical formula of…

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Q: What is the chemical formula of a compound with an empirical formula of CH2O and a molar mass of…

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Q: Elemental analysis of a sample containing only B and H shows that it contains 479.4 g of boron…

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Q: Combustion analysis of a hydrocarbon produces 33.01 g CO2 and 13.51 g H2O. Calculate the empirical…

A: Given: Combustion analysis gives 33.01 g CO2 and 13.51 g H2O.

Q: A compound containing selenium and fluorine is decomposed in the laboratory and produces 2.231 g Se…

A: wt. Of Se obtained = 2.231 g wt. Of  F obtained = 3.221 g Empirical Formula = To be determined

Q: A 2.52-g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur is…

A: The compound contains carbon (C), hydrogen (H), nitrogen (N), oxygen (O) and sulphur (S). In three…

Q: A combustion analysis of 5.214 g of a compound yields 5.34 g CO, 1.09 g HO, and 1.70 g N. If the…

A: Correction: It should be CO2  not CO It should be H2O not HO It should be N2 not N Given, Mass of…

Q: Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen…

A: molar mass of CO2 = 44 g/molmolar mass of carbon = 12 g/mol1 CO2 has 1 C in itmolar mass of H2O = 18…

Q: what is the empirical formula of the compound 330g carbon 55.6g hydrogen 220.2g oxygen

A: Empirical formula represents the simplest whole number ratio of atoms of elements present the…

Q: For many years chloroform (CHC]3) was used as an inhalation anesthetic in spite of the fact that it…

A: The mass percentage of a component in a solution is obtained by using the formula: Mass percent=Mass…

Q: Find the empirical formula for a compound that is 34.59% NA, 23.31% P, and 42.10% O by mass?  2:…

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Q: [References] Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas ( CH4) by the…

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.