The fuel used in many disposable lighters is liquid butane, C4H10. Butane has a molecular weight of 58.1 grams in one mole.  How many carbon atoms are in 2.00 g of butane?

Q: What is the molecular formula of a compound with an empirical formula of CH and a molar mass of 78.1…

A:

Q: The empirical formula for xylene is C4H5(l), and its molar mass is 106 g/mol. What is the molecular…

A: Given :-  Molar mass of xylene = 106 g/mol  Empirical formula = C4H5   To determine :-  Its…

Q: For the reaction C + 2H2 → CH4, how many moles of hydrogen are needed to make  182 grams of methane,…

A: Here a chemical reaction is given that is  C + 2H2 → CH4. Now, we have to calculate how many moles…

Q: The elemental composition of the welding gas acetylene (C2H2) is 92.24% C and 7.76% H by mass. What…

A: Since from the formula of acetylene, we can say that the number of atoms of C and H are same in it.…

Q: 4) How many moles of cesium are in 66.45 g Cs? 5) What is the mass (grams) of 2500. carbon atoms? 6)…

A:

Q: What is the molecular formula of a compound with the empirical formula CH2 if the molecular mass of…

A: Empirical formula is defined as the formula with smallest integral ratio of elements in the…

Q: What is the molecular formula of a compound with the empirical formula CH2 if the molecular mass of…

A: Given : Empirical formula = CH2  And molar mass of compound = 56.10 g/mol

Q: Aspirin has the molecular formula C3HO4. 1. What is the % C in aspirin by mass in aspirin? 2. What…

A: all answers in setp2 2,3,4 and 5

Q: The chemical formula for chlorophyll is C 55 H 22 MgN 4 O 5 a) What is the molar mass of the…

A: Molar mass of a substance is the mass of one mole of that particular substance. The no of moles in a…

Q: A 12.3 g sample of a compound known to consist of only carbon and hydrogen was found to be 14.40 %…

A: Mass of sample = 12.3 g Hydrogen percent by mass = 14.40 % Mass % = Mass of solutemass of…

Q: The fuel used in many disposable lighters is liquid butane, C4H10C4H10. Butane has a molecular…

A: The molar mass of butane is 58.1 g/mol. 1 mole of butane contains 6.023 × 1023 atoms and 1 mole of…

Q: What is the mass in grams of 7.3 x 1024 molecules of lactic acid (C3H6O3), the compound responsible…

A: Given;

Q: If 8.9 x 1025 molecules of CO, are produced in a combustion reaction, what is the mass in kg of CO,…

A: Given:  Number of molecules of carbon dioxide =8.9 x 1025Mass of carbon dioxide produced has to be…

Q: 1. An organic compound was found to contain 54.5% C, 9.2% H, and 36.3% O. a. What is the empirical…

A:

Q: A well-known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula C2HANO. It…

A: The atomic massses are as follows : C: 12 g/mol H: 1 g/mol N: 14 g/mol O: 16 g/mol B : 11 g/mol

Q: the fuel used in many disposable lighters is liquid butane, C4H10. Butane has a molecular weight of…

A: Number of moles of butane is calculated by dividing the amount in grams by molar mass.

Q: The fuel used in many disposable lighters is liquid butane, C4H10C4H10. Butane has a molecular…

A: In one mole of butane C4H10 total 4 mole of carbonatoms are present .→ No of atoms in 4 mole of…

Q: Consider a sample of calcium carbonate, CaCO3 (100.09 g/mol), in the form of a cube measuring 2.88.…

A: The length of the cube of calcium carbonate, CaCO3 =2.88 cm The density of the calcium carbonate,…

Q: Consider the chemical reaction: aCH4+bO2→cCO2+dH2O

A: Balancing of a chemical equation.

Q: A sample of rubbing alcohol solution contains ethanol, C2H5OH(l). If the sample contains 1.25 × 1023…

A: Given;

Q: The chemical formula for chlorophyll is C₅₅H₇₂MgN₄O₅. Given the molar mass of the compound is 893.49…

A: Given, mass of C₅₅H₇₂MgN₄O₅. = 1.501 g Molar mass of C₅₅H₇₂MgN₄O₅. = 893.49 g/mol  Number of moles =…

Q: How many molecules of CO2 are there in 98.3 grams?

A: 1 mole of any compound contains Avogadro number6.022×1023 of molecules.We have to find number of CO2…

Q: A well-known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula C2H4NO. If…

A:

Q: For many years the extraction of gold-that is, the separation of gold from other materials-involved…

A: P

Q: the mass, in grams, of 112 atoms of iron, Fe (1 mol of Fe has a mass of 55.85 g).

A:

Q: the formula for disulfiram decafluoride is S2F10   A.How many molecules are in 1.35 grams of…

A: A.

Q: EDTA, which is short for ethylenediaminetetraacetic acid, is a chemical used in the textile industry…

A:

Q: Ethylene glycol, the substance used in automobile antifreeze, is composed of 38.7% C, 9.7% H, and…

A: Let us assume we have 100 g of Ethylene glycol, then percentages become grams as follows –  mass of…

Q: A compound contains 39.0 % C, 6.72 % H and 53.4 % O by mass. a) What is its empirical formula? b)…

A: Given:  A compound contains 39.0 % C, 6.72 % H and 53.4 % O by mass which means that 100 g of a…

Q: Prevacid is used to treat gastroesophageal reflux disease (GERD). The chemical formula of Prevacid…

A:

Q: A 3.06 mg sample of a compound containing carbon, hydrogen, and oxygen underwent combustion…

A: Empirical formula: Formula containing atoms in smallest possible integer ratio Molecular formula:…

Q: How many moles of aspirin, C9H8O4, are in a bottle containing 450 g by weight? (Note: The…

A: Given,  Weight of aspirin is 450 g Atomic weight of C is 12 g/mol. Atomic weight of H is 1 g/mol.…

Q: 3. What is the mass (in kg) of 6.89 x 1025 molecules of CO2? The molar mass of CO2 is 44.01 g/mol.

A:

Q: What is the molecular formula of a compound with an empirical formula of CH20 and a molar mass of…

A: Empirical Formula:- It is the simplest positive integer ratio of atoms present in a compound.…

Q: What is the mass, in grams, of 4.06 1023 molecules of aspirin, C9H8O4?

A: Number of molecules of aspirin = 4.06 × 1023 One mole contains Avogadro’s number of atoms.…

Q: The semi-precious stone turquoise is a hydrate and with the chemical formula CuAl₆(PO₄)₄(OH)₈･4 H₂O.…

A:

Q: A molecular cluster is formed from iron atoms and carbon monoxide (CO) molecules. If the molar mass…

A: The chemical formula of a compound in which elements are present in the simplest whole number molar…

Q: 5. The empirical formula of a compound is CaH10. hat could its molecular formula be 86 6. A compound…

A: SOLUTION [5.] : Empirical formula of a compound = C4H10O So, molecular formula of a compound will be…

Q: If 6.63 × 10−6 mol of a compound has a mass of 2.151 mg, what is the molar mass of the compound?

A: Number of moles is calculated by dividing the given mass with molecular mass.

Q: Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs,…

A:

Q: The chemical formula of blue crystalline substance of hydrated penta-aqua copper II sulphate is…

A: Molecular formula: CuSO4.5H2O Chemical formula: CuH10O9S Molar mass of CuSO4.5H2O = 64 + 10 x 1 + 9…

Q: What

A: Given, The molecules of N2O = 1.37 x 1017 The mass of nitrogen atom has to be calculated.

Q: What is the molar mass of Mg3(PO4)2, a substance formerly used in medicine as an antacid? 251 g…

A:

Q: If the same amount of electricity that is used to produce 500 g copper metal (Cu Cu") is used to…

A:

Q: ron is biologically important in the transport of oxygen by red blood cells from the lungs to the…

A: 2.63 x 1013 red blood cells     2.90 g of iron molar mass Fe = 55.85 g/mol first we will calculate…

Q: The fertilizer ammonium sulphate is prepared by the reaction between ammonia and sulphuric acid.…

A:

Q: 1. Ethanol has a chemical formula of C2H6O. What is its molar mass? 2. How many molecules of the…

A: Ethanol has a chemical formula of C2H6O

Q: If you have 168 grams of C6H12O6 (glucose), how many moles of glucose do you have? How many…

A: The number 6.022 × 1023 indicating the number of atoms or molecules in a mole of any substance is…

Q: The average nicotine (C 10H 14N 2, molar mass 162.3 g/mol) content of a Camel cigarette is 1.93 mg.…

A: Number of moles is given by the ratio of mass of the substance to that of the molar mass of the…

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.