1. A 1.31g sample of sulfur was reacted with chlorine to form 4.22g of compound. What is the empirical formula of the compound?

Q: When 2.750 g of the oxide of lead is stronglyheated, it decomposes and produces 0.0640 g of oxygen…

A: The determination of the simplest form of a compound is called its empirical formula. It is…

Q: 5. Analysis of 20.0 g of a compound containing only calcium and bromine indicates that 4.00 g of…

A: Given, The mass of a compound is 20.0 grams The mass of the calcium in the compound is 4.00 grams

Q: A 0.858-g sample of copper was reacted with oxygen to form 1.074 g of copper oxide. Determine the…

A: Given, mass of copper sample = 0.858 g Mass of copper oxide formed = 1.074 g Empirical formula of…

Q: A 0.338-g sample of antimony was completely reacted with 0.295 g of chlorine gas to form antimony…

A:

Q: Why is it important to be able to calculate an empirical formula from experimental data? A. A…

A: Empirical formula of a compound represents the smallest whole number relative ratio of elements in…

Q: A block of pure magnesium metal weighs 76.9 grams. How many moles of magnesium are present in the…

A: Mole= mass of Mg / molar mass of Mg Given - 1) mass of Mg =76.9              2) Molar mass of Mg=…

Q: A 5.41g sample of carbon reacts with hydrogen to form 6.32g of an organic compound. What is the…

A: Empirical formula is written using simplest ratio of elements present in the compound but not the…

Q: What do hybrid orbitals provide?

A: ANSWERE IS DISCUSSED BELOW :

Q: A 13.0-g sample of titanium reacts with oxygen to form 21.6 g of metal oxide. What is the empirical…

A: Given that  Mass of Titanium reacted = 13.0 g  Mass of metal oxide formed = 21.6 g  Empirical…

Q: 12. Complete combustion of 1.550 grams of a compound produces 1.250 grams of carbon dioxide and…

A: Given data :

Q: 2. A 13.07g sample of an unknown compound is composed of 9.48 g of barium, 1.66g of carbon and 1.93…

A: Empirical formula of a compound is denoted by the proportion of numbers of atoms present in the…

Q: completely

A:

Q: 9. A compound of titanium and oxygen has a composition by mass of 60 % Ti and 40 % O. Determine the…

A: In the given questions we are given that titanium is 60% and oxygen is 40%  Means for every 100 g of…

Q: 1. A compound is 48.38% carbon, 8.12% hydrogen, and 53.5% oxygen by mass. Find its empirical…

A:

Q: 5.00 g of a compound containing nitrogen and oxygen was decomposed and 1.52 g of nitrogen was…

A: Given: Mass of compound = 5.00 g  Mass of Nitrogen produced=1.52 g  Molar mass of nitrogen = 28…

Q: If only 15.8 grams of sodium chloride were isolated from the above reaction, what is the percent…

A: Given that :  NaCl produced from reaction = 16.48 g  It means theortical yield of NaCl = 16.48g…

Q: A compound contains arsenic and oxygen as its only elements. A 1.626g sample of the compound…

A: A 1.626 g of the sample contain 1.060 g of arsenicSo, Oxygen = (1.626 -1.060)g…

Q: 17. Complete combustion of 2.90 g of a hydrocarbon produced 8.94 g of CO2 and 4.12 g of H2O. What is…

A:

Q: A student reacted 0.3000 g of aluminum with oxygen gas and obtained 0.5333 g of aluminum oxide.…

A: The empirical formula is the chemical formula of any compound that represents the proportions of…

Q: 1. What do you call to the unit amount of a substance used for measuring large quantities of very…

A: Given:  unit amount of  substance used for measuring large quantities of very small entities such as…

Q: a. A 9.475 gram sample of copper is heated in the presence of excess chlorine. A metal chloride is…

A: Given question related to calculating empirical formula of metal halide formed when metal is heated…

Q: A 2.87 g sample of carbon reacts with hydrogen to form 3.41 g of car fuel. What is the empirical…

A: Given Car Fuel mass= 3.41 g mass of carbon = 2.87 g By the law of definite proportions, Mass of…

Q: An unknown organic compound contains 41.4 % carbon, 3.47 % hydrogen, and 55.1 % oxygen by mass. A…

A: Given data,Percentage of C=41.4%Percentage of H=3.47%Percentage of O=55.1%Moles of compound…

Q: An oxide of gold thermally decomposes. A. 0.204 g sample of oxide is heated, forming 0.182 g of…

A:

Q: An analysis shows that 5.90 g of a chromium metal combines with oxygen to form 8.62 g of chromium…

A:

Q: 59. A 0.5998-g sample of a new compound has been analyzed and found to contain the following masses…

A: Empirical formula can be calculated as follows -  First of all calculate the no. Of moles for each…

Q: 3. A student reacted 0.3000 grams of aluminum with oxygen gas and obtained 0.5333 grams of aluminum…

A: Given : mass of aluminium reacting = 0.3 g and mass of aluminium oxide formed = 0.5333 g

Q: 33. Combustion analysis of a hydrocarbon containing only carbon and hydrogen produces 22.4g of CO2…

A: Given:CO2 formed = 22.4 gH2O formed = 12.6 gKnown:Molar mass of CO2 = 44.011 g/molMolar mass of H2O…

Q: If 0.537 g of copper completely reacts with 0.321 g of fluorine to form a compound, what is the…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume a 100.-g sample of this compound.

A: Stoichiometry allows us to make predictions about the outcomes of chemical reactions. Making useful…

Q: 63. When 3.269 g of zinc is heated in pure oxygen, the sample gains 0.800 g of oxygen in forming the…

A:

Q: A student calculated the number of moles of carbon dioxide present in a 100.0 g sample of a gaseous…

A: Percentage composition of an element is calculated from its molecular mass. Percentage composition…

Q: A student used 1.50 g of manganese to react with excess fluorine to form manganese fluoride. If 4.09…

A:

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.