A 9.478 gram sample of iron is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of 15.93 g. Determine the empirical formula of the metal fluoride.

Q: 1. A term used to describe the amount of substance. 2. The relationship between the mass or quantity…

A: In chemistry and every other scientific or engineering subject a long term is given a specific name…

Q: 1. A platinum (II) compound , which is used to treat tumors, contains 65.0% Pt., 23.6% Cl, 9.35% N,…

A: As you have asked multiple question we will solve the first one for you .If you want answer to 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 18.92 gram sample of copper is heated in the presence of excess fluorine. A metal fluoride is…

A:

Q: 0.172 g of Mn was heated in the presence of oxygen to make 0.272 g of MnxOy.  Based on this data,…

A:

Q: A sample of phosphorous is placed in a 10.05 g crucible and gives 10.24 g then heated red hot to…

A: Mass of empty crucible =10.05g Mass of phosphorus  + crucible =10.24 g Mass of phosphorus oxide +…

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: Many fertilizers contain ammonium phosphate as a source of phosphorus and nitrogen. A 8.22 g sample…

A:

Q: Suppose that 6.71 × 10³ g of titanium(IV) chloride is reacted with 2.45 × 10° g of oxygen. Calculate…

A:

Q: 19. A sample of a compound contains 19.97g Ti and 13.37g O. Determine the empirical formula of the…

A: To find empirical formula, first we will calculate the moles of each element present in that…

Q: Calculate the empirical formula for 1.386 g Zn, 5.381 I

A: Given,

Q: A chemist is given a sample of the CuSO4 hydrate and asked to determine the empirical formula of it.…

A: Given,  Mass of hydrated CuSO4 = 42.75 g Mass of Unhydrated salt = 27.38 g  Formula of hydrate = ?

Q: 2.40 kg nitrogen reacts with 0.500 kg hydrogen to produce ammonia.  Calculate the grams of ammonia…

A: Reaction between Nitrogen and Hydrogen gas take place to produce ammonia as follows;   N2  + 3H2…

Q: A 6.032 gram sample of chromium is heated in the presence of excess bromine. A metal bromide is…

A:

Q: Describe the process of Interconverting Masses and Moles?

A: Moles of a substance = given mass of substancemolar mass of substance  Mass of a substance = moles…

Q: A 20.97 gram sample of cobalt is heated in the presence of excess fluorine. A metal fluoride is…

A:

Q: A sample of an oxide of vanadium weighing 4.589 g was reduced with hydrogen gas to form water and…

A: Given : Mass of initial vanadium oxide used = 4.589 g Mass of another vanadium oxide formed = 3.782…

Q: A 21.21 gram sample of iron is heated in the presence of excess iodine. A metal iodide is formed…

A:

Q: A compound was found by elemental analysis to contain 39.96 % carbon, 13.42 % hydrogen, and 46.62 %…

A: Molecular formula is the formula of the molecule in which all the atoms are represented with number…

Q: A flask contains 0.490 mol of liquid bromine, Br2Br2. Determine the number of bromine molecules…

A:

Q: If 2.50 g of aluminum metal is heated in Fluorine gas it’s found that 5.28g will combine with…

A: Given data,  Mass of aluminium = 2.50 g  Mass of F = 5.28 g

Q: Calculate the mass percentage of each element in vanadium (III) acetate.

A: Given :- name of compound = vanadium (III) acetate  To calculate :- mass percentage of each element

Q: If 27.0 g of iron nail was used to react with oxygen gas (O2). Calculate the mass of ferric oxide…

A: Iron nails react with oxygen to form ferric oxide. According to the balanced equation, 4 moles react…

Q: A 16.14 gram sample of chromium is heated in the presence of excess sulfur. A metal sulfide is…

A: Mass of chromium sample is 16.14 g Mass of metal sulfide is 26.09 g Calculate the moles of chromium,…

Q: A sample of an oxide of vanadium weighing 4.589 g was reduced with hydrogen gas to form water and…

A: Solution :    The empirical formula gives the simple whole-number ratio of elements present in a…

Q: A 4.67 g sample of a pure strontium halide reacts with excess sulfuric acid, and the solid strontium…

A: Given, A 4.67 g sample of a pure strontium halide reacts with excess sulfuric acid, and the solid…

Q: Calculate the number of moles of potassium ions in a 25.0 g sample of potassium oxide

A: Here, we have to calculate the number of moles of potassium ions in a 25.0 g sample of potassium…

Q: A 2.45g sample of strontium completely reacts with oxygen to form 2.89g of strontium oxide. Use the…

A: Since the reaction taking place can be written as, strontium  + oxygen  ----->  strontium oxide…

Q: A compound having an approximate molar mass of 150.0–155.0 g has the following percentage…

A: The question is based on the concept of elemental analysis. we have been given percentage of…

Q: Calculate the mass (in g) of sample. 1 glucose molecule (C6H12O6)

A:

Q: 1.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A:

Q: A sample compound contains 19.97g Ti and 13.37g O. Determine the empirical formula of the compound.

A:

Q: In a reaction involving manganese, Mn and sulfur, S it was determined that 0.549 g of manganese…

A: First we convert the mass sulfur and manganese to Moles. By this moles of Mn & S  , we have to…

Q: Coke is an impure form of carbon that is often used in the industrial production of metals from…

A: Given: percentage of carbon by mass = 95% Mass of copper(II) oxide = 1.0 ton To find: The mass of…

Q: . Aluminum metal is produced by passing an electric current through a solution of aluminum oxide…

A:

Q: An acid, HEl, is formed from a hypothetical element, El, and a subsequent aqueous solution is…

A:

Q: How many grams of oxygen does it contain? What is the percentage by mass of nitrogen in the…

A:

Q: A piece of aluminum foil 1.00 cm square and 0.570 mm thick is allowed to react with bromine to form…

A: Using the given area and thickness, find the volume of aluminum foil.

Q: A 22.15 gram sample of cobalt is heated in the presence of excess oxygen. A metal oxide is formed…

A:

Q: When 0.273 g Mg is heated in a nitrogen atmosphere, a chemical reaction occurs. The mass of the…

A: We have given that  When 0.273 g Mg is heated in a nitrogen atmosphere, a chemical reaction occurs.…

Q: An impure sample of table salt (NaCl) that was dissolved in water and treated with silver nitrate to…

A: Mass of the impure sample = 1.741 g  Mass of AgCl formed = 4.084 g

Q: A sample of an oxide of vanadium weighing 4.589g was reduced with hydrogen gas to form water and…

A: The empirical formula represents the number of atoms in the molecule with the smallest positive…

Q: 6.778 X 102 vanadium (V) ions react with 15.001 grams of magnesium metal producing vanadium metal…

A:

Q: Calculate the maximum yield of sodium sulfate in grams: Mass = g Na,SO4

A:

Q: If 2.952 g of copper(II) nitrate is reacted with sufficient sodium hydroxide, how much copper (II)…

A: The balanced reaction of copper (II) nitrate with sodium hydroxide can be given as

Q: An acid, HEl, is formed from a hypothetical element, El, and a subsequent aqueous solution is…

A: The number of moles of compound is given by the expression: Number of moles=Given mass of…

Q: An acid, HEl, is formed from a hypothetical element, El, and a subsequent aqueous solution is…

A: Given, Mass percentage of acid, HEI = 20.09%  Atomic Mass: H: 1.00784 g/mol O: 15.999 g/mol El:…

Q: Determine the maximum mass of lithium nitride that could be formed from a reaction involving 5.00 g…

A: Lithium ⇒LiNitrogen ⇒N2Lithium Nitride ⇒Li3N

Q: Calculate the percentage by mass of magnesium in magnesium sulphate (MGSO4). 24 +32 +16 ×4 = 120 .

A: Introduction The percentage by mass of any element that is available in any particular compound can…

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.