1. A 4.00g sample of iodine was reacted completely with excess bromine. The mass of the compound formed was 11.56g. Determine the empirical formula.

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

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Q: A 18.92 gram sample of copper is heated in the presence of excess fluorine. A metal fluoride is…

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Q: Mass of crucible and cover is 43.92 g. The mass of crucible, cover, and magnesium is 44.62g. Mass of…

A: Empirical formula is the chemical formula  which represents the simple ratio of atoms of constituent…

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

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Q: C. If we desired to make 34.00g of Copper(1) Hydroxide, how many grams of Copper(11) Chloride would…

A: Given :-  Mass of  Copper(II) hydroxide, Cu(OH)2 = 34.00 g  Mass of  Copper(II) chloride, CuCl2 = ?…

Q: How can the Percentage Composition be obtained from chemical formulas?

A: Percentage composition is given by, % composition = mass of the elementTotal mass of the…

Q: Suppose a student starts with 2.4185 g of a sand mixture and separates the components into 1.3012 g…

A: The mass percentage is the simplest way of representing the mass of the components present in the…

Q: Mass of watch glass and evaporating dish (g) 52.08 Mass of watch glass, evaporating dish, and Mg…

A: Given- Mass of watch glass and evaporating dish = 52.08 g Mass of watch glass, evaporating dish, and…

Q: If 0.587 g of nickel metal reacts with 1.065 g of chlorine gas, what is the empirical formula of the…

A: Answer :- A] NiCl2 Product formed in the is independent of the moles of reactants present as it…

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: Dichloroethane, a compound that is often used for dry cleaning, contains carbon, hydrogen, and…

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Q: A compound was analyzed and was found to contain the following percentages of the elements by mass:…

A: Applying steps to determination of empirical formula..

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: A 170.00 g sample of an unidentified compound contains 29.84 g sodium, 67.49 g chromium, and 72.67 g…

A: Given :-  Mass of Na = 29.84 g  Mass of Cr = 67.49 g  Mass of O = 72.67 g  To be determined :-…

Q: A 9.478 gram sample of iron is heated in the presence of excess fluorine. A metal fluoride is formed…

A: The empirical formula represents the simplest whole number ratio of elements present in a compound.

Q: A 6.117gram sample of cobalt is heated in the presence of excess fluorine. A metal fluoride is…

A: We have to predict the formula for metal fluoride.

Q: A compound of copper was formed when 1.643 g of Cu was heated in oxygen. The mass of the compound…

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

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Q: Determination of a chemical formula, mass of crucible is 14.9234g, crucible + hydrated  sample is…

A: Mass of hydrated sample =( Mass of crucible + hydrated sample) - Mass of crucible

Q: A compound is 22.76% Carbon, 68.30% Boron and 8.93% Hydrogen by mass. What is this compound’s…

A: The given percentage of different elements firstly changed into moles by deviding it by atomic…

Q: When 56.39 g of phosphorus pentachloride reacts with excess water, what mass of hydrogen chloride…

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Q: A molecular substance contains only carbon and hydrogen and has an empirical formula of C15H9 and a…

A: Empirical formula The empirical formula is the molecular formula of the compound that represents the…

Q: An empirical formula can be defined as: A)The exact number of atoms in a compound. B) The formula…

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Q: A 4.560 g sample containing impure CuCl2x2H2O was heated to constant mass. The sample mass after…

A: Here, impure sample of CuCl2.2H2O heated to drive off all the water then the mass of the mixture is…

Q: A white powder is analyzed and found to contain 43.64% phosphorus, and 56.36% oxygen by mass. The…

A: Given: Percent by mass of P = 43.64 % Percent by mass of O = 56.36 % And molar mass of compound =…

Q: 4. Potassium permanganate Туре of Atoms Amount of Total each atom amount Mass of each Formula Total…

A: Given :  To find the type of atoms and total molar mass for the following compounds. 1. KMnO4  2.…

Q: Determining the Formula of a Hydrate #1: A 15.67 g sample of a hydrate of magnesium carbonate was…

A: Given :  Mass of sample of a hydrate of magnesium carbonate = 15.67 g Mass of sample after drying it…

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: You have a compound that is 79.9% C and 20.1% H by mass. a. Determine the empirical formula.

A: Given information,   Compound with 79.9% C and 20.1% H by mass.

Q: 0.474g of nitrogen were reacted with oxygen, the resulting mass was 0.745g. What is the empirical…

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

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Q: mass of 1.2 × 10^23 atoms of phosphorus (molar mass= 31 gm/mo

A: The one mole of a substance contains 6.022×1023 number of its atoms.here moles of…

Q: On a weight basis, a compound is 39.1% car- bon, 52.2% oxygen and the rest is hydrogen. What is the…

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Q: Tin reacts with sulfur in a reaction similar to the reaction of copper and sulfur. A student heats…

A: Given :-A student heat 2.83 gm of tin metal with excesssulphur and obtains a product with a find…

Q: What is the empirical formula for this compound?

A: Number of moles = mass/molar mass  Molar mass of Oxygen = 16 g/mol  Molar mass of nitrogen = 14…

Q: A sample of a pure compound contains 68.4% chromium and 31.6% oxygen by mass. What is the empirical…

A: Let the mass of the pure compound be 100 g. Thus, mass of chromium in the compound is = 68.4 % x 100…

Q: and

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Q: 4. What is the mass percent composition? Why is it useful?

A: Mass percent of each type of element in a compound is called the mass percent composition of the…

Q: A student, Ken, is given a mixture containing two carbonate compounds. The mixture includes MgCO,…

A: Given: Percent by mass of CO32- ions in sample = 69.14 %

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

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Q: Completé the föllóWing tåbles. Mass of Sample Moles of Sample Molecules in Sample Total Atoms in…

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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: 0.374g of phosphorous was reacted with chlorine, the resulting mass was 2.515g. What is the…

A: Given that -  Mass of phosphorus = 0.374 g  Mass of produced Phosphorus Chloride = 2.515 g  Then,…

Q: Barium and sulfur react with each other in a synthesis reaction. If 0.7850 g of sulfur reacts with…

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Q: A compound that contains only carbon, hydrogen, and oxygen is 68.84%  and 4.95%  by mass. What is…

A: The solution for this question is provided considering the compound contains carbon, hydrogen, and…

Q: What is the empirical formula of this mineral

A: Empirical formula is lowest whole number ratio of elements in compound. Sometimes empirical formula…

Q: C. A compound has been found to contain 38.8% K, 29.4% Mn by mass. The remainder of the compound is…

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Q: A 1.271 g sample of aluminum metal is heated in a chlorine gas atmosphere, and the mass of aluminum…

A: We can calculate the mass of the chlorine from the mass of aluminium chloride and the mass of…

Q: in 17.83 moles of carbon dioxide?

A: Molar mass(MM) of CO2 = 12 + 2×16 = 32 g Moles = mass/MM Mass = moles × MM   = 17.83×44 = 784.5 g

Q: Consider the compound QX3, where Q has a molar mass of 42.11 g/mol and X is 15.07 g/mol. A hydrate…

A: i) First you have to calculate the molecular weight of the QX3 ii) Then consider you took 100g of…