When 0.2004 g of calcium is heated in pure nitrogen gas, the sample gains 0.04670 g of nitrogen. Calculate the empirical formula of the calcium nitride formed.

Q: List three ways compositional data may be given in a prob-lem that involves finding an empirical…

A: An empirical formula is derived from the following compositional data The data having information…

Q: What is the mass to mass stoichiometry calculation of Boric Acid ?

A: The explanation is given below-

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

A:

Q: A 0.4647 g sample of CxHyOz was burned. The combustion produced .8635 g CO, and 0.1767 g H,O.…

A:

Q: How many conversions are needed to go from mass (g) of the given to Mole (Y) of the find ?

A: We have been asked to find the no. Of steps needed to go from mass to mole of a compound.

Q: A compound consisting of B, N, and H undergoes elemental analysis. The % composition by mass is…

A: Given,Percent of B in the compound = 40.28 %Percent of N in the compound = 52.20 %Percent of H in…

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: Combustion of a 1.505 g sample of thiophene, a carbon–hydrogen–sulfur compound,yields 3.149 g 0.645…

A: Thiophene is composed of carbon, hydrogen, and sulfur. On combustion, it will give carbon dioxide,…

Q: A compound containing nitrogen and oxygen is decom-posed in the laboratory and produces 1.78 g of…

A: Given data contains, Mass of nitrogen is 1.78 g. Mass of oxygen is 4.05 g.

Q: in a combustion analysis,0.0300 moles of element R reacts with 0.0350 moles of oxygen gas.Determine…

A: Given : moles of element R = 0.0300                                   moles of oxygen gas = 0.0350…

Q: Calculate the percentage by mass of the indicated element in the following compounds: oxygen in…

A: Molar mass of SO2 is 64.06 g/mol Atomic mass of Oxygen is 16.00 g/mol

Q: An organic compound consists of carbon, hydrogen and nitrogenonly. Complete combustion of a 150. mg…

A: Answer:- This question is answered by using the simple concept of determination of empirical formula…

Q: A sample of histamine having a mass of 385mg is composed of 208mg of carbon, 31mg of hydrogen, and…

A: Molecular formula: In a molecular formula we describe the number of atoms of all the elements…

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: How many moles of H2 would be produced

A: Given :- number of moles of Al = 16.0 mol To calculate :- number of moles of H2 produced

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…

A:

Q: Calculate the molar mass of a compound if 0.460 mole of it has a mass of 385.0 g.

A: Given :-  No.of moles of compound = 0.460 mol  Mass of compound = 385.0 g  To calculate :-  Molar…

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

A:

Q: A 0.700 g sample of phosphorous is reacted with excess oxygen to form a product with a mass of 1.604…

A:

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

A:

Q: Consider the chemical reaction N2 + 3H2 = 2NH3    If one begins with 0.25 mole N2  and excess…

A:

Q: When aluminum metal is placed into hydrochloric acid (HCl), aluminum chloride and hydrogen gas are…

A: Here we are required to find the mass of HCl needed to produce 2.02gm of hydrogen gas

Q: A compound was decomposed and determined to be 51.27 % C, 7.75% H and 40.98 %O  by mass.  What is…

A: Given  C%   = 51.27 % H     = 7.75 %  O     = 40.98 %  Subscript of Carbon in Empirical Formula   =…

Q: How many molecules (not moles) of NH3 are produced from 7.42×10−4 g of H2?

A: To obtain the number of molecules, first of all the reaction for the production of NH3 should be…

Q: Consider the balanced chemical reaction below. What is the maximum amount of grams of Fe that can be…

A: The limiting reagent in a chemical reaction is a reactant that is totally consumed when the chemical…

Q: Calculate the mass in g corresponding to 7.500 mol NH3.

A: The Answer to the following question is given as:

Q: When 2.004 g calcium is heated in pure nitrogen gas, the sample gains .4670 g of nitrogen. Calculate…

A: Mass of Calcium = 2.004 g Atomic mass of calcium= 40g/mol Moles of calcium = 2.004g/40g/mol = 0.0501…

Q: How many molecules (not moles) of NH3 are produced from 5.01×10−4 g of H2?

A: Calculate the number of moles of hydrogen gas. The molar mass of hydrogen gas is 2g/mol.

Q: What mass in grams of TNT can be made from 598 g C7H8?

A:

Q: In a lab experiment, 7.97 g of phosphorus reacts with bromine to form 69.65 g of phosphorus…

A: When mole fraction of element is multiply by 100 we obtained percentage by mass .

Q: A 0.025-g sample of a compound composed of boron and hydrogen, with a molecular mass of ~28 amu,…

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

Q: 0.238g of carbon were burned in the presence of oxygen, the resulting mass was 0.872g. What is the…

A: Amount of carbon = 0.238 g Amount of product = 0.872 g Carbon + Oxygen → Product

Q: cumene is compound comtaining only carbon and hydrogen that is used in the production of acetone and…

A: Interpretation: The range of molar mass of cumene that contains only carbon and hydrogen is given.…

Q: What is the simplest or empirical formula of a compound which is found to have a mole ratio    of…

A: Given;

Q: A chemical reaction occurs when 0.378g of Mg is heated in a Nitrogen environment. The product of the…

A: Mass of mg = 0.378 g Mass of product = 0.456 g

Q: . Calculate the mass of manganese(II) carbonate

A:

Q: Determine the molar mass of a substance if 0.290 moles has a mass of 152 g.

A: Molar mass of a substance is defined  as mass of 1 mol lf that substance. Molar mass = mass /moles

Q: A 2.20 g sample of an oxide of bromine is converted to 3.692 g of AgBr. Calculate the empirical…

A: Step : 1         Calculate the empirical formula of the oxide.

Q: The characteristic odor of decaying flesh is due to the presence of various nitrogen-containing…

A: The molar mass of any substance is the mass present in one mole of the substance and the molecular…

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

A:

Q: when 2.004 G of calcium is heated  in pure nitrogen gas the sample gains 0.4670 G of nitrogen.…

A: It is given that, Mass of calcium = 2.004 g Mass of nitrogen gained = 0.4670 g We need to determine…

Q: In a reaction to produce ammonia, the theoretical yield is 420.0 g. What is the percent yield if the…

A: Percent yield of the reaction is equal to the ratio of actual yield and theoretical yield multiplied…

Q: Calculate the number of grams Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen

A: The reaction taking place will be  6 Li + N2 -----> 2 Li3N hence from the above reaction we can…

Q: Enter your answer in the provided bex. Calculate the molar mass of a compound if 0.382 mole of it…

A: This question is related to stoichiometry which determines the quantitative relationship between…

Q: molar mass

A:

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

A:

Q: A 16.35mg sample of unknown compound A produced 48.05mg of CO2 and 14.05mg of H2O when subjected to…

A:

Q: Barium and phosphorus react with each other in a synthesis reaction. If 0.2856 g of phosphorus…

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.