What is the mass in grams of 6.57 × 10²⁵ molecules of N₂? 7.57 × 10²⁵ molecules of O₂?

Q: If 6.1 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂…

A: Given: 6.1 × 10²⁵ molecules of CO₂ are produced in a combustion reaction.  To determine : The mass…

Q: 1. Sphalerite is a zinc sulfide (ZnS) mineral and an important commercial source of zinc metal. The…

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Q: What is the mass, in grams, of 2.70×10−3 mol of ammonium phosphate?         Express your answer…

A: Molecular Formula and Molar Mass Ammonium phosphate has molecular formula (NH4)3PO4 .  Molar mass of…

Q: How many molecules of hydrogen chloride (HCI) are there in 25.0 g of hydrogen chloride? (Given: H=…

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Q: 5. A 2.000 g sample of CoCl2·xH2O is dried in an oven. When the anhydrous salt is removed from the…

A: By calculating moles of CoCl2 and H2O we can find value of x.

Q: Consider the reaction: ZnO(s) + H20(1) - Zn(OH)2(aq) Given an initial mass of 19.85 g Zno, an excess…

A: The given reaction is, ZnO (s) + H2O (l) →  Zn(OH)2 (aq) Given that: mass of ZnO = 19.85 g To find…

Q: How many grams are in 3.01 × 1024 molecules of (NH4)2SO4?

A: Given,Molecules of NH42SO4 = 3.01 × 1024Required,                   Grams of NH4SO4 .

Q: Write the six (6) conversion factors (ratios) that you can derive from the relations below: 1 mole…

A: The mathematical entity that is employed to convert the units of a substance from one value into…

Q: Table salt, NaCl(s),NaCl(s), and sugar, C12H22O11(s),C12H22O11(s), are accidentally mixed. A 5.50…

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Q: What is the mass in grams of 3.88 × 1025 molecules of Br2?

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Q: e composition of a given substance is as follows: 3.5 mol C, 2.52 g H, 24.0 g O, 01 x1023 atoms of…

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Q: if 9.3×10^25 molecules of CO2 are produced in a combustion reaction , what is the mass in kg of CO2…

A: Applying mole concept and avogadro number.

Q: What is the mass in grams of 4.28 × 10²⁵ molecules of O₂?

A: Given:molecules of O2 = 4.28 × 10²⁵ moleculesRequired: Mass of O2 = ?

Q: Calculate the mass in grams of 3.07×10243.07×1024 molecules of propane. The chemical formula for…

A: Given that : The number of molecules of propane = 3.07×1024 The chemical formula for propane is…

Q: What is the mass, in grams, of 9.47×1024 molecules of methanol (CH3OH)?

A: The number of moles of methanol is calculated as,

Q: Calculate the mass in grams of 6.12 mole Cu(NO3)2.

A: Solution stoichiometry is mainly based on the calculation of moles and volumes. These two values are…

Q: 2Mg(s) + O₂(g) →→→ 2MgO(s) A chemistry student is performing this reaction in a lab, in which…

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Q: Sulfur is used in the production of vulcanized rubber, detergents, dyes, pharmaceuticals,…

A: volume of SO2= 1.3x104 m3 Volume of H2S= 2.5x104m3      as we know 1m 3=1000litre so, volume of…

Q: Balance the following chemical equation CB,H.(g) + O₂(g) - > CO₂(g) + H₂O(g)

A: Is an equation in which the number of atoms for each element in the reaction and the total charged…

Q: A combustion analysis is a technique to find the the empirical formula of compounds. In a combustion…

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Q: If 6.7 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂…

A: Given: The number of molecules of CO₂=6.7 × 10²⁵ molecules The moles of CO₂=(6.7 × 10²⁵ )÷ (6.022 x…

Q: How many grams of carbon are in 1.13 x 1025 molecules of (carbon dixide) CO2 ?

A: Given, Number of molecules of CO2 = 1.13 x 1025  Mass of Carbon (C) = ? Note: molar mass of C =…

Q: Elemental phosphorus reacts with chlorine gas according to the equation P4(s) + 6Cl2(g) --> 4PCl3…

A: The limiting reagent of a chemical reaction is the species which is totally consumed in the course…

Q: Elemental phosphorus reacts with chlorine gas according to the equation P4(s) + 6Cl2 (g)➡️ 4PCl3 (l)…

A: The reaction taking place is given as, => P4 (s) + 6 Cl2 (g) --------> 4 PCl3 (l)  Given :…

Q: The chemical formula for dimethyl ether is: CH;OCH3 Calculate the molar mass of dimethyl ether.…

A: The mass of one mole of a substance is known as molar mass. The molar mass of the sum of the masses…

Q: What is the mass in grams of 5.57 × 10¹⁵ molecules of SO₂?

A: We know that , 1 mole = 6.023x1023molecules/atoms/ions.1 mole = molar mass of molecule .6.023x1023…

Q: How

A: moles of water = ( molecules of water ) / ( Avogadro number )  Where :  Molecules of water is 2.0 •…

Q: How many grams are in 2.38 × 1022 molecules of ammonia (NH3)?

A: Mole=molecuy÷6×1023 Mass=mole×molar mass

Q: The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). What is the mass in grams of…

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Q: What is the mass of 7.004 x 10" molecules of calcium chloride? How many moles are in 9.83 x 10-…

A: Note: According to the rules we can answer only first three parts. Given: Molecules of calcium…

Q: How many grams are in 2.85 x 10^23 molecules of CO2?

A: The question is based on mole concept. we have to calculate mass of carbon dioxide present in the…

Q: A chemist prepares a solution of potassium bromide (KBr) by measuring out 31. mg of KBr into a 100.…

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Q: What is the mass in grams of 4.28x10^22 molecules of water ?

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Q: Determine the molar mass of Al(NO3)3⋅9H2O.

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Q: What is the mass, in grams, of 9.70×1024 molecules of methanol (CH3OH)?

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Q: The chemical formula for octane is: CH3 (CH₂) CH3 Calculate the molar mass of octane. Round your…

A: Since, Molar mass of the compound is the sum of molar mass of each atom present in the molecule.…

Q: What

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

Q: 2Fe(s) + 3Cl2(g) → 2FeCl3(s) Given an initial mass of 11.01 g Fe, an excess of Cl2, and assuming…

A: The number of moles of 11.0 g of Fe is calculated as shown below where 55.845 g/mol is the molar…

Q: If 9.9 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂…

A: 1 mole of a substance has 6.022 ×1023 atoms or molecules. The mass of 1 mole of a substance is equal…

Q: Mass (in grams) of 1.00×10−2 molof CdS. Express the mass in grams to three significant digits.…

A: The mass in grams is calculated for CdS as shown,

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.