Which of the following could be the empirical formula for a compound? O A. C6H1206 O B. CH3OH O C. Ag2(C2H3O2)2 D. Hg2Cl2

Q: Vhich molecular formula is also an empirical formula? O H202 O C6H1206 C2H4 PCI3

A: It’s explained below:

Q: 4. Calculate moles and atoms in 50 grams of 'S'. 5. Find the weight of 30 moles of H2SO, and find…

A:

Q: 24) Which of the following compounds contains the largest number of atoms? A) 1.00 mole of H,PO, C)…

A:

Q: A compound consists of 4.50 g of nitrogen for every 7.71 g of oxygen and has the same empirical and…

A: The given mass of nitrogen = 4.50 g.The given mass of oxygen = 7.71 g. It is given that compound has…

Q: Only need help with subpart "d"   Use the following data and steps below to calculate the formula…

A: The di-hydrate of copper chloride has the molecular formula, CuCl2.2H2O

Q: 1. a.) How many moles of sodium in 0.46g of sodium? b.) How many atoms of sodium are in 0.46g of…

A: The number of moles (n) of a substance can be calculated as: n=Given massMolar mass······(1) One…

Q: The number of hydrogen atoms in 0.050 mol of C3H3O3 is A) 3.0 x 1022 H atoms. D) 4.8 x 1023 H atoms.…

A: Interpretation: The number of hydrogen atoms in 0.050 mol of C3H8O3 is to be determined.

Q: Number of atoms of C in 9 moles of C4H10 are: O 54.20x10^23 O 216.79x10^23 O 3.74x10^23 O…

A:

Q: 50 Soap, vitamin Cand orange juice The main constituent of soap has a formula C18HON The formula of…

A:

Q: determine the numbers of moles or molecules (or formula units) in each sample: A) 34.0 g sodium…

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

Q: Which pair of compounds have the same empirical formula?  CH and C2H2  C2H6 and CH  C3H8 and C3H…

A: Answer is explained below.

Q: A certain compound is composed of 26.57% potassium, 35.36% chromium and 38.07% oxygen.  Derive the…

A:

Q: Number of atoms of C in 17 moles of C4H10 are: O 24.09x10^23 7.06x10^23 O 409.50x10^23 102.37x10^23

A: Number of atoms of carbon  = carbon atoms × moles × NA

Q: What is the empirical formula for the substance in the figure?   A. S2O6 B. S3O C. SO3 D. SO

A: Given ,  %S= 40.05 % Therefore, %O = 100-40.05 =59.95 %

Q: Q9) How many moles of Cl atoms are in 65.2g of CHCI3 ? a) 15 b)35 c) 30 d) 3.5

A: Provided amount of CHCl3=65.2g Molar mass of CHCl3=119.38g

Q: The empirical formula for the following compound is: ОН HO a. C3H60 O b. C6H1202 O c. C3H50 O d.…

A: Empirical formula means representation of chemical formula in simple molar ratio.

Q: 4. Determine the number of molecules of compounds or atoms for the following. 15.8 mol H2O 9.51 b.…

A: 1 mole of a substance contain 6.022×1023 molecules.

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

A: Given: Compound contains only C, H and O. Mass of compound combusted = 1.000 g. Mass of CO2 produced…

Q: Complete combustion of 2.90 g of a hydrocarbon produced 8.94 g of CO, and 4.12 g of H,O. What is the…

A: Given  Mass of hydrocarbon = 2.90 gram  Mass of CO2  = 8.94 gram  Mass of H2O = 4.12 gram  Empirical…

Q: Which of the following is not true for 1 mole of the compound (CH3)2O?          a.     It contains…

A: 1 mole of a molecular/atomic substance is that amount of the substance which has 6.022×1023…

Q: A Sample of a compound containing only carbon, chlorine, and fluorine was analyzed and found to…

A:

Q: How many moles of fluorine are present in 11.77 g of mercury(II) fluoride? O a. 4.933 101 moles O b.…

A: 1) d  2) MgCr2O7

Q: What is the empirical formula of a compound that contains 72.0% carbon 12.0% hydrogen and 16.0%…

A: We have given percentage of carbon, Hydrogen and oxygen. We have to predict the empirical formula of…

Q: Number of atoms of Carbon in 15 moles of C4H10 are: 90.33x10^23 361.32x10^23 O 6.23x10^23

A:

Q: Number of atoms of C in 10 moles of CAH10 are: O 24.09x10^23 O 240.88x10^23 O 4.15x10^23 O…

A:

Q: MOLES/MOLECULES T04/SO2 If a sample of B10H10Bra is found to contain 1.20 - 1019 B atoms how many…

A:

Q: What is the mass of 29.4 mol of benzene (C6H6)?

A: Mole is a unit of measurement to represent the amount of substance. It can be expressed as,…

Q: A compound is analyzed and found to contain 86.55% boron and 13.45% hydrogen by mass. What is the…

A: Given, Boron contains 86.55% and hydrogen contains 13.45% by mass. Molar mass of Boron B = 10.811…

Q: Which of the following represents an empirical formula? a. C3H6O3 b. N2O2 c. CH4 d. C2H2Br2 e.…

A: The simplest ratio of the elements in the chemical compound is called empirical formula.The ratio…

Q: Which of the compounds have the same empirical formula? (Choose all that apply.) O CH4 O C2H4 O C4H6…

A:

Q: Glycine is an amino acid with the formula C2H5NO2. Determine the number of moles of carbon in 81.39…

A: By using the mole concept we can calculate the number of moles carbon in C2H5NO2

Q: Determine whether or not each chemical formula is an empirical formula or not? Caco3? Ba3(PO4)2?…

A: Chemical formula: In the chemical formula we write the atoms of each element present in the compound…

Q: The formula for nitrogen dioxide is NO₂2. a. How many grams of nitrogen are present in 3.85 moles of…

A: Here, we have to calculate the mass of nitrogen that is present in 3.85 moles of NO2 and the number…

Q: Which substances have the same empirical formula? Explain how you know. Sample Formula 1 CH3OH CH2O…

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

Q: One mole of glucose C_6 H_12 0_6 contains how many hydrogen atoms

A:

Q: 3. Consider the equ: Moles: C8H14 Masses: C8H14

A: First convert mass into mole by dividing molarity mass of H2O  Then use mole-mole relationship…

Q: 4. Determine the number of molecules of compounds or atoms for the following. 15.8 mol H20 9.51 x10…

A: Mole concept: The number of molecules or atoms present in the one mole of the substance is equal to…

Q: Complete combustion of 7.90 g of a hydrocarbon produced 24.2 g of CO, and 11.6 g of H,O. What is the…

A:

Q: Calculate the folowing   1-number of atoms in 6.54 g Be =37 x 1023 atoms 2-number of atoms in 28.0…

A: Number of Moles = (Mass of the Sample)/(Molar Mass)   Number of Atoms or Molecules = (Number of…

Q: The empirical formula a compound of uranjum and fluorine that is composed OF - uranium and 3 2.4%…

A:

Q: 1. Which of the following is an example of an empirical formula? CH4 C6H1206 N306 C2H2 2. Which of…

A: Empirical formula It is the formula with simplest whole number ratio of atoms in a molecule.…

Q: The empirical formula for C12H12N2O3 is O C2H2NO1.5 O C12H12N203 O CHAN1.50 O None of these

A: Empirical formula is defined as the simplest positive integer ratio of atoms present in a compound.…

Q: Complete combustion of 6.70 g of a hydrocarbon produced 21.4 g of CO2 and 7.67 g of H2O. What is the…

A: Empirical formula :-  The simplest formula of a compound which shows only relative number of atoms…

Q: A. Complete the following table for Ca(HCO3)2 of No. Molecules No. of No. of Grams Moles 1.53 5.27 x…

A:

Q: 1.) Which is the empirical formula for the compound below? I. C3H60 1 C6H10O2 X III. C3H50 IV.…

A: The answer is given as follows

Q: A sample of C12H22011 contains 0.4662 moles of carbon atoms. How many moles of hydrogen atoms are in…

A:

Q: sample of propane, C3H8 C 3 H 8 , contains 11.5 moles m o l e s of carbon atoms. How many total…

A: C3 H8 contains 3 carbon and 8 hydrogen . So 1 mole contain 11 mole of atom.

Q: Which of the following represent an empirical formula? O C2H6 CH20 C6H1206 Pb2(C204)4 AlgP3

A: An empirical formula is depicted by the simplest whole number ratio of the various atoms present in…

Q: 11. Determine the empirical formula for the following: (a) a compound made from 32.86% potassium and…

A: In chemistry, the empirical formula of a chemical compound is the simplest whole number ratio of…

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.