1. How many MOLECULES of carbon tetrafluoride are present in 2.25 moles of this compound ?molecules.2. How many MOLES of carbon tetrafluoride are present in 6.76x1022 molecules of this compound ?moles.

The number of moles of a substance is determined as the number of molecules, atoms or ions upon…

Answered: 1. How many MOLECULES of carbon…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter3: Equation, The Mole, And Chemical Formulas

Section: Chapter Questions

Problem 3.11QE

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Similar questions

Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion, hcpLcnc reacts with oxygen to produce carbon dioxide and water. What is the mole ratio that would enable you to calculate the number of moles of oxygen needed to react exactly with a given number of moles of heptene? What mole ratios would you use to calculate how many moles of each product form from a given number of moles of heptene?
How many molecules of C2H4Cl2 can be prepared from 15C2H4 molecules and 8Cl2 molecules?
Consider the following diagram, where atom X is represented by a square and atom Y is represented by a circle. (a) Write the equation for the reaction represented by the diagram. (b) If each circle stands for a mole of Y and each square a mole of X, how many moles of X did one start with? How many moles of Y? (c) Using the same representation described in part (b), how many moles of product are formed? How many moles of X and Y are left unreacted?
What does it mean to say an equation is balanced? Why is it important for an equation to be balanced?
In a chemical reaction, the total number of atoms present after the reaction is complete is (larger than/smaller than/the same as) the total number of atoms present before the reaction began.
What amount (moles) of compound is present in 1.00 g of each of the compounds in Exercise 52?
Considering your answer to Exercise 79, which type of formula, empirical or molecular, can be obtained from elemental analysis that gives percent composition?
itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is C63H88CoN14O14P . A lack of this vita min in the diet can lead to anemia. Cyanocohalamin is the form of the vitamin found in vitamin supplements. l type='a'> What is the molar mass of cyanocobalamin to two decimal places? How many moles of cyanocohalamin molecules are present in 250 mg of cyanocobalamin? What is the mass of 0.60 mole of cyanocobalamin? How many atoms of hydrogen are in 1 .0 mole of cyanocobalamin? What is the mass of 1.0107 molecules of cyanocobalamin? What is the mass (in grams) of one molecule of cyanocobalamin?
What mass of compound is present in 5.00 moles of each of the compounds in Exercise 52?
Calculate the number of molecules present in each of the following samples. l type="a"> 4.75 mmol of phosphine, PH3 i>4.75 g of phosphine, PH3 i>1.25102 g of lead(II) acetate, Pb( CH3 CO2)2 i>1.25 X 10 2 moles of lead(II) acetate, Pb( CH3 CO2)2 i>a sample of benzene, C6H6 , which contains a total of 5.40 moles of carbon
1. How many MOLECULES of water are present in 3.55 moles of this compound? molecules. 2. How many MOLES of water are present in 8.62×1022 molecules of this compound? moles.
1. How many MOLECULES of phosphorus pentachloride are present in 1.34 moles of this compound ? molecules. 2. How many MOLES of phosphorus pentachloride are present in 1.32x1022 molecules of this compound ? moles.

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1. How many MOLECULES of carbon tetrafluoride are present in 2.25 moles of this compound ? molecules. 2. How many MOLES of carbon tetrafluoride are present in 6.76x1022 molecules of this compound ? moles.