(a) Interpretation: The total number of atoms in the given species needs to be calculated. Concept introduction: According to Avogadro’s law , in 1 mol of a substance there are 6.023 × 10 23 atoms. Thus, from number of moles and Avogadro’s number , the number of atoms of an element can be calculated as follows: N = n × N A Here, n is number of moles and N A is Avogadro’s number with a constant value of 6.023 × 10 23 .
(a) Interpretation: The total number of atoms in the given species needs to be calculated. Concept introduction: According to Avogadro’s law , in 1 mol of a substance there are 6.023 × 10 23 atoms. Thus, from number of moles and Avogadro’s number , the number of atoms of an element can be calculated as follows: N = n × N A Here, n is number of moles and N A is Avogadro’s number with a constant value of 6.023 × 10 23 .
Solution Summary: The author explains how Avogadro's law calculates the total number of atoms in a given species.
Definition Definition Number of atoms/molecules present in one mole of any substance. Avogadro's number is a constant. Its value is 6.02214076 × 10 23 per mole.
Chapter 2, Problem 55E
Interpretation Introduction
(a)
Interpretation:
The total number of atoms in the given species needs to be calculated.
Concept introduction:
According to Avogadro’s law, in 1 mol of a substance there are 6.023×1023 atoms. Thus, from number of moles and Avogadro’s number, the number of atoms of an element can be calculated as follows:
N=n×NA
Here, n is number of moles and NA is Avogadro’s number with a constant value of 6.023×1023.
Interpretation Introduction
(b)
Interpretation:
The total number of atoms in the given species needs to be calculated.
Concept introduction:
According to Avogadro’s law, in 1 mol of a substance there are 6.023×1023 atoms. Thus, from number of moles and Avogadro’s number, the number of atoms of an element can be calculated as follows:
N=n×NA
Here, n is number of moles and NA is Avogadro’s number with a constant value of 6.023×1023.
Interpretation Introduction
(c)
Interpretation:
The total number of atoms in the given species needs to be calculated.
Concept introduction:
According to Avogadro’s law, in 1 mol of a substance there are 6.023×1023 atoms. Thus, from number of moles and Avogadro’s number, the number of atoms of an element can be calculated as follows:
N=n×NA
Here, n is number of moles and NA is Avogadro’s number with a constant value of 6.023×1023.
I only need parts B and D, thank you!
The following quantities are placed in a container: 1.98 × 10^24 atoms of hydrogen, 1.32 mol of sulfur, and 113.8 g of diatomic oxygen.
(b) What is the total number of moles of atoms for the three elements?
(c) If the mixture of the three elements formed a compound with molecules that contain two hydrogen atoms, onesulfur atom, and four oxygen atoms, which substance is consumed first?
(d) How many atoms of each remaining element would remain unreacted in the change described in (c)?
9. When a candle has been burning for an hour, its mass is less than it was at the beginning.
(a) How is it possible for the candle to lose mass without violating the law of conservation of mass?
(b) How might you find the mass of the missing material?
14. Hydrochloric acid reacts with zinc. The chemical equation for this reaction is Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq)
a) Classify this reaction.
(b) Name the product that forms bubbles in this reaction. How do you know?
c) How does the mass of zinc metal change as the reaction proceeds?
d) What does the (aq) symbol in the equation mean?
24. Consider this chemical equation: Zn + 2 AgNO3 → Zn(NO3)2 + 2 Ag
a) How many atoms of zinc are on the left side of the equation? How many are on the right?
(b) How many atoms of silver are on the left side of the equation? How many are on the right?
(c) Is the equation balanced? Explain.
25.How are coefficients different from subscripts in equations?
30. Consider this neutralization reaction: HCl +…
(a) What is a hydrocarbon? (b) Butane is the alkane with a chain of four carbon atoms. Write a structural formula for this compound and determine its molecular and empirical formulas.
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY