Convert the mass of zinc in the data table into moles of zinc using the atomicmass of zinc.Data TableMass of Zn HCI Volume Tinitial final0.55 g100.0 mL20.0 °C 23.1°CHow many moles of zinc were used?O a. 0.0084 mol ZnO b. 0.55 mol ZnO c. 65.39 mol ZnData TableMass of Zn HCI Volume Tinitial Tfinal0.55 g100.0 mL20.0 °C 23.1°CThe density of the 6M HCI is 1.07 g/mL. Which of the following shows how toconvert the volume of the solution used into grams of solution?O a.100.0 mL x1ml1.07 gO b. 1.07 g100.0 mLOC.1.07 g100.0 mL x1ml

We have given that Mass of of zinc = 0.55g Molar mass of Zinc = 65.38g/mole No of mole = Given…

Convert the mass of zinc in the data table into moles of zinc using the atomic mass of zinc. Data Table Mass of Zn HCI Volume Tinitial Tfinal 0.55 g 100.0 ml 20.0 °C 23.1°C How many moles of zinc were used?

Convert the mass of zinc in the data table into moles of zinc using the atomic mass of zinc. Data Table Mass of Zn HCI Volume Tinitial Tfinal 0.55 g 100.0 ml 20.0 °C 23.1°C How many moles of zinc were used?

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter8: Chemical Composition

Section: Chapter Questions

Problem 120AP

See similar textbooks

Related questions

Q: The following equations represent chemical reactions. Chemical Reactions 1 2Na + 2H2O 2 H2 + O2 +…

A: The reaction which is blance follows law of conservation of mass i.e total mass remains same or…

Q: In the chemical formula Mg(NO3)2, the numerical coefficient is equal to…

A: Chemical formula are representation of molecules or compounds by fixed proportions of elements in…

Q: Which of the following shows a correct setup? O1.45 mol Ca x- 40 g Ca X1 mol Ca O1.45 mol Ca x Са хт…

Q: Using the periodic table for this course (Chem 100 Periodic Table.pdf ), which substance contains…

Q: Identify the choice that best completes the statement or answers the question. Analysis of a…

A: According to law of constant proportion, the ratio of mass of elements in any fixed compound will…

Q: Without doing any calculations, determine which sample contains the most atoms.(a) one gram of…

A: Given; The mass of cobalt (Co) = 1 g The mass of carbon (C) = 1 g The mass of lead (Pb) = 1 g The…

Q: What is the mass, in grams, of 1.51 ×-1018 atoms of gold present in one nanoparticle? eTextbook and…

A: Given: Number of gold atoms = 1.51 × 1018 atoms.

Q: 2) a) Write formulas for the figures. Dark circles represent element A and light circles represent…

A: Atomic element : Atomic element have single atoms as their basic unit. Molecular element : The…

Q: The cullinan diamond was the largest natural diamond ever found (january 25 , 1905 25, 1905). It…

A: Use formulas Mole=mass÷molar mass Total atoms=mole×6×1023 MOLAR mass of diamond= 12g/mol

Q: An electric current is passed through 60.0 mL of water (H2O). This converts the water into 53.33 g…

A: Given Volume of water = 60 mL Mass of Oxygen = 53.33 gram Mass of hydrogen gas = 6.67 gram…

Q: A molecule has a mass of 4.65 x 10^-23 g. Provide two possible chemical formulas for such a…

A: Given mass of 1 molecule = 4.65 x 10-23 g we know mass of 1 molecule = 1 mole 1 mole = 6.022 x…

Q: In a series of experiments, a chemist prepared three differentcompounds that contain only iodine and…

Q: Atomic # 7 Atomic # Atomic # Atomic # Atomic Mass 14 Atomic Mass 12 Atomic Mass_40 Atomic Mass 5e 2e…

Q: Tia has a sample of pure gold (Au). She weighed the sample and the result was 96.896.8 grams. Tia…

A: Formula used: Moles = Mass/ Molar Mass Number of atoms = Moles x Avagadro Number

Q: What is the mass of a 12.56L sample of carbon dioxide? A. 17.9 g B. 8.9 g C. 4501 g D. 24.7 g

A: 22.4 L of CO2 = 44g 1L of CO2=44/22.4g 12.56 L of CO2= 44*12.56/22.4 12.56 L of CO2=24.7g

Q: A student has a sample of zinc that weighs 22.19 g How many zinc atoms are in this

A: Given :- mass of Zn = 22.19 g To be calculated :- number of Zn atoms molar mass of Zn = 65.38…

Q: A sample of trifluoroacetic acid, C2HF3O2, contains 32.1 g of oxygen. Calculate the mass of the…

A: Given, Mass of O in a sample of C2HF3O2 = 32.1 g Calculate the mass of C2HF3O2 sample = ?

Q: What is the mass of 4.50 x 1022 cu atoms? Multiple Choice O 747 x 102 amu O 747 x 1029 4.75 g

Q: Convert 1.89 • 1024 atoms of carbon to coles of carbon

A: Given, the number of moles of carbon atoms = 1.89 x 1024 atoms 1 moles of carbon atom = 6.022 x 1023…

Q: Calculate the number of atoms in each element.a. 25.8 g of Hg c. 150 g of Arb. 0.0340…

A: a. 25.8 g of Hg = Molar mass of Hg = 200.59g/mol Mass of Hg = 25.8g Now, the number of atoms in Hg…

Q: Atoms are the smallest spherical particles that make up any matter. If 6.0x10^23 atoms of aluminum…

A: Avogadro’s number is used to determine the number of atoms present in 1 mol of an element.…

Q: 6. (ii) One coin has a mass of 5.00g and contains 84.0% of copper, by mass. Calculate the number of…

A: Mass of one coin is = 5.00 g The percent of Cu in the coin is = 84.0 % The number of copper atoms in…

Q: How many atoms of He can a balloon that has a 19 cm diameter hold? The density of Helium is 1.18…

A: Given data,Diameter of balloon=19cmRadius of balloon=19cm2=9.5cmDensity of He=1.18g/L

Q: A 36.41-g sample of calcium carbonate (CaCO3 ) contains 14.58 g of calcium and 4.36 g of carbon.…

A: Given data: Mass of CaCO3 sample = 36.41 g Mass of calcium = 14.58 g Mass of carbon = 4.36 Formula…

Q: A piece of aluminum foil measuring 11.20 cm × 6.00 cm × 0.566 mmis dissolved in excess HCl(aq). What…

A: Given, Aluminium foil measuring = 11.20 cm × 6.00 cm × 0.566 mm Density for Al = 2.70 g/cm3 Volume…

Q: Write the chemical formula for each compound, and then calculate the amount in moles in each sample.…

A: Given: Mass of copper(II) sulfate pentahydrate = 78.1 kg

Q: Record the number of each atom in the molecule, then record the total number of atoms in the…

A: We have to determine no of element and atoms

Q: Determine the mass (in grams) of aluminum present in 1.07 grams of Al2S3? Do not type units into…

Q: 1. How many grams are present in 12 atoms of Potassium? a. 7.8 grams b. 3.91 x 10-22 grams 39.1…

Q: 1. 6.02 x 1023 is called a. Avogadro's number. b. Newton's C. Aristotle's d. Planck's mass. 2. The…

A: Avogadro's Hypothesis:- 1 mole of substance = 6.02*1023 particle

Q: Jotmest Atoms are the smallest spherical particles that make up any matter. If 6.0x1023 atoms of…

A: Introduction: Atomic mass is an average of the masses of a number of different atoms.It is also…

Q: Atoms are the smallest spherical particles that make up any matter. If 6.0x1023 atoms of aluminum…

A: Step : 1 Calculate the mass of 1 atom of aluminium in picograms.

Q: Use the following information to determine the mass of chlorine combined with the magnesium to two…

A: Given, mass of crucible = 35.1 mass of crucible and magnesium = 38.92 mass of crucible and…

Q: Determine the volume of a carbon sample that contains 2.40 x 1024 atoms and a density of 0.968g/cm3

A: We have given that No.of atom of carbon = 2.40 × 1024 atom Density of sample = 0.968g/cm3 Find…

Q: Determine the number of atoms of C in 24.8 grams of CH1206- atoms 1 3 4 C 7 9. +/- x 100 2. 5

A: Given : Mass of carbon = 24.8 g Compound = C6H12O6 To Find : Number of atoms Solution : Number of…

Q: Data Table 1 Day 2 Mass (g) Day 3 Mass (g) % Change Day 1 Mass (g) Beaker T 0% Acidic 1.73g 1369…

A: The percentage change of mass is as follows.

Q: Find the mass of 1 molecule of NH3 in gram. a. 2.82 x1023 b. 17 C. 10 d. 2.82 x1023

A: We know that 1 mol of any substance contains Avogadro's number of molecules or atoms i.e 6.023 ×…

Q: Tia has a sample of pure gold (Au). She weighed the sample and the result was 84.784.7 grams. Tia…

A: First of all calculate the number of moles of gold by using formula- mole = mass/molar mass then…

Q: Tia has a sample of pure gold (Au). She weighed the sample and the result was 85.2 grams. Tia wants…

A: Find the number of moles of gold present in the given sample. 196.967 g of gold forms 1 mole of…

Q: Calculate the mass percent composition of each of the following Part A. 6.00 g of Si and 5.55 g of O…

Q: A. Sentence Completion. Complete each statement with a word/ concept in the blank of the item. 1. is…

A: The chemical formula defined the number of atoms or the type of atoms present in the compound. The…

Q: Use the mass spectrum of lead shown here to estimate 100% - the atomic mass of lead. Esti- mate the…

A: INTRODUCTION: Mass spectroscopy is defined as the technique used to determine the atomic mass of an…

Q: A student used a piece of aluminum that had a mass of 2.583 grams, and treated according to the same…

A: Given:Mass of Al= 2.583 gramsChemical equation:2 Al(s) + 2 KOH(aq) + 4 H2SO4(aq) + 22 H2O(l) → 2 KAl…

Q: Rank the following according to DECREASING number of S atoms: A. 31.0 g S8 B. 50.0 mL CS2 (density…

A: To rank them, first calculate number of S atoms in each case.

Q: Complete each row of the table below by filling in the missing prefix or missing exponent. -9 1mol…

Concept explainers

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

Question

Convert the mass of zinc in the data table into moles of zinc using the atomic
mass of zinc.
Data Table
Mass of Zn HCI Volume Tinitial final
0.55 g
100.0 mL
20.0 °C 23.1°C
How many moles of zinc were used?
O a. 0.0084 mol Zn
O b. 0.55 mol Zn
O c. 65.39 mol Zn
Data Table
Mass of Zn HCI Volume Tinitial Tfinal
0.55 g
100.0 mL
20.0 °C 23.1°C
The density of the 6M HCI is 1.07 g/mL. Which of the following shows how to
convert the volume of the solution used into grams of solution?
O a.
100.0 mL x
1ml
1.07 g
O b. 1.07 g
100.0 mL
OC.
1.07 g
100.0 mL x
1ml

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

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.

Similar questions

A 0.755-g sample of hydrated copper(II) sulfate CuSo4xH2O was heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO4 ) with a mass of 0.4183 g. Determine the value of x. [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit ofCuSO4 in the hydrated crystal.]
High-density lipoprotein (HDL) cholesterol is the good cholesterol because adequate levels reduce the risk of heart disease and stroke. HDL levels between 40. and 59 mg/dL are typical for a healthy individual. What is this range of HDL cholesterol in units of mol/L? The formula for cholesterol is C27H46O.
When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. :math>C(s)+O2(g)CO2(g) wever, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. :math>2C(s)+O2(g)CO(g) at mass of each product is expected when a 5.00-g sample of pure carbon is burned under each of these conditions?
Use the average atomic masses given inside the front cover of this book to calculate the mass in grains of each of the following samples. l type='a'> 0.251 mole of lithium 1.51 moles of aluminum 8.75102 moles of lead 125 moles of chromium 4.25103 moles of iron 0.000105 mole of magnesium
Calculate the number of atoms of each element present in each of the following samples. l type='a'> 4.2 1 g of water 6.81 g of carbon dioxide 0.000221 g of benzene, C6H6 i>2.26 moles of C12H22O11
How many moles of aluminum are in an aluminum block that meausres 3.00cm x 3.00 cm x 5.00cm? The density of aluminum is 2.70 g/cm3. a. 121.5 moles b. 45 moles c. 6.25 moles d. 27 moles e. 4.5 moles
please complete following table Mass of KNO3 Test tube + KNO3 Test tube only KNO3 only m1g = m0/g = m/g = 9.000 nKNO3= 0.089 mol
One mole of sulfur approximately has a) 6.02214 * 10^23 b) 6.02222 * 10^23
1. How many moles are in each of the given samples? a) 2.50 mL of water (assume density of water is 1.00 g/mL) b) 10.00 mL of acetone (assume density of acetone is 0.7899 g/mL) c) 23.00 mL hydrochloric acid (12N) d) 33.25 g acetylferrocene (MW of acetylferrocene is 228.07 g/mol)