Question

Option 2:  Kim thinks she’s got Avogadro’s number down, she can use it to get to molecules...

Option 2:  Kim thinks she’s got Avogadro’s number down, she can use it to get to molecules from moles and to moles from molecules, but she runs into a roadblock when they start using atoms within the molecules.  She comes to you with the following problems and wants a step by step explanation of how to solve them.  What conversions would you have her use?  What steps are involved for each one?  How would you explain how these are different from the problems she already understands?

If you have 7.54 x 1025Oxygen atoms in Silver sulfate, what mass of silver sulfate do you have?

If you have 2.89g of Aluminum Hydroxide.  How many moles of Hydrogen do you have in the Aluminum Hydroxide?  How many atoms of Hydrogen is this?

If you have 70.0g of Chloride ions in Calcium chloride, how many molecules of calcium chloride do you have?

Option 3:  Jake is confused about where to start in solving questions about moles, grams, and molecules. He brings you the following problems. Can you teach him HOW to tell these four things for problems A-C?

What the starting information is in each problem.

What they question wants him to solve for.

When to use which conversions.

How to set up the math for each problem

Then walk him through to the solution of each problem.  The problems he is looking to solve are:

How many moles are found in 65.7g of Lithium Sulfate?

How many moles of H are found in 22.5g of Ammonium Acetate?

What mass of water do you have if you have 6.43 x 1028molecules of water?

0 0
Add a comment Improve this question Transcribed image text
Answer #1

1)

Silver sulfate is Ag2SO4 so, number of moles of Ag2SO4 = no. of moles of O atoms/4 (Each molecule contains 4 O atoms)

So, 7.54*1025 O atoms have 7.54*1025/Na moles of atoms = 7.54*1025/6.022*1023 = 125.2 moles of O atoms so, moles of Ag2SO4 = 125.2moles/4 = 31.3 moles

Molar mass of Ag2SO4 = molar mass of Ag*2 + molar mass of S + molar mass of O*4 = 107.8g/mole*2 + 32g/mole + 16g/mole*4 = 311.6 g/mole

So, weight of 31.3 moles of Ag2SO4 = moles* molar mass = 31.3moles*311.6g/mole = 9753 g

2)

Aluminium hydroxide is Al(OH)3 and its molar mass = molar mass of Al + molar mass of O*3 + molar mass of H*3 = 27g/mole + 16g/mole*3 + 1g/mole*3 = 78 g/mole

So, moles of Al(OH)3 in 2.89 g = weight/molar mass = 2.89g/ 78g/mole = 0.037 moles

As each Al(OH)3 molecule contains 3 atoms of H we can say that each mole of Al(OH)3 will contain 3 moles of H atoms so, 0.037 moles of Al(OH)3 will contain 0.037*3 moles of H atoms = 0.111 moles

3)

Atoms in 0.111 moles = moles*Avogadro's constant = 0.111*6.022*1023 = 6.69*1023 H atoms.

4)

Chloride ions are Cl- ions with molar mass = 35.45 g/mole

So, moles of Cl- in 70 g = weight/molar mass = 70g/ 35.45g/mole = 1.97 moles

Calcium chloride is CaCl2

Each molecule of CaCl2 contains two chloride ions (2Cl-) so, 1.97 moles of Cl- will be present in 1.97/2 moles of CaCl2 = 0.987 moles

Molecules of CaCl2 in 0.987 moles = moles*Avogadro's constant = 0.987*6.022*1023 = 5.94*1023 molecules

Add a comment
Know the answer?
Add Answer to:
Option 2:  Kim thinks she’s got Avogadro’s number down, she can use it to get to molecules...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • how do you do this?(please explain with what types of reactions) 10. calcium phosphate plus aluminum...

    how do you do this?(please explain with what types of reactions) 10. calcium phosphate plus aluminum sulfate _11. calcium sulfate plus ammonium nitrate 12. potassium plus fluorine gas 13. sodium chloride electrolyzed to form sodium and chlorine gas 14. silver plus barium 15. Iron (III) hydroxide plus phosphoric acid 16. sodium plus nitric acid 17. iron (III) iodide plus copper (II) 18. copper (1) plus sulfuric acid _19. sodium sulfate plus barium chloride _20. hydrogen gas plus oxygen gas

  • > < Question 2 of 12 The formation of aluminum chloride can be described by the...

    > < Question 2 of 12 The formation of aluminum chloride can be described by the balanced chemical equation. 2 Al+3 Cl, 2 AICI How many moles of Cl, molecules are required to react with 1.61 mol Al atoms? mol Cl moles of CI, required: For the chemical reaction, 2 Al +3 H,SO 3 H, + Al, (SO what mass of sulfuric acid in grams is needed to produce 4.69 mol of aluminum sulfate? mass:

  • 2. Mass-mass problems. Show your work and label your answers. a. How many grams of sulfur...

    2. Mass-mass problems. Show your work and label your answers. a. How many grams of sulfur dioxide are needed to react with 10.0 g of oxygen gas according to the following UNBALANCED reaction? SO2 + O2 → SO3 b. Aluminum reacts with hydrogen sulfate to produce aluminum sulfite and water. If 32.3 grams of aluminum are used, how many grams of aluminum sulfite can be produced? C Hard water contains calcium sulfate and can be softened by adding sodium carbonate...

  • 1) Calculate AH (250°C) for the formation of ammonia gas from nitrogen gas and hydrogen gas...

    1) Calculate AH (250°C) for the formation of ammonia gas from nitrogen gas and hydrogen gas Substance Enthalpy value (kJ/mole) Entropy value K-mole) 1925 1306 191.5 Ammonia gas Hydrogen gas Nitrogen gas (write rxn with phase labels) 1) Calculate the standard Enthalpy change at 25.0°C Gaseous water (-241.8 kJ/mole) plus Carbon graphitel( 0.0 kJ/mole) yields hydrogen gas (0.0kJ/mole) plus carbon dioxide gas(-393.5 kJ/mole) Calcium carbonate (marble chips) reacts with hydrochloric acid to produce carbon dioxide gas, water and calcium chloride....

  • CHM 1210 Final practice Name: Know electrolyte table, 5 solubility rules; 26 polyatomics (name/formula) Write 7...

    CHM 1210 Final practice Name: Know electrolyte table, 5 solubility rules; 26 polyatomics (name/formula) Write 7 naturally occurring diatomic molecules (name; formula, phase , charge) Write rite out strong acids and weak acids by name; formula, phase ,charge Write out the molecular, complete, and net-ionic equations for the following reactions The mixing of Cobalt(IlI) chloride and silver nitrate The mixing of acetic acid and sodium hydroxide The mixing of hydrochloric acid and cakcium hydroxide The mixing of barium chloride and...

  • all of our classes are online now and i have no idea HOW to do this....

    all of our classes are online now and i have no idea HOW to do this. please explain with steps if you can. thank you! Class Worksheet Chapter 98p16 (2) (Protected View) - Word out References Mailings Review View Help Tell me what you want to do Enable Editing the Internet can contain viruses. Unless you need to edit it's safer to stay in Protected View 2) How many moles of oxygen are required to burn 3.25 moles of butane...

  • A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a...

    A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a "1" if necessary. Identify the type of reaction in the right column. Balanced Equation Type of Reaction 1. H.As2O7 → _ As2O3 + _H20 2. _N2+_02—_N20 _NaI + _Br2 → _NaBr +_12 PbCrO4 +_HNO3 → __Pb(NO3)2 + __H2CrO4 . _C3H8 +_02 → __CO2 + __H20 TiCl4 + _ Mg → _ MgCl2 + ____Ti CuSO4 +_ KCN → ___Cu(CN)2 +_K2SO4 Ca(ClO3)2 → _ CaCl2...

  • POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got...

    POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got Mol-aria Why? Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction. This is called Stoichiometry- (stoi-key-ah-meh-tree) Another way of looking at it is using the mole ratio from the balanced equation and information about one compound in the reaction to determine information about another compound in the equation. A mole ratio...

  • PO9Recitation HW Complete the following questions in your lab notebook! Use the periodic table of the...

    PO9Recitation HW Complete the following questions in your lab notebook! Use the periodic table of the Denniston book for the molar mass calculations (at least 2 decimal places). Part 1. 1. What is the molar mass of Nicotin? (hint: determine the molecular formula first) 2. Based on what you learned in Ch3, what do you predict about nicotine and the solubility in water? 3. Calculate how many grams there are in 0.74 mol Ala(504) 4. The mass of 1.63 x102...

  • 19) How many of each type of atom are there in the formula Ca3(PO4)2? A) Ca...

    19) How many of each type of atom are there in the formula Ca3(PO4)2? A) Ca = 3, P = 1,0 = 4 B) Ca 3, P = 2, O = 4 C) Ca = 3, P = 2,0=8 D) Ca = 3, P = 1,0 = 8 E) none of the above le Ol be 20) What is the correct formula of a compound that has ten oxygen atoms and four phosphorus atoms? A) O10P4 B) 100P4 C) 4P010...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT