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Name ……………………………………………. Team ……………………….

Title: moles Date ………………………

1. What is the gram formula mass of sodium sulfate?

1) 119 g/mol (3)55 g/mol

2) 142 g/mol (4) 78 g/mol

2. What is the gram formula mass of elemental oxygen?

1) 8 g/mole (3) 32 g/mole

2) 16 g/mole (4) 64 g/mole

3. How many atoms are in 4.0 g of helium?

(1)6.02x 1023

(2) 3.01 x 1023

(3) 12.04 x 10 23

(4)4.0x 1023

4a. A balloon is filled with 32 g of elemental oxygen. How many diatomic molecules would be in to balloon?

1)6.02x 1023

(2) 3.01 x 1023

(3) 12.04 x 10 23

(4)4.0x 1023

4b. A balloon is filled with 32 g of elemental oxygen. How many atoms of oxygen would be in to balloon?

(1) 6.02x 1023

(2) 3.01 x 1023

(3) 12.04 x 10 23

(4) 4.0x 1023

Name ……………………………………… Team ……………………….

Title: Particles Date ………………………

How many particles make up one mole?

Whose number is this?

How many moles are in 48.6 grams of magnesium?

How many grams are in 2.5 moles of diatomic oxygen?

How many moles are in 22 grams of diatomic hydrogen?

How many particles in 2 moles of Li

Apply the dimensional analysis set up to solve each of the following

2 NaOH + H2SO4(2 H2O + Na2SO4

How many grams of sodium sulfate will be formed if you start with 2.007 x1023 particles of sodium hydroxide and you have an excess of sulfuric acid?

Complete the bottom row of the dimensional analysis grid

How many moles are in 27 g of water?

(1) 18 moles (3) 1.5 moles

(2) 2.0 moles (4) 1.0 moles

What do we start with?

Have do we convert this to moles of H2O?

What is the molar mass of water?

For the following balanced reaction

2 H2 (g) + O2 (g) 2 H2O(g)

What mass of water can be produced from 4.0 g of elemental hydrogen and excess oxygen?

(1)4.0g (3)36g

(2)18g (4)32g

. Given the balanced equation:

2 C4H10 (g) + 13 O2 (g) 8 CO (g) + 10 H2O (g)

What is the total number of moles of O2(g) that must be available to react completely with 5.00 moles of C4H10?

1) 10.0 moles (3) 26.5 moles

2) 20.0 moles (4) 32.5 moles

2. Balance the following equation using the smallest whole-number coefficients.

___ CH3OH (g) + ___ O2 (g) ___ CO2 (g) + ___ H2O(g)

Using your balanced equation, show a correct numerical setup for calculating the total number of grams of H2O (g) produced when 5.0 moles of O2(g) are completely consumed.

3. Given the unbalanced equation:

____ C6H12O6 (s) - ____ C2H5OH (l) + ____ CO2 (g)

a. Balance the equation provided using the lowest whole-number coefficient.

b. How many grams of carbon dioxide gas can be produced from 90 g of C6H12O6

4. How many grams of aluminum are required to react with of 160 g iron (III) oxide in order to produce iron metal and aluminum oxide according to the following reaction? To receive complete credit you must show your work in the form of dimensional analysis.

2 Al (s) + Fe2O3 (s) Al2O3 (s) + 2 Fe (l)

5. If 20.0 grams of zinc react with excess hydrochloric acid, how many grams of zinc chloride are produced?

Zn (s) + HCl (aq) ZnCl2 (aq) + H2 (g)

6. How many grams of chlorine gas must be reacted with excess sodium iodide if 10.0 grams of sodium chloride are needed?

___NaI (aq) + ___Cl2 (g) _______ NaCl (aq) + ____ I2 (g)

7. How many grams of oxygen are produced in the decomposition of 5.00 grams of potassium chlorate?

_______KClO3 (s) ________KCl (s) + ______O2 (g)

8. How many grams of copper are required to replace 4.00 grams of silver nitrate which are dissolved in water?

______Cu (s) + _____AgNO3 (aq) _________Cu(NO3)2 (aq) + _____Ag (s)

9. If excess ammonium sulfate reacts with 20.0 grams of calcium hydroxide, how many grams of ammonia are produced?

___(NH4)2SO4 (aq) + ___Ca(OH)2 (s) ___ CaSO4(s) + ___NH3 (g) + ___H2O (l)

10. a) How may moles and how many grams of magnesium phosphate are produced by starting with 100.0 grams of phosphoric acid and an excess of magnesium carbonate?

___MgCO3 (s) + ___H2PO4 (aq) _____Mg3(PO4)2 (aq) + ___H2O (l) + ___CO 2(g)

___MgCO3 (s) + ___H2PO4 (aq) _____Mg3(PO4)2 (aq) + ___H2O (l) + ___CO 2(g)

10. b) If 20.0 grams of carbon dioxide are produced, how many moles of magnesium carbonate were used initially?

10.c Starting with 50.0 grams of magnesium carbonate and excess phosphoric acid, calculate the number of grams of each product produced.

Name …………………………………………… Team ……………………….

Title: DA mass moles calcs Date ………………………..

1a) How may moles and how many grams of magnesium phosphate are produced by starting with 100.0 grams of phosphoric acid and an excess of magnesium carbonate?

____MgCO3 (s) + ____H2PO4 (aq) ______Mg3(PO4)2 (aq) + ___H2O (l) + ___CO 2(g)

b) If 20.0 grams of carbon dioxide are produced, how many moles of magnesium carbonate were used initially?

c) Starting with 50.0 grams of magnesium carbonate and excess phosphoric acid, calculate the number of grams of each product produced.

Name ………………………………………… Team ……………………….

Title: DA Mass mole calcs Date ………………………

1. Phosphorous will burn in oxygen to give two different compounds: Diphosphorus trioxide and diphosphorus pentaoxide.

a) How many grams of oxygen are required to produce the trioxide if 15.0 grams of phosphorus are used?

P + O2 P2O3

b) How many grams of oxygen are required to produce the pent oxide if 15.0 grams of phosphorus are used?

P + O2 P2O5

2. If a plant needed to make 30.0 grams of glucose, C6H12O6, through the process of photosynthesis from CO2 and H2O, how many grams of water are required? Photosynthesis is a complex process composed of many steps. The initial reactants are carbon dioxide and water and the final products are glucose and oxygen gas.

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2.007 x1023 particles NaOH

g Na2SO4

1 mole NaOH

1 mole Na2SO4

6.022 x1023 particles of NaOH

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