how all work on a separate sheet and attach. Use atomic weights rounded to 2 decimal places. 1. For the following reaction, AgNO 3 + BaCl 2  AgCl + Ba(NO 3 ) 2 : a. Balanced equation including states ___________________________________________ b. If you have 2.50 moles of AgNO 3 , how many moles of Ba(NO 3 ) 2 can be formed? ____________ 2. For the reaction N 2 + 3H 2  2NH 3 , if you have 2.00 moles of N 2 and 4.00 moles of H 2 : a. Identify the limiting reactant. ____________ b. How many moles of NH 3 can be formed? ____________ c. How many moles of the excess reactant will remain? _________ 3. If for the equation in (2) above, you have 1000. g of N 2 and 150.0 g of H 2 : a. Identify the limiting reactant. _____________ b. Calculate the theoretical yield in grams of NH 3 . __________ c. Calculate the grams of excess reactant. ____________ 4. Consider the reaction: P 4 + 6Cl 2  4PCl 3. a. How many grams of Cl 2 are needed to react with 20.00 g of P 4 ? ______________ b. You have 15.00 g. of P 4 and 22.00 g. of Cl 2 , identify the limiting reactant and calculate the grams of PCl 3 that can be produced as well as the grams of excess reactant remaining. LR____________ grams PCl 3 _________ grams excess reactant _________ __ c. If the actual amount of PCl 3 recovered is 16.25 g., what is the percent yield? ______________ d. Given 28.00 g. of P 4 and 106.30 g. of Cl 2 , identify the limiting reactant and calculate how many grams of the excess reactant will remain after the reaction. LR ______________ grams excess reactant _____________ 5. Consider the reaction: CH 4 + 2O 2  CO 2 + 2H 2 O a. Calculate the grams of O 2 needed to react with 20.00 grams of CH 4 . _____________ b. Given 15.00 g. of CH 4 and 22.00 g. of O 2 , identify the limiting reactant and calculate the grams of CO 2 that can be produced. LR _________ grams CO 2 _________ 30 c. For the reaction CH 4 + 2O 2  CO 2 + 2H 2 O, if you have 10.31 g. of CH 4 and an unknown amount of oxygen, and form 20.00 g. of CO 2 , i. Identify if there is a limiting reactant ______________ ii. Calculate the number of grams of the limiting reactant present if there is one. ______________ 6. What mass percent solution will result from dissolving 0.126 moles of AgNO 3 in 475 g. of water? ________________ 7. If you take 225 g. of 2.50 mass % solution, how many grams of solute do you have? ____________ 8. How many grams of BaCl 2 are needed to prepare 550 ml of 0.60M solution? _____________ 9. How many moles of solute are present in 322 ml of 0.25 0 M solution? _________ 10. If a 1.20M solution is used to prepare 275 ml of 0.52M solution, what volume of 1.20M solution is needed? __________ 11. If 52.00 ml of 0.50 0 M CaBr 2 solution is added to 128 ml of 0.32 0 M solution of KCl solution, what will the molarity of CaBr 2 and the molarity of KCl in the final solution? (assume volumes are additive) CaBr 2 _____________ KCl _________ 12. What will be the molarity of a 236 ml solution if it has been prepared from 75 .0 ml of 3.00 M solution of NH 4 NO 3 ? _________________ 13. What volume of a 1.63 mass % solution of Mg(NO 3 ) 2 is needed to contain 0.316 grams of Mg(NO 3 ) 2 ? The solution has a density of 1.016 g/ml. ________________ 14. If you have 48.00 g. of K 2 CrO 4 , what volume of 0.1500 M BaCl 2 solution is needed to completely react with all the K 2 CrO 4 ? ____________ BaCl 2 + K 2 CrO 4  BaCrO 4 + 2KCl 15. If 1 00.0 ml of 0.10 0 M Cu( NO 3 ) 2 is reacted with 50.0ml of 0.20 M NaOH, according to the following reaction, how many moles of Cu(OH) 2 will be formed? ___________ Cu(NO 3 ) 2 + 2Na OH  Cu(OH) 2 + 2 NaNO 3 16. From the titrations below, calculate the molarity of the NaOH solution in each of the following? Make sure you balance the equations. a) NaOH + HCl  NaCl + H 2 O 32.00 ml of NaOH is required to completely react with 25.00 ml of 0.15 0 M HCl. ___________ b) NaOH + H 2 SO 4  Na 2 SO 4 + H 2 O 42.00 ml of NaOH is required to completely react with 18.00 ml of 0.10M H 2 SO 4 . __________ 17. How many moles of CoCl 3 are in 172.6 ml of a 19.6 mass % solution of CoCl 3 which has a density of 1.206 g/mL ? __________

how all work on a separate sheet and attach. Use atomic weights rounded to 2 decimal places. 1. For the following reaction, AgNO 3 + BaCl 2  AgCl + Ba(NO 3 ) 2 : a. Balanced equation including states ___________________________________ b. If you have 2.50 moles of AgNO 3 , how many moles of Ba(NO 3 ) 2 can be formed? 2. For the reaction N 2 + 3H 2  2NH 3 , if you have 2.00 moles of N 2 and 4.00 moles of H 2 : a. Identify the limiting reactant. b. How many moles of NH 3 can be formed? c. How many moles of the excess reactant will remain? _ 3. If for the equation in (2) above, you have 1000. g of N 2 and 150.0 g of H 2 : a. Identify the limiting reactant. _ b. Calculate the theoretical yield in grams of NH 3 . c. Calculate the grams of excess reactant. 4. Consider the reaction: P 4 + 6Cl 2  4PCl 3. a. How many grams of Cl 2 are needed to react with 20.00 g of P 4 ? b. You have 15.00 g. of P 4 and 22.00 g. of Cl 2 , identify the limiting reactant and calculate the grams of PCl 3 that can be produced as well as the grams of excess reactant remaining. LR grams PCl 3 _ grams excess reactant _ c. If the actual amount of PCl 3 recovered is 16.25 g., what is the percent yield? ____ d. Given 28.00 g. of P 4 and 106.30 g. of Cl 2 , identify the limiting reactant and calculate how many grams of the excess reactant will remain after the reaction. LR grams excess reactant _ 5. Consider the reaction: CH 4 + 2O 2  CO 2 + 2H 2 O a. Calculate the grams of O 2 needed to react with 20.00 grams of CH 4 . ___ b. Given 15.00 g. of CH 4 and 22.00 g. of O 2 , identify the limiting reactant and calculate the grams of CO 2 that can be produced. LR _ grams CO 2 _ 30 c. For the reaction CH 4 + 2O 2  CO 2 + 2H 2 O, if you have 10.31 g. of CH 4 and an unknown amount of oxygen, and form 20.00 g. of CO 2 , i. Identify if there is a limiting reactant ii. Calculate the number of grams of the limiting reactant present if there is one. 6. What mass percent solution will result from dissolving 0.126 moles of AgNO 3 in 475 g. of water? 7. If you take 225 g. of 2.50 mass % solution, how many grams of solute do you have? 8. How many grams of BaCl 2 are needed to prepare 550 ml of 0.60M solution? _ 9. How many moles of solute are present in 322 ml of 0.25 0 M solution? _ 10. If a 1.20M solution is used to prepare 275 ml of 0.52M solution, what volume of 1.20M solution is needed? 11. If 52.00 ml of 0.50 0 M CaBr 2 solution is added to 128 ml of 0.32 0 M solution of KCl solution, what will the molarity of CaBr 2 and the molarity of KCl in the final solution? (assume volumes are additive) CaBr 2 ___ KCl _ 12. What will be the molarity of a 236 ml solution if it has been prepared from 75 .0 ml of 3.00 M solution of NH 4 NO 3 ? ___ 13. What volume of a 1.63 mass % solution of Mg(NO 3 ) 2 is needed to contain 0.316 grams of Mg(NO 3 ) 2 ? The solution has a density of 1.016 g/ml. 14. If you have 48.00 g. of K 2 CrO 4 , what volume of 0.1500 M BaCl 2 solution is needed to completely react with all the K 2 CrO 4 ? BaCl 2 + K 2 CrO 4  BaCrO 4 + 2KCl 15. If 1 00.0 ml of 0.10 0 M Cu( NO 3 ) 2 is reacted with 50.0ml of 0.20 M NaOH, according to the following reaction, how many moles of Cu(OH) 2 will be formed? _ Cu(NO 3 ) 2 + 2Na OH  Cu(OH) 2 + 2 NaNO 3 16. From the titrations below, calculate the molarity of the NaOH solution in each of the following? Make sure you balance the equations. a) NaOH + HCl  NaCl + H 2 O 32.00 ml of NaOH is required to completely react with 25.00 ml of 0.15 0 M HCl. _ b) NaOH + H 2 SO 4  Na 2 SO 4 + H 2 O 42.00 ml of NaOH is required to completely react with 18.00 ml of 0.10M H 2 SO 4 . 17. How many moles of CoCl 3 are in 172.6 ml of a 19.6 mass % solution of CoCl 3 which has a density of 1.206 g/mL ? ______

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

how all work on a separate sheet and attach. Use atomic weights rounded to 2 decimal places.

For the following reaction, AgNO

+ BaCl



AgCl + Ba(NO

)

Balanced equation including states ___________________________________________

If you have 2.50 moles of AgNO

, how many moles of Ba(NO

)

can be formed? ____________

For the reaction N

+ 3H



2NH

, if you have 2.00 moles of N

and 4.00 moles of H

Identify the limiting reactant. ____________

How many moles of NH

can be formed? ____________

How many moles of the excess reactant will remain? _________

If for the equation in (2) above, you have 1000. g of N

and 150.0

g of H

Identify the limiting reactant. _____________

Calculate the theoretical yield in grams of NH

. __________

Calculate the grams of excess reactant. ____________

Consider the reaction: P

+ 6Cl



4PCl

How many grams of Cl

are needed to react with 20.00 g of P

? ______________

You have 15.00 g. of P

and 22.00 g. of

, identify the limiting reactant and calculate the grams of PCl

that can be

produced as well as the grams of excess reactant remaining.

LR____________

grams PCl

_________

grams excess reactant _________

If the actual amount of PCl

recovered is 16.25 g., what is the percent yield? ______________

Given 28.00 g. of P

and 106.30 g. of Cl

, identify the limiting reactant and calculate how many grams of the excess

reactant will remain after the reaction.

______________

grams excess reactant

_____________

Consider the reaction:

+ 2O



+ 2H

Calculate the grams of O

needed to react with 20.00 grams of CH

. _____________

Given 15.00 g. of CH

and 22.00 g. of O

, identify the limiting reactant

and

calculate the grams of

that can be

produced.

LR _________ grams

_________

For the reaction

+ 2O



+ 2H

O, if you have 10.31 g. of CH

and an unknown amount of oxygen, and

form 20.00 g. of

Identify if there is a limiting reactant ______________

ii.

Calculate the number of grams of the limiting reactant present if there is one. ______________

What mass percent solution will result from dissolving 0.126 moles of AgNO

in 475 g. of water? ________________

If you take 225 g. of 2.50 mass % solution, how many grams of solute do you have? ____________

How many grams of BaCl

are needed to prepare 550 ml of 0.60M solution? _____________

How many moles of solute are present in 322 ml of 0.25

0 M solution?

_________

10.

If a 1.20M solution is used to prepare 275 ml of 0.52M solution, what volume of 1.20M solution is needed? __________

11.

If 52.00 ml of 0.50

0 M

CaBr

solution is added to 128 ml of 0.32

0 M solution of KCl solution, what will the molarity of CaBr

and

the molarity of KCl in the final solution? (assume volumes are additive)

CaBr

_____________

KCl _________

12.

What will be the molarity of a 236 ml solution if it has been prepared from 75

.0 ml of 3.00 M solution of

_________________

13.

What volume of a 1.63 mass % solution of Mg(NO

)

is needed to contain 0.316 grams of Mg(NO

)

? The solution has a density

of 1.016 g/ml. ________________

14.

If you have 48.00 g. of K

CrO

, what volume of 0.1500 M BaCl

solution is needed to completely react with all the K

CrO

____________

BaCl

+ K

CrO



BaCrO

+ 2KCl

15.

If 1

00.0 ml of 0.10

0 M

Cu(

)

is reacted with 50.0ml of 0.20 M NaOH, according to the following reaction, how many moles of

Cu(OH)

will be formed?

___________

Cu(NO

)

+ 2Na



Cu(OH)

+ 2 NaNO

16.

From the titrations below, calculate the molarity of the NaOH solution in each of the following? Make sure you balance the

equations.

NaOH + HCl



NaCl + H

32.00 ml of NaOH is required to completely react with 25.00 ml of 0.15

0 M HCl. ___________

b) NaOH + H



+ H

42.00 ml of NaOH is required to completely react with 18.00 ml of 0.10M H

. __________

17.

How many moles of CoCl

are in 172.6 ml of a 19.6 mass % solution of CoCl

which has a density of 1.206 g/mL ? __________

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