The Mole and Stoichiometry Unit Review

1) Calculate the mass of one mole of each of the following. This is known as the molecular mass or molecular weight.

a. Sodium?fJ/<~o\

b. Chlorine *0*0 j/^l

c. Water l*\^2 3/(Ml)

d. sulfur dioxide

e. (NH4)2S04 132.

f. Al(OH)3 ?S.OI /

2) Calculate the mass of

a. 1.50 moles of N2WC—l x £2*023/^1 ~ HZ.o

b. 2.50 moles of Mg3(P04)2

2 «5"O x f

c. 8.50 moles of AICI38 .So *+.0(* l-5s ^A.t - iis^a

d. 7.50 moles of sodium7-§"Oa 22.?? //2 5

3) Calculate the number of moles of

II2 x im, aa. 250.0 g of S02 3* ^ u-vdl3

( U* <3 ) (b. 250.0 g of 02 ~ 7'9\Z ^32-00%

(c. 250.0 g of Na l v-*. 6 * h-£7-^l3* ' 2-2 -9 f ^

lId. 250.0 g of (NH4)2Cr207 ZiTd 4> •3 * I* 0? um. a<25*2.(04

4) How many grams are in 3.2L of C02 at STP3'2L y _ 1__ x clH ’O I ^

3 <3I K'W

5) What is the volume of 1.3 x 10 29 molecules of H2 at STP

I -3 * Ir ga,* ll^rl

- X /£> * u^-02 R.

6) What is the volume of 2.459 moles of nitrogen gas at standard pressure and temperature?

l «*■*■ 0» ( ~ Jr&.OR U

7) How many moles of 02 are there in a 2.00 L container at STP?

[Z-.oVU X I (0 *4~

8) How many particles are there in a 3.57 Cplastic bag if it is filled with a gas at STP?

3.5-yi- x .i»«£2.4 *-

* &iQtZ. x (Q j.

| <^-or | -

/

9) What volume would butane [C4H10 (g)] occupy at STP if you have 2.222 grams of it?

2-2,2: I U^a I V = ^ 9 / Z_57>, I l (

10) Consider 9.00 moles of C6H14a. How many C6H14 molecules are present?

7.^3M J K S.6Z* v*3 lecvjzr

b. What percent mass of C atoms are present?IZ.QlofiJ

zoV„\11) Consider 150.0 g of C4H8O

• x <<50

a. How many moles of C4H8O are present?/I ~ ^ 0O IM-O

b. How many molecules are present?x 6sdZ £cO****-0 ^ / /

ia-'.cJ «<SC VI &£>l&C. ~ l.2*-Zx/0>

(

c. What is the % by weight of the element C?*4 x 1/o**(

12ja.(Calculate the concentration of each of the following solutions:

a. 2.35 moles of CaCl2 are dissolved in water to make a volume of 25 L.2 j '35' »•-*(, p.

2.S L-

12)

H - o .01f h

b. 790 ml of solutions that contains 1.35 moles of silver acetate.1. 3EW.0 1

1.7-1 M

c. 1.25L of solution that contains 13g Sodium Hydroxide.£> « 7<i? (

1-25'Lx . lr±L- =

0 tfaaia - 6.Z6n3

d. 8.57 g of lead (II) hydroxide are dissolved in water to make a volume of 550 ml.

0 'S&O Uk J**■<*!

ti I -Z2j-O'OSSM

You have 245 ml of a 4.52M silver nitrate solution. Describe how you would dilute down to a 1.00 M solution.

13)

^3L O . “/—Z*5L = Vz_

uJ a-f ec>1

- V*.I-I* L.14) You have 725.0 ml of a 0.998 M calcium chromate solution. Describe how you

would dilute this down to a 0.0500 M solution.IZ.7-#L- of,-. Ujd &X.6 7iroL 9\f

0.OGOOH.

vWtF L15) How do you make a 1M, 0.500L solution of HC1 from a 18M stock solution?

lid I A*} iVi * 1 /1*0,u

tv< -- <>;

<5?U16) The combustion of a sample of butane, C4H10 (lighter fluid), produced 2.46 grams

of water.AZZLC4H10+ (3 o2 £co2+ !<*h2o

What type of reaction is this and How much Butane was used in the reaction?Ocrv^K. b U$ ftu^a ,

vfa>H 3l **-<*( ) =- /.^a2.4^ I (/<5 -02- j

17) Calculate how many grams of iron can be made from 16.5 grams of Fe203 by the following equation. (What type of reaction is this) 3 « l <s> <*>\ j £>(

. <S>J Fe203

ir5 H2->ZFe+3H20+

US<\/ ^ -V /5-f.WpC * \ ~ H.iT 3

18) Nickel metal reacts with silver nitrate solution according to the following equation. <&<£<£

Z, AgN03 -A 2_Ag\ Ni I Ni(N03)2+ +a. If 15.32 grams of nickel reacts with a 32.55g of silver nitrate solution, what is the

limiter in the reaction?W

u,l

2_ U„( X

iMz5^6f^

Ay Ai#3(v-v.* I

2^ ^9isf.e?3Ay ^0^ \ \ U~e

l

15

L. t

b. How much of the excess material is left over?

Z.0.6 ?(tr.j?15.3Z* — 3J

- f. ?%>

19) When sulfur trioxide mixes with water it forms sulfuric acid&

1 H20 + 1 SO3 1 H2SO4

a. What type of reaction is this?£ y~n __________

b. If I start this reaction with 102 grams of sulfur trioxide and an excess of water, how many grams of sulfuric acid could I produce?

f *<*(\OL66-Of

c. If 98 grams of sulfuric acid is actually produced, what was my percent yield of

hydrogen?

79Kk toO/a|253