assuming this is a quanatiative reaction

the reaction is:

   NaSO_4(aq) + CaCl_2(aq) --> CaSO_4(s) + NaCl_(aq)

0.50mol/L of sodium sulfate solution is meaured and put into 4 150ml beakers and 4 different volumes of 0.50mol/L of calcium chloride solution are prepared in a graduated cylinder. the caclium chloride will be added to the sodium solfate solution which is in the beaker and stirred. 

find the limiting and excess reagents for each trial

trial  | volume  of 0.50mol/L of Na₂SO₄(aq) (mL)  |   Volume of 0.50mol/L CaCl_2(aq) (mL) | 

1)     |  50                                                         |   25

2)     |  50                                                         |   50

3)     |  50                                                         |   75

4)     |  50                                                         |   100

A TECHNICION PLAES 0.50 MOL OF NITROGEN MONOXIDE GAS AND 0.20 MOL IF CHLORINE GAS IN A 1.00L SEALED CONTAINER AT 100 DEGREES CELSUIS. THE FOLLOWING EQUALIBRIUM IS ESTABLISHED AT 4.5 MIN. 

2NO(g) + Cl₂(g) --->2NOCK(g)

the arrow is supposed to be meant as forward and reverse 

THE TECHNICION DETERMIBES THAT AT EQUALIBRIUM THERE ARE 0.30 MOL OF NOCL, 0.20 mol of nitrogen monoxide and 0.050 mol of chlorine gas. 

question 1 

calculate the percent yeild 

question 2 

calculate the equalibrium constant 

a technicion placed 4.0 mol of PO₂Br(g) in a 2.0L sealed container. the following equalibirum established

2PO₂Br(g)<---> 2PO₂(g) + Br₂(g) 

at equalibrium it was determined that the sealed reaction vessel contained 1.8 mol of Br₂(g) 

calculate kc for this equalibirum 

CO_(g) + H₂O_(g) <--->CO_2((g) + H_2(g) 

kc= 7.3

delta H= -41.2KJ

if the temperature of the system at equilibrium is increased, then the concentration of the H2(g₎ will _______ and the value of kc will_____

for the blanks choose one from the following 

- increase

-decrease

-stay the same 

question 2 

Solid copper(II) sulfate was added to a flask containing water and then stoppered. the following solubility equilibrium was established . 

CuSO_4(s) <---> Cu²⁺_(aq)+ SO₄^2-_(aq)

which of the following observations would indicate that equilibrium has been established?

1. the forward and the reverse reaction have stopped

2. the mass of the solid copper(II) sulfate is completely dissovled

3. the pressure of the system is constant

4. the mass of solid copper(II) sulfate remaining in the flask is constant

a technicion placed 2.5mol of NO(g) in an  empty 2.0L flask and allowed the contents to establish the following equilibrium. 

4NO(g)<---> 2N₂O(g) + O₂(g) + 197KJ

AT EQUILIBIRUM IT WAS DETERMINED THAT THERE WAS 0.58 MOL OF N₂O(g) present. 

what is the percent yield? 

part b. 

what is the equilibrium concentration of NO(g)?

part c. 

the equilibrium constant for this equilibrium is? 

the constant should be expressed in scientific notation is a.b $\times$× 10^-c

question 2. 

solid copper(II) sulfate is added to a flask containing water and then stoppered. the following equilibrium was established. 

CuSO4(s)<---> Cu²⁺(aq) + SO4^2-(aq)

when a small amount of a saturated solution of barium nitrate is added to the equilibrium system, the amount of solid copper(II) sulfate would ________(increase or decrease) as the system shifts to the _________ (left or right)

only choose one of the opitions to fill the blanks!

assgin the oxidation numbers for each 

make sure to put the -/+ 

oxidation number       entity 

                                 I in I₂(s)

                                 S in HS^-(aq)

                                  Xe in XeF6(s)

determine whether each of the following equations is a redox reaction or not

C6H12O6(s)→CO2(g)+C2H5OH(l)

NaOH(aq)+Al(s)+H2O(l)→H2(g)+NaAlO2(s)

SO2(g)+H2O(l)→H2SO3(aq)

2NaOH(aq)+Cl2(g)→NaCl(aq)+H2O(l)+NaClO(aq)

Na2CO3(aq)+2HCl(aq)→2NaCl(aq)+H2O(l)+CO2(g)

C6H12O6(s)+6O2(g)→6CO2(g)+6H2O(l)

Fe3O4(s)+CO(g)→3FeO(s)+CO2(g)

2Fe(OH)3(s)→Fe2O3(s)+3H2O(l)

  C 

STRONG OXIDIZING AGENTS WILL HAVE STRONG AFFINITY FOR ELECTRONS AND TEND TO GAIN ELECTRONS 

IS THIS TRUE OR FALSE?

STRONG REDUCING AGENTS WILL HAVE STRONG AFFINITY FOR ELECTRONS AND TEND TO GAIN ELECTRONS 

IS THIS TRUE OR FALSE?

WEAK REDUCING AGENTS WILL HAVE A WEAK AFFINITY FOR ELECTRONS AND TEND TO LOSE ELECTRONS 

IS THIS TRUE OR FALSE?

IN AN EXPERIMENT TO STUDY THE SPONTANEITY OF REDOX REACTIONS, A STUDENT PLACED DIFFERENT METALS INTO FIVE SEPERATE TEST TUBES, EACH CONTAINING A DIFFERENT 1.0MOL/L SOLUTION, AS SHOWN BELOW. 

TEST TUBE 1- THE METAL IS Zn(s) in a solution of Fe(NO3)2(aq)

Test tube 2- the metal is Co(s) in a solution of Sn(NO3)2(aq)

test tube 3- the metal is Cu(s) in a solution of Cu(NO3)2(aq) 

tets tube 4- the metal is Au(s) in a solution of Cu(NO3)2(aq) 

test tube 5- the metal is Ag(s) in a solution of HNO3(aq) 

test tube 6- the metal is Ni(s) in a solution of AgNO3(aq)

for each test tube, determine which one is a spontaneous reaction and which one is not a spontaneous reaction. 

2. which of the entities will react spontaneously with Zn(s) but not with Cd(s) 

- Sn²⁺_(aq)

_- Mg²⁺_(aq)

- H2O(l)

- Cr³⁺_(aq)

 3. find the strongest SOA AND SRA

a solution of iron(II) chloride is mixed with an acidifed sodium nitrate 

b. solution of sodium hydroxide, potassium sulfite and chromium(II) nitrate are mixed. 

4. which of the following is an entity that will copper(II) ions and also oxidize metallic nickel

this is a titration question 

answer the following questions using the information provided below 

1. The moles of Cr₂O₇^2-(aq) that reacted, expressed in scientific notation, is a.bc x 10^-dmol. The values of a, b, c and d are 

2. The concentration of Sn²⁺(aq), expressed in scientific notation, is a.bc x 10^-d mol/L. The values of a, b, c and d are 

It has been determined that fluoride can prevent the decay of tooth enamel. Historically, tin(II) fluoride was added to toothpaste to help combat tooth decay. Titration analysis was used to determine the concentration of tin(II) fluoride in a NMmple of toothpaste. A 10.0 mL sample of tin(II) fluoride solution was acidified and titrated with 0.0100 mol/L potassium dichromate solution as represented by the following equation.

3Sn2+(aq)+Cr2O2−7(aq)+14H+(aq)→3Sn4+(aq)+2Cr3+(aq)+7H2O(l)

The following data was collected during the four trials.