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The fluorocarbon, C2Cl3F3 has a normal boiling point of 47.6 oC. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g. oC and 0.67 J/g.oC, respectively. The heat of vaporization of the compound, ΔHvap, is 27.49 kJ/mol. Calculate the enthalpy change (in kj) for converting 50.0 g of this compound from the liquid at 5.0 oC to the gas at 80.0 oC (Mw.of C2Cl3F3 = 187.37 g/mol)

Calculate the ph 0.025 of HNO3 solution

circle and label the functional group of aspirin that causes it to irritate the stomach

Which of the following is base?

1.  

2.  

3.  

4.  

5.  

6. All of these

7. None of these

The heat of fusion of water is 6.01 k J / m o l . The heat capacity of liquid water is 75.3 J / m o l ⋅ K . How much k J of heat is required for the conversion of 50.0 g of ice at 0.00 ∘ C to liquid water at 22.0 ∘ C

You have a set of solutions of , and .
To each of these solutions, you add of . Given that , , and , what would you expect to happen (use the idea)?

Ammonia gas enter the reactor of a nitric acid plant with more dry air than is required for a complete conversion of the ammonia into nitric oxide and water vapour. If the gases enter the reactor at , if conversion is complete, if no side reaction occur and if the product stream leaves at , determine the heat loss from the reactor.

 A rigid plastic container holds 35.0g of ethylene gas (C2H4) at a pressure of 793 torr. What is the pressure if 5.0g of ethylene is removed at constant temperature?

After the completion of a gas forming reaction, the column of water remaining in the collection flask was measured to me high, the vapor pressure of water is at , and the atmospheric pressure that day was measured as , what is the partial pressure of the gas produced by the reaction .

Nitric acid neutralizes potassium hydroxide. To determine the heat of reaction, a student placed of in a coffee cup calorimeter, noted that the temperature was , and added of , also at . The mixture was stirred quickly with a thermometer, and its temperature rose to .

A titration of of was done with . For the diprotic acid , . Calculate the pH after of have been added.

A.  

B.  

C.  

D.  

E.  

A volume of of is added to of weak acid . What is the pH of the resulting buffer? 

The equilibrium constant for the chemical equation is at . Calculate the value of for the reaction at .

The combustion of of glucose, , in a bomb calorimeter with a heat capacity of results in an increase in the temperature of the calorimeter and its contents from to . What is the internal energy change, , for the combustion of of glucose?

When of a stock solution containing is diluted to , how many moles of are in the new solution?

The solubility of in water is per at and per at . Write the equation for the solubility equilibrium, including heat as a reactant or product. What is the sign of ?

• You are to read through Scenarios A and B.  Figure out which one that the researcher did incorrectly.  After choosing that one, you are to write out what they did incorrectly and why. 
• Then, explain what the scientist should do to make the experiment correct.

Your answer must be in complete sentences and use proper sentence structure.  Use proper grammar and spelling in your responses.  You must include the correct balanced equation for both scenarios and any calculations for determining your answer. Write as much as you can showing all balancing equations and calculations and be accurate on the topic since this is worth 9 points.  

• Scenario A
  • Wilma was given the task to produce of aluminum oxide, .  She had one tank of oxygen gas, and of solid aluminum, .  She knew that if she heated the aluminum in the presence of the oxygen gas, she could produce the aluminum oxide. Since she had such little amount of aluminum, she decided to use as little of aluminum as she could to produce the of aluminum oxide.  She measured out of aluminum and heated it with excess oxygen.  Assume Wilma’s reaction went .  Wilma was very happy that her reaction produced the .
• Scenario B
  • Fred was given the task to produce of aluminum bromide, . He had a tank of bromine gas, , and of solid aluminum, . He knew that if he heated the aluminum in the presence of excess bromine gas, he could produce the aluminum bromide.  Since he had such little amount of aluminum, he decided to use as little of aluminum as he could to produce the 63 grams of aluminum bromide.  He measured out of aluminum and heated it with excess bromine gas.  Assume Fred’s reaction went .  Fred was very happy his reaction produced the .

A quantity of of is mixed with of in a constant-pressure calorimeter that has a heat capacity of . If the initial temperatures of both solutions are the same at , what is the final temperature of the mixed solution? The heat of neutralization is . Assume the density and specific heat of the solutions are the same as those for water.

Is it true that is an equilibrium constant that can be used to express quantitatively the extent to which a compound dissolves?

The heat from an acetylene torch is produced by burning acetylene in oxygen.

How many grams of water can be produced by the reaction of with ?

A piece of metal A and a piece of Metal B are placed on identical hot plates at identical settings. Metal B gets hot to the touch faster than metal A. What must be true?

A. Metal A has higher specific heat than Metal B

B. Metal B has higher specific heat than metal A

C. The metals both have low specific heats

D. Metal A has a lower specific heat than Metal B

E. The metals both have high specific heats

What happens to the solubility of a gas when the pressure above a liquid increases?

A. The solubility decreases
B. It depends on the numerical value of the pressure
C. It depends on the chemical nature of the gas
D. The solubility increases
E. The solubility remains the same

The concentrations of and in a sample of river water are and , respectively. Express the concentration in molality?

A sample of aniline was combusted in a bomb calorimeter. If the temperature rose by , use the information below to determine the heat capacity of the calorimeter.

Given the following information:
 

and , , ,

What is at ?

Consider the reaction below:

At STP, what volume oxygen  is consumed in producing  energy?

1. ___________ is the energy used to move an object against a force.

a) kinetic energy

b) potential energy

c) heat

d) work

e) Galen-Marek

2. All of the ____________ have a valence shell electron configuration of ns2.

a) noble gases

b) halogens

c) chalcogens

d) alkali metals

e) alkaline earth metals

Calculate the heat required to melt of ice.

You need to make of ammonium chloride solution. How many grams of ammonium chloride do you use? What volume of water will be used? (hint: recall the density of water).

What is electronic theory of valency?

Iron is biologically important in the transport of oxygen by red blood cells from the lungs to the various organs of the body. In the blood of an adult human, there are approximately red blood cells with a total of of iron. On average, how many iron atoms are present in each red blood cell?  

A)  

B)  

C)  

D)  

E)

A sample of iron was dissolved in hydrochloric acid. The liberated hydrogen was collected by displacement of water. The hydrogen occupied 262 mL at 26°C. The barometric pressure was 748 torr. What mass of iron was dissolved? The vapor pressure of water is 25 torr at 26°C. Fe(s) + 2HCl(aq) ® FeCl 2 (aq) + H 2 (g)

 Write the reaction when solid magnesium acetate is put into water

(a) Analysis of a certain compound showed that of it contained of hydrogen, of carbon, and of oxygen. Calculate the empirical formula of the compound. If the vapor density of the above molecule is 45, determine its molecular formula.

(b) Calculate the pH of a solution of (strong acid).

The solubility of sodium chloride in water is at . What is the maximum amount of sodium chloride that will dissolve in of water at ?

Which has the higher boiling point and why? or ? or ?

A. Is oxygen gas an element, a compound, or a mixture?

B. Which of the following is a polysaccharide?

a. sucrose

b. hexose

c. glucose

d. cellulose

e. two of the above

What is the van't Hoff factor for ?