Calculate the concentration (in mol/L) of the products of the following equilibrium when the equilibrium constant is 19.0 and the equilibrium concentration of NOBr2(g) is 2.69 mol/L.

NOBr2(g) → NO(g) + Br2(g)

Draw a condensed structural diagram of 1,3-diethylbenzene. ( note can use a line diagram to represent benzene)

In an experiment, a student heated 550 g of water from 25oC to 91oC using 0.13 g of glycerol monostearate, an emulsifying agent used in the production of margarine.  If it is assumed that all the heat energy was absorbed by the calorimeter water, calculate the experimental enthalpy of combustion for glycerol monostearate in kJ/g.   

Top fuel dragsters (sometimes called funny cars) burn nitromethane.  This combustion is represented by the equation below.  

4 CH3NO2(l) + 3 O2(g)→ 4 CO2(g) + 6H2O(g) + 2N2(g)   

?cH = -1418.4 kJ    

16. Calculate the molar enthalpy of combustion for nitromethane.   

17.   A  5.00 g sample of nitromethane was burned in a calorimeter that  contained 250 g of water at 20.5 degrees celcius.  Calculate the final temperature of the water if all 5.00 g of nitromethane is combusted.

Hint – you will need to use the molar enthalpy of combustion that you calculated in Question 16. 

 question  1. 

Calculate the enthalpy of reaction for the reaction of nitrogen dioxide with water represented by the following equation:  

3 NO2(g) + H2O(l) →2 HNO3(aq) + NO(g)                  ?rH=?

questiion  2 

Nitrogen monoxide gas, which is used to treat some pulmonary diseases, is transported in pressurized gas cylinders.  Nitrogen monoxide gas is produced by reacting ammonia gas and oxygen gas, as represented by the following equation. 4 NH3(g) + 5 O2 (g)→ 4 NO(g) + 6 H2O(g)     

 Calculate the standard enthalpy of reaction for the above equation.    

 Write a balanced equation for the formation of copper(II) oxide at standard state.  Include the enthalpy change as an energy term in the balanced equation.   

Write a balanced equation for the simple decomposition of iron(II) oxide at standard state.  Include the enthalpy change as an energy term in the balanced equation.   

A TECHNICIAN PLACES  3.0 mol OF SULFUR TRIOXIDE IN A GAS SEALED  500 mL CONTAINER AND ALLOWED THE REACTION TO ESTABLISH THE FOLLOWING EQUALIBRIUM

2SO_3(g) ---> 2SO_2(g)  + O_2(g)

_{P.S THE ARROW IS SUPPOSED TO BE A REVERSE AND FORWARD REACTION SYMBOL.}

_{AT EQUALIBRIUM THE SYSTEM WAS DETERMINED TO CONTAIN 0.95 MOL OF OXYGEN GAS.}

_{WHAT IS THE PERCENT YIELD?} 

consider the following 

CO(g) + H2O(g)---> CO2(g) + H2(g) kc= 5.0

at equalibrium a 2.0 L container was found to contain 0.20 mol of CO2(g) , 0.30 mol of H2O(g) and 0.90 mol of H2(g).

The equalibirum amount of carbon dioxide is

question 2 

4HCl(g) + O2(g) ---> 2H2O(g) + 2Cl₂(g) kc= 357

An equalibirum mixture of the above system was found to contain the following concentratins: HCl(g)= 0.35mol/L, O2(g)= 0.078 mol/L and H2O(g)= 1.2mol/L. the equalibirum concentration of Cl₂(g) is? 

THE FOLLOWING SYSTEM WAS HEATED 

H2(g) + I2(g) + 53kJ ---> 2HI(g) 

identify the effect of the temperature increase on the concentation of HI and on Kc of this system. 

choose either it decreases or increases for both 

Concentation of HI= 

Kc= 

question 2 

consider the following equalibrium 

BaS(s)--> Ba²⁺(aq) + S^2-(aq)

when Ba(NO₃)₂(aq) is added to this solution the equalibirum shifts to the ________ and the concentration of the sulfide ions___________ 

choose either right or left for the shift 

and choose decrease or increase for the concentration of ions

P.S THE ARROWS ARE SUPPOSED TO BE MEANT AS REVERSE AND FORWARD 

sour gas H₂S(g) can establish the following equalibrium system under certain conditions. 

note that S₂(g) is a violet coloured gas. both sour gas and hydrogen gas are colourless 

2H₂S(g) ---> 2H₂(g) + S₂(g)

state the effect each of the following stressers  will have on this system in terms of the colour of the system: darker violet, lighter violet, or no colour change to the colour of the system.