1.When CO(g) reacts with NO(g) to form CO 2 (g) and N 2 (g) , 373 kJ of energy a
ID: 1005799 • Letter: 1
Question
1.When CO(g) reacts with NO(g) to form CO2(g) and N2(g) , 373 kJ of energy are evolved for each mole of CO(g) that reacts.
Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive.
Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank.
A.When H2S(g) reacts with H2O(l) to form H2(g) and SO2(g), 295 kJ of energy are absorbed for each mole of H2S(g) that reacts.
Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive.
Use the SMALLEST INTEGER coefficients possible and put the energy term in the last box on the appropriate side of the equation. If a box is not needed, leave it blank.
B.The following thermochemical equation is for the reaction of nitrogen(g) with hydrogen(g) to form ammonia(g).
How many grams of N2(g) would have to react to produce 30.7 kJ of energy?
grams ___
B.The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g).
When 59.2 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are _________evolvedabsorbed.
Hint: An amount of energy is expressed as a positive number. The sign indicates whether the energy is absorbed or evolved.
C.The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g).
When 59.2 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are
D>Ethanol, C2H6O, is most often blended with gasoline - usually as a 10 per cent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The heat of combustion of ethanol is 326.7 kcal/mol.
The heat of combustion of hexane, C6H14, is 995.0 kcal/mol. How much energy is released during the complete combustion of 379grams of hexane ?
kcal
Assuming the same efficiency, would 379 grams of ethanol provide more, less, or the same amount of energy as 379 grams ofhexane? _________morelessthe same amount
E.Hydrocarbons, compounds containing only carbon and hydrogen, are important in fuels.
The heat of combustion of cyclopropane, C3H6, is 499.8 kcal/mol.
Write a balanced equation for the complete combustion of cyclopropane.
How much energy is released during the complete combustion of 433 grams of cyclopropane ?
kcal
F.
The standard enthalpy change for the following reaction is 74.8 kJ at 298 K.
What is the standard enthalpy change for this reaction at 298 K?
kJ
G.The standard enthalpy change for the following reaction is -579 kJ at 298 K.
What is the standard enthalpy change for the reaction at 298 K?
kJ
H.
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
I.A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter.
In the laboratory a student burns a 0.303-g sample of pyrene (C16H10) in a bomb calorimeter containing 1010. g of water. The temperature increases from 25.70 °C to 28.00 °C. The heat capacity of water is 4.184 J g-1°C-1.
The molar heat of combustion is 7851 kJ per mole of pyrene.
Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter = J/°C
J,
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.
A student heats 68.73 grams of magnesium to 98.02 °C and then drops it into a cup containing 76.51grams of water at 24.13 °C. She measures the final temperature to be 37.68 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.52 J/°C.
Assuming that no heat is lost to the surroundings calculate the specific heat of magnesium.
Specific Heat (Mg) = J/g°C.
K.
Explanation / Answer
1. 2CO(g) + 2NO(g) <-----> 2CO2(g) + N2(g) DHrxn = -373 kj/mol
B. N2(g) + 3H2(g) -----> 2NH3(g) DHrxn = -92.2 kJ
from the data
28 grams of N2 = 92.2kj
? = 30.7 kj
mass of N2 required = 30.7*28/92.2 = 9.32 grams
B. Fe2O3(s) + 3H2(g) ---> 2Fe(s) + 3H2O(g) dH = 98.8 kJ
No of mol of Fe2O3 = 59.2/159.69 = 0.37 mol
amount of energy released = 98.8*0.37 = 36.556 kj
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