Homework Answers
Given:
ΔHo rxn = -2599.3 KJ/mol
From thermodynamics table:
Hof(O2(g)) = 0.0 KJ/mol
Hof(CO2(g)) = -393.509 KJ/mol
Hof(H2O(l)) = -285.83 KJ/mol
Balanced chemical equation is:
2 C2H2(g) + 5 O2(g) ---> 4 CO2(g) + 2 H2O(l)
ΔHo rxn = 4*Hof(CO2(g)) + 2*Hof(H2O(l)) - 2*Hof( C2H2(g)) - 5*Hof(O2(g))
-2599.3 = 4*(-393.509) + 2*(-285.83) - 2*Hof(C2H2(g)) - 5*(0.0)
Hof(C2H2(g)) = 226.802 KJ/mol
Answer: 226.80 KJ/mol
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The thermochemical equation for the combustion of acetylene gas, C2H2(g), is 2CH2(g) + 502(g) – 4C02(g)...
all 3. Calculate the heat released (kJ) in the reaction of 1.35L of acetylene (C2H2) and 0.235L of hydrogen gas at...
all 3. Calculate the heat released (kJ) in the reaction of 1.35L of acetylene (C2H2) and 0.235L of hydrogen gas at STP to form ethane gas as determined by the following equation: C2H2(g) + 2H2() → C2H6(g) Given: 2C2H2(g) +502(g) + 4CO2(g) + 2H20(g) 2C2H.(g) + 702(g) → 4CO2(g) + 6H20(g) 2H2(g) + O2(g) → 2H2O(g) AH = -2320 kJ/mol AH = -3040 kJ/mol AH = -572 kJ/mol
Put it together: Acetylene, C2H2, is a gas commonly used in welding. It is formed in...
Put it together: Acetylene, C2H2, is a gas commonly used in welding. It is formed in the reaction of CaC2, with water. Given the thermochemical equations below, calculate the value of AH for acetylene. NOTE: This doesn't give you the equation you are shooting for -you must come up with that on your own. Notice the word formation. 2.30 J CaO(s)+H20 Ca(OH)26s) AH°=-65.3 kJ/mole AH°=+462.3 kJ/mole CaO()+3 Cs)CaC2(s)+COe) AHO+178 kJ/mole CACO 3()CaO) +CO2(e CaC2(0)+2H2Om) Ca(OH)2)C2H2 AH-126 kJ/mole AHO-220 kJ/mole 2C19)...
Acetylene burns in air to produce carbon dioxide and water: C2H2(g) + 5/2O2(g) → 2CO2(g) +...
Acetylene burns in air to produce carbon dioxide and water: C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(l). Use the following thermochemical equations to obtain ΔGr0 at 25 °C for the combustion of acetylene: C2H2(g) + 3H2(g) → 2CH4(g) ΔGr0 = −310.7 kJ/mol at 25 °C CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔGr0 = −817.97 kJ/mol at 25 °C H2(g) + 1/2O2(g) → H2O(l). ΔGr0 = −237.18 kJ/mol at 25 °C
1. Acetylene (C2H2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given...
1. Acetylene (C2H2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given AH [CO2(g)] = -393.5 kJ/mol, AH [H20(8)] = -241.8 kJ/mol, and AH[C2H2(g) = 226.6 kJ/mol, how much energy is released (kJ) when 92.5L of CO2 gas are produced at 225atm and 785°C?
5. How much heat is produced by the combustion of 5.25 g of acetylene (C2H2, 26.036...
5. How much heat is produced by the combustion of 5.25 g of acetylene (C2H2, 26.036 g/mol)? 2C2H2+502( 4CO2(@+ 2H20( AH -2602 kJ a) 131 kJ b) 262 kJ c) 496 kJ d) 6830 k e) 13660 kJ 10 6. How many grams of Nal (149.89 g/mol) are required to produce 92.2 g of Pbl2 (461.00 g/mol)? Pb(NO 3)2(aq) + 2NaI (a) Pbl2)+ 2NANO3(ag) a) 567 g b) 284 g c) 60.0 g d) 30.0 g e) 92.9 g
it has the answers I just don't know how to get them. Write an chemical equation...
it has the answers I just don't know how to get them.
Write an chemical equation for the reaction corresponding to the enthalpy of formation of 9. acetylene, C2H2. 2Cgraphite +H2(g)-C2H2(g) 10. Write a chemical equation for combustion of acetylene under standard thermodynamic conditions 2C2H2(g)502g)4C02(g) 2H20(l) 11 12. Determine the standard enthalpy change for the combustion of acetylene. AH° = -2600 kJ/2mol or AH° = -1300 kJ/mol
5. An acetylene torch works according to the following reaction: C2H2(g) +502(g) – 2 CO2(g) +...
5. An acetylene torch works according to the following reaction: C2H2(g) +502(g) – 2 CO2(g) + H20(g) AH = -1255.5 kJ Calculate the change in internal energy, AE, when 15.5 g of acetylene reacts against an external pressure of 1,00 atm and after the products are able to return to 25°C. [ANSWER: -747 kJ]
Acetylene gas, C2H2(g), is used in welding. C2H2(g)+52O2(g)→2CO2(g)+H2O(l) Part B How much heat is produced in...
Acetylene gas, C2H2(g), is used in welding. C2H2(g)+52O2(g)→2CO2(g)+H2O(l) Part B How much heat is produced in burning 4 mol of C2H2 under standard conditions if both reactants and products are brought to 298 K? Express your answer using five significant figures. ΔH Δ H = kJ Part C What is the maximum amount of useful work that can be accomplished under standard conditions by this reaction when 4 mol of C2H2 is burned? Express your answer using five significant figures.
The combustion of acetylene C2H2, takes place according to the equation: 2C2H2 + 5O2 ---> 4CO2...
The combustion of acetylene C2H2, takes place according to the equation: 2C2H2 + 5O2 ---> 4CO2 + 2H2O; delta H is -5198 kJ In an experiment, 0.338 g C2H2 is combusted in a bomb calorimeter. If the heat capacity of the calorimeter is 729 J/K and it contains 1/150 kg of water, what is the temperature increase of the bomb calorimeter? The spedicif heat capacity of water is 4/184 J/g.K
1. Acetylene (C2H2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given...
1. Acetylene (C2H2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given AHC02(8)] = -393.5 kl/mol, AH® [H20(8)] = -241.8 kJ/mol, and AH(CH2(g)] = 226.6 kJ/mol, how much energy is released (kl) when 32.5L of CO2 gas are produced at 3.5atm and 255°C? 2C₂H2 (g) + 302 (5) 4CO2(g) + 2 H₂Org)
all 3. Calculate the heat released (kJ) in the reaction of 1.35L of acetylene (C2H2) and 0.235L of hydrogen gas at STP to form ethane gas as determined by the following equation: C2H2(g) + 2H2() → C2H6(g) Given: 2C2H2(g) +502(g) + 4CO2(g) + 2H20(g) 2C2H.(g) + 702(g) → 4CO2(g) + 6H20(g) 2H2(g) + O2(g) → 2H2O(g) AH = -2320 kJ/mol AH = -3040 kJ/mol AH = -572 kJ/mol
Put it together: Acetylene, C2H2, is a gas commonly used in welding. It is formed in the reaction of CaC2, with water. Given the thermochemical equations below, calculate the value of AH for acetylene. NOTE: This doesn't give you the equation you are shooting for -you must come up with that on your own. Notice the word formation. 2.30 J CaO(s)+H20 Ca(OH)26s) AH°=-65.3 kJ/mole AH°=+462.3 kJ/mole CaO()+3 Cs)CaC2(s)+COe) AHO+178 kJ/mole CACO 3()CaO) +CO2(e CaC2(0)+2H2Om) Ca(OH)2)C2H2 AH-126 kJ/mole AHO-220 kJ/mole 2C19)...
1. Acetylene (C2H2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given AH [CO2(g)] = -393.5 kJ/mol, AH [H20(8)] = -241.8 kJ/mol, and AH[C2H2(g) = 226.6 kJ/mol, how much energy is released (kJ) when 92.5L of CO2 gas are produced at 225atm and 785°C?
5. How much heat is produced by the combustion of 5.25 g of acetylene (C2H2, 26.036 g/mol)? 2C2H2+502( 4CO2(@+ 2H20( AH -2602 kJ a) 131 kJ b) 262 kJ c) 496 kJ d) 6830 k e) 13660 kJ 10 6. How many grams of Nal (149.89 g/mol) are required to produce 92.2 g of Pbl2 (461.00 g/mol)? Pb(NO 3)2(aq) + 2NaI (a) Pbl2)+ 2NANO3(ag) a) 567 g b) 284 g c) 60.0 g d) 30.0 g e) 92.9 g
it has the answers I just don't know how to get them.
Write an chemical equation for the reaction corresponding to the enthalpy of formation of 9. acetylene, C2H2. 2Cgraphite +H2(g)-C2H2(g) 10. Write a chemical equation for combustion of acetylene under standard thermodynamic conditions 2C2H2(g)502g)4C02(g) 2H20(l) 11 12. Determine the standard enthalpy change for the combustion of acetylene. AH° = -2600 kJ/2mol or AH° = -1300 kJ/mol
5. An acetylene torch works according to the following reaction: C2H2(g) +502(g) – 2 CO2(g) + H20(g) AH = -1255.5 kJ Calculate the change in internal energy, AE, when 15.5 g of acetylene reacts against an external pressure of 1,00 atm and after the products are able to return to 25°C. [ANSWER: -747 kJ]
1. Acetylene (C2H2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given AHC02(8)] = -393.5 kl/mol, AH® [H20(8)] = -241.8 kJ/mol, and AH(CH2(g)] = 226.6 kJ/mol, how much energy is released (kl) when 32.5L of CO2 gas are produced at 3.5atm and 255°C? 2C₂H2 (g) + 302 (5) 4CO2(g) + 2 H₂Org)
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