Question 22 Acetylene burns according to the following equation. C2H2(g) + 5/2 O2(g) --> 2 CO2(g)...
Question 22 Acetylene burns according to the following equation. C2H2(g) + 5/2 O2(g) --> 2 CO2(g) + H2O(g) \DeltaΔΔHorxn = -1255.8 kJ What is the \DeltaΔΔH for the reaction if 5.50 grams of acetylene (C2H2) burns completely?
-4.38 J
-228 J
-531 J
Correct Answer -265 J
-6910 J
PLEASE SHOW THE WORK SO I CAN UNDERSTAND.
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Question 22 Acetylene burns according to the following equation.
C2H2(g) + 5/2 O2(g) --> 2 CO2(g)...
For the combustion of acetylene at 298.15 K, 2 C2H2(g) + 5 O2(g) →4 CO2(g) +...
For the combustion of acetylene at 298.15 K, 2 C2H2(g) + 5 O2(g) →4 CO2(g) + 2 H2O(g) calculate ASⓇ(universe) given AS (system) = -194.6 J/K and AH°(system) = -2511.2 kJ. +8228.0 J/K +1290.4 J/K 0 -186.2 J/K +186.2 JK 0-2453.2 J/K
2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2 2 C2H2 + 5 O2...
2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2 2 C2H2 + 5 O2 (g) 4 CO2 (g) + 2 H2O (g) If the enthalpy change for the reaction is -251 1.14 kJ/mol, a) How much heat can be produced by the reaction of 10 g of C2H2? b) Is it an endotherm ic or exothermic reaction? Molar mass of acetylene is 26.04 g/mol.
Write a Balanced equation for the chemcial reaction Acetylene gas (C2H2) burns in a welding torch with oxygen to form carbon dioxide gas and water vapor
Write a balanced equation for the chemical reaction Acetylene gas (C2H2) burns in a welding torch with oxygen to form carbon dioxide gas and water vapor.C2H2(g) + O2(g) ==> CO2(g) + H2O(g) It isn't balanced. I will leave that for you.How do I balance it?trial and error. C2H2 + O2 ==> CO2 + H2O. I see 2 C on the left and only 1 on the right so I place a coefficient of 2 for CO2 on the right. And...
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is...
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H20. The unbalanced equation for this reaction is shown below: C2H2 + O2 +CO2 + H2O Part C How many grams of C2H, are present after the reaction is complete? VALO ? m = Бn Submit Request Answer
When a mixture of 11.0 g of acetylene (C2H2) and 11.0 g of oxygen (O2) is...
When a mixture of 11.0 g of acetylene (C2H2) and 11.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H2O. a) How many grams of C2H2 are present after the reaction is complete? b) How many grams of O2 are present after the reaction is complete? c)How many grams of CO2 are present after the reaction is complete? d)How many grams of H2O are present after the reaction is complete?
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 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
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is...
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H20. The unbalanced equation for this reaction is shown below. C2H2 + O2 CO2 + H2O Part A Write the coefficients in the balanced equation in the order the substances are written. Templates Symbols undo rédo reset keyboard shortcuts 'help ΑΣ και C2H2, O2, CO2, H2O Submit Request Answer Part B Which is the limiting reactant?...
use the following table for the reaction C2H2 (g) + 5/2 O2 (g) = 2CO2 (g)...
use the following table for the reaction C2H2 (g) + 5/2 O2 (g) = 2CO2 (g) + H2O (g) delta H = -1255.5 KJ/mol substance S (J. mol-1. K-1) C2H2 (g) 200.8 C2H4 (g) 219.5 CO (g) 197.6 CO2 (g) 213.6 CO2 (aq) 117.6 H2O (l) 69.91 H2O (g) 188.7 O2 (g) 205.0 O (g) 161.0 O3 (g) 238.8 a. Use the data to calculate delta S in J/K for this reaction b. Calculate delta G in KJ , since the...
Acetylene burns in oxygen to give CO2 and H20 according to the equation below. 2 CH2(g)...
Acetylene burns in oxygen to give CO2 and H20 according to the equation below. 2 CH2(g) +502(g) — 4CO2(g) + 2 H20(g) What volume of oxygen will react completely with 33 L CH?! 170L 13L 83 L 66L 33 L Submit Answer Try Another Version 2 item attempts remaining 1 PE pl
For the combustion of acetylene at 298.15 K, 2 C2H2(g) + 5 O2(g) →4 CO2(g) + 2 H2O(g) calculate ASⓇ(universe) given AS (system) = -194.6 J/K and AH°(system) = -2511.2 kJ. +8228.0 J/K +1290.4 J/K 0 -186.2 J/K +186.2 JK 0-2453.2 J/K
2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2 2 C2H2 + 5 O2 (g) 4 CO2 (g) + 2 H2O (g) If the enthalpy change for the reaction is -251 1.14 kJ/mol, a) How much heat can be produced by the reaction of 10 g of C2H2? b) Is it an endotherm ic or exothermic reaction? Molar mass of acetylene is 26.04 g/mol.
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H20. The unbalanced equation for this reaction is shown below: C2H2 + O2 +CO2 + H2O Part C How many grams of C2H, are present after the reaction is complete? VALO ? m = Бn Submit Request Answer
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]
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H20. The unbalanced equation for this reaction is shown below. C2H2 + O2 CO2 + H2O Part A Write the coefficients in the balanced equation in the order the substances are written. Templates Symbols undo rédo reset keyboard shortcuts 'help ΑΣ και C2H2, O2, CO2, H2O Submit Request Answer Part B Which is the limiting reactant?...
Acetylene burns in oxygen to give CO2 and H20 according to the equation below. 2 CH2(g) +502(g) — 4CO2(g) + 2 H20(g) What volume of oxygen will react completely with 33 L CH?! 170L 13L 83 L 66L 33 L Submit Answer Try Another Version 2 item attempts remaining 1 PE pl
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