For the combustion of acetylene at 298.15 K, 2 C2H2(g) + 5 O2(g) →4 CO2(g) +...
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.
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.
loab beboo 2CO2 + H2O. 7. Calculate AH for C2H2 +5/202 Given C(s) +O2(g) CO2(g) AH = -393.5 kJ H2+½ O2 H2O AH= -285.8 kJ 2C+H2 C2H2 AH = 226.8 kJ 008700000 08.0 Lon Qoe cOeEo.O60
Find AHrxn for: C2H2(g) → 2C(s) + H2(g) given the following information: C2H2(g) + 5/2 O2(g) → 2002(g) + H2O (1) AH° = -1291 kJ C(s) + O2(g) + CO2(g) AH° = -391 kJ H2(g) + 1/2O2(g) + H2O(1) AH° = -280 kJ kJ
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...
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]
Calculate the standard enthalpy of formation of gaseous
acetylene (C2H2) using the following
thermochemical information:
2
C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(l)
H = -2599.3 kJ
CO2(g) C(s) + O2(g)
H = +393.5 kJ
2 H2O(l) 2 H2(g) + O2(g)
H = +571.7 kJ
H = 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 C How many grams of C2H, are present after the reaction is complete? VALO ? m = Бn Submit Request Answer
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?
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?