For the reaction: C2H2 (g) + 2 H2 (g) > C2H6 (g) , calculate and Keq at 25 degrees Celsius. Also, calculate Keq for this same reaction at 75 degrees Celsius.
Answers :
At 25 degrees Celsius, are -311.38 kJ, -242.09 kJ, -232.46 J respectively. Keq at 25 degrees Celsius is 3 x 1042; at 75 degrees Celsius it is 4 x 1034
For the reaction: C2H2 (g) + 2 H2 (g) > C2H6 (g) , calculate and Keq...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g)+2H2(g)?C2H6(g) Given the following data, what is the value of Kp for this reaction? Substance ?G?f (kJ/mol) C2H2(g) 209.2 H2(g) 0 C2H6(g) ?32.89 In Part A, we saw that ?G?=?242.1 kJ for the hydrogenation of acetylene under standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K ). In Part B, you will determine the ?G for the...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g)+2H2(g)⇌C2H6(g) Given the following data, what is the value of K for this reaction? Substance ΔfG∘ (kJ mol−1) C2H2(g) 209.2 H2(g) 0 C2H6(g) −32.89 Express your answer to two significant figures.
1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) + 3.5O2 (g) -----> 2CO2 (g) + 3H2O (l) ΔH2 = -1560 kJ/mo 3) C2H4 (g) + 3O2 (g) -----> 2CO2 (g) + 2H2O (l) ΔH3 = -1411 kJ/mol 4) 2H2O (l) -----> 2H2 (g) + O2 (g) ΔH4 = 571.6 kJ/mol How much heat is transferred between the system and the surroundings when 25 grams of ethane (C2H6) decomposes to produce ethylene (C2H4) and...
Given the following reactions and subsequent delta H values, C2H6 (g) -> C2H2 (g) + 2H2 (g) delta H= 283.5 kJ H2 (g) + 1/2 O2 (g) -> H2O (g) delta H= -213.7 kJ 2CO2 (g) + 3H2O (g) -> C2H6 (g) + H2O (g) delta H= 849 kJ Find the delta H for the reaction: C2H2 (g) + 5/2 O2 (g) -> 2CO2 (g) + H2O (g)
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g)+2H2(g)⇌C2H6(g) At 25 ∘C the reaction from ^ has a composition as shown in the table below. Substance Pressure (atm) C2H2(g) 5.35 H2(g) 5.75 C2H6(g) 5.25×10−2 What is the free energy change, ΔG, in kilojoules for the reaction under these conditions? Express your answer numerically in kilojoules.
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data. C2H4 (g) + 3 02 (®) → 2 CO2 (s) + 2 H20 (1) C2H6 (g) + 7/2 02(g) → 2 CO2(g) + 3 H20 (1) H2 + 1/2O2() → H20 (1) AH = -1411. kJ/mole AH = -1560. kJ/mole AH = -285.8 kJ/mole 2. Calculate AH for the reaction 4 NH3(g) +502 (g) → 4 NO(g) + 6 H20 (g), from the following...
C2H2 + 2H2 --> C2H6. If ΔH for the above reaction is -728 kJ, calculate the value of the carbon bond in C2H2.
Given the following information at 25°C, Calculate AS° for the h drogenas ethylene: C2H2(g) + 2H2(g) → C2H6(g) Sº Species J/(mol.K) H2(g) C2H2(g) C2H6(g) 130.68 200.94 229.60 a) 561.22 J/K Ob) 232.70 J/K Oc) -232.70 J/K d) -561.22 J/K
Determine Heat of reaction (Hrxn) for: 2 C (s, graphite) + 3 H2 (g) ------> C2H6 (g) from the following C (s, graphite) + O2 (g) ------> CO2 (g) delta H = -393.5 kJ H2 (g) + 1/2 O2 (g) ------> H2O (l) delta H = -285.8 kJ 2 C2H6 (g) + 7 O2 (g) ------> 6 H2O (l) + 4 CO2 (g) delta H = -3,119.6 kJ
1. Calculate the change in enthalpy for this reaction: 2C(s) + H2(g) → C2H2(g) Given the following AHo -1299.5 kJ HP =-393.5 kJ HP -285.8 kJ CHI2(g) + (5/2)O2(g) → 2CO2(g) + H2O(1) C(s) + O2(g) → CO2(g) H2(g) + (12)O2(g) → H2O(1) A balloon contains 0.45 g of carbon dioxide and 0.6 grams of helium at 1.1 bar. If you compress the container to 80%ofits original volume, what will be the final pressure? Half a liter of water is...