When 27.8 g of acetylene reacts with hydrogen, 21.4 g of ethane is produced. What is the percent yield of C2H6 for the reaction? C2H2(g)+2H2(g)→C2H6(g)
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
When 27.8 g of acetylene reacts with hydrogen, 21.4 g of ethane is produced. What is...
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.
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) 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.
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
When ethane, C2H6, reacts with chlorine, Cl2, the main product is C2H5Cl, but other products containing Cl such as C2H4Cl2 are also obtained in small quantities. C2H6 + Cl2 C2H5Cl + "Other Stuff" The formation of these other products reduces the yield of C2H5Cl. Using the stoichiometry given in the chemical formula above, calculate the percent yield of C2H5Cl if the reaction of 150 g of C2H6 with 230. g of Cl2 produced 170 g of C2H5Cl.
Problem 3: (Limiting and Excess Reactants): Hydrogenat (25%) tion of acetylene to form ethane is carried out in a continuous reactor. C2H2 +2H2 C2Hs The product stream is analyzed and found to contain 68.7 mole% C2H6 and 16 H2. The fractional conversion of the limiting reactant and the percentage by which the other reactant is in excess. The molar flow rate of the feed stream is 135 mol/h. .3% feed to the reactor contains only acetylene and hydrogen. Calculate the
When ethane (C2H6) reacts with chlorine (Cl2), the main product is C2H5Cl; but other products containing Cl, such as C2H4Cl2, are also obtained in small quantities. The formation of these other products reduces the yield of C2H5Cl. a. Calculate the theoretical yield of C2H5Cl when 111 g of C2H6 reacts with 207 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl. b. Calculate the percent yield of C2H5Cl if the reaction produces 161 g...
When 8.42 g of B2H9 reacts with 27.8 g O2 according to the equation : 2B2H9 + 12O2 → 5B2O3 + 9H2O 8.24 g H2O forms. What is the percent yield for the reaction.
Acetylene is hyrodgenated to form ethane. The feed to the reactor contains 1.70 mol H2/mol C2H2. The reaction proceeds to completion a. Calculate the stoichiometric reactant ratio (mol H2 reacted/mol C2H2 reacted) and the yield ratio (mol C2Hs formed/mol H2 reacted) mol H2 reacted/mol C2H2 reacted mol C2Hg formed/mol H2 reacted b. Determine the percentage by which acetylene is in excess. c. Calculate the mass feed rate of hydrogen (kg/s) required to produce 6.00 x 10s metric tons of ethane...
The gas ethane, C2H4, reacts with oxygen gas to form ethylene oxide, C2H4O, according to the unbalanced equation: C2H2(g) + O2(g) → C2H4O(g) What is the theoretical yield if ethylene oxide from 120.0g of ethane? If 180.0g of ethylene oxide is obtained from 120.0g of ethane, what is the percent yield?