Given an initial mass of 19.24 g H2, an excess of C2H4, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of C2H6 produced by the reaction.
Given an initial mass of 19.24 g H2, an excess of C2H4, and assuming that all...
H2(g) + I2(s) → 2HI(g) Given an initial mass of 15.28 g H2, an excess of I2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction.
Consider the reaction: H2(g) + I2(s) = 2HI (g) Given an initial mass of 19.02g H2 an excess of I2 and assuming that all of the reactant is conserved to products and non is lost calculate the mass (g) of HI produced by the reaction?
1. The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: H2(g) + C2H4(g) = C2H6(g) If 10.20 g H2 is mixed with 16.60 g C2H4, calculate the theoretical yield (g) of C2H6 produced by the reaction.
The reaction between ethene and hydrogen occurs according to the following stoichiometry. C2H4 (g) + H2 (g) → C2H6 (g) Which of the following statements is true? d[C2H4]/dt = +d[H2]/dt = –d[C2H6]/dt d[C2H4]/dt=–d[H2]/dt=+d[C2H6]/dt d[C2H4]/dt=+d[H2]/dt=+d[C2H6]/dt d[C2H4]/dt = –d[H2]/dt = –d[C2H6]/dt None of the above statements are true show working
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...
Ethene is converted to ethane by the reaction C2H4 (9) + H2(g) - C2H6(g) C2H4 flows into a catalytic reactor at 28.6 atm and 250.ⓇC with a flow rate of 1000. L/min. Hydrogen at 28.6 atm and 250°C flows into the reactor at a flow rate of 1400. L/min. If 14.7 kg C2H6 is collected per minute, what is the percent yield of the reaction? Submit Answer Try Another Version 5 item attempts remaining
A sample of C2H4 with a pressure of 1.78 atm and a volume of 295 mL is allowed to react with excess H2 at 151 °C. H2 (g) + C2H4 (g) C2H6 (g) Calculate the pressure of the C2H6 produced in the reaction if it is transferred to a 2.62-L flask and cooled to 34 °C.
A sample of C2H4 with a pressure of 1.70 atm and a volume of 299 mL is allowed to react with excess H2 at 190 °C. H2 (g) + C2H4 (g) ==> C2H6 (g) Calculate the pressure of the C2H6 produced in the reaction if it is transferred to a 1.12-L flask and cooled to 29 °C. atm
Estimate the enthalpy change for the following reaction : H2(g) + C2H4(g) -------> C2H6(g), given the following bond energies: BE(H-H) = 436 kJ/mol; BE(C-H) = 414 kJ/mol; BE(C-C) = 347 kJ/mol; BE(C=C) = 620 kJ/mol. A. -119 kJ B. +119 kJ C. -392 kJ D. +392 kJ E. none of the above
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 20 °C given that ∆rG° = -92.2 kJ mol-1, P(C2H4) = 1.41×10-2 bar, P(H2) = 1.47×10-2 bar, and P(C2H6) = 3.00×10-1 bar.