The second-order rate constant for the following gas-phase reaction is 0.048 1/MLaTeX: \cdot⋅s. We start with...
The second-order rate constant for the following gas-phase reaction is 0.048 1/MLaTeX: \cdot⋅s. We start with 0.136 mol C2F4 in a 2.47 liter container, with no C4F8 initially present. C2F4 LaTeX: \longrightarrow⟶ 1/2 C4F8 What will be the concentration of C2F4 after 1.61 hours? Enter to 4 decimal places.
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The second-order rate constant for the following gas-phase
reaction is 0.048 1/MLaTeX: \cdot⋅s. We start with...
The second-order rate constant for the following gas-phase reaction is 0.043 1/M?s. We start with 0.497...
The second-order rate constant for the following gas-phase
reaction is 0.043 1/M?s. We start with 0.497 mol C2F4 in a 2.23 liter
container, with no C4F8 initially present.
C2F4 ? 1/2 C4F8
What will be the concentration of C4F8 after 2.17 hours? Enter
to 4 decimal places. HINT: You will need to figure out how much of
C2F4 was used (that is the only material that can be converted to
the product).
The second order gas phase irreversible reaction: 2.4-B is carried out in an isothermal batch reactor...
The second order gas phase irreversible reaction: 2.4-B is carried out in an isothermal batch reactor containing 40 kg of catalyst and with an initial volume of 60-liter. The reactor is initially filled with equal molar quantities of A and inert I at 300 K and 2.5 atm. Calculate the time needed for the concentration of product (B) to be 0.02 mole/liter if: a) the reaction takes in a constant pressure batch reactor (3 points) b) the reaction takes place...
The second order rate constant of the following gas phase reaction at 338°C was found to...
The second order rate constant of the following gas phase reaction at 338°C was found to be 7.5 x 10-4dm-mol-15-1: H2+C2H4 → CHE Determine k2 at 113°C assuming the activation energy and the collision cross sections are constants (ignore the steric factor).
The reaction A --> Products is second order with a rate constant of 0.2500 L mol-1...
The reaction A --> Products is second order with a rate constant of 0.2500 L mol-1 s-1. If we start with a 1.000 M concentration of A, what is the rate of the reaction (in mol L-1 s-1) after 20 s? Your answer should be rounded up to four decimal places.
For the reaction 2NO2 + F2 2NO2F, the rate constant is 38M-1s-1. The reaction is first...
For the reaction 2NO2 + F2 2NO2F, the rate constant is 38M-1s-1. The reaction is first order in NO2 and first order in F2, being of the second order total. Calculate the concentration of NO2, F2, and NO2F present after 30.0 seconds, if initially 3.00 mol of NO2 are mixed. with 1.00 mol of F2 in a container of 400 dm3 at 27oC.
The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 → CH4 + H2...
The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 → CH4 + H2 + CO is 3.2 x 10-4 5-1 at 450°C. The reaction is carried out in a constant-volume container. Initially, only dimethyl ether is present, and the pressure is 0.343 atm. What is the pressure of the system after 8.1 min? Assume ideal-gas behavior. 49) 0.29 x 0.44 atm
The second order rate constant of the following gas phase reaction at 338°C was found to...
The second order rate constant of the following gas phase reaction at 338°C was found to be 7.5x 10'dm-mol's H2+C2Ha C2H6 Determine K2 at 113°C assuming the activation energy and the collision cross ross sections are constants (ignore the steric factor). • 6.0x10-4 M 1-1 1.2x10-7 MS1 5.0x10-5-1 4.3x10-4M-'s
12. The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K...
12. The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K is 54.7 and the reaction is: Br2(g) +F2(g) 2 BrF(g) What is the equilibrium concentration of fluorine if the initial concentrations of bromine and fluorine were 0.125 moles/liter in a sealed container and no product was present initially? Submit Answer Tries 0/99
1) 2) 3) 4) The equilibrium constant for the gas phase reaction 2803 (g) = 2802...
1)
2)
3)
4)
The equilibrium constant for the gas phase reaction 2803 (g) = 2802 (g) + O2 (g) is Keg = 7.1 x 102 at 999 K. At equilibrium,_ O only reactants are present O roughly equal amounts of products and reactants are present products predominate only products are present reactants predominate QUESTION 20 The rate law of a reaction is rate = k[X]-. The units of the rate constant are O mol L-15-2 OL mol-15-1 O mol2...
The gas phase reaction OH(g) + CH4(g) → H2O(g) + CH(g) is second order overall and...
The gas phase reaction OH(g) + CH4(g) → H2O(g) + CH(g) is second order overall and first order in both reactants. The initial rate of appearance (measured at constant volume and temperature) of HO as a function of temperature is given in the table below. The initial concentration of OH and CH, is 0.500 mol m23. (a) Calculate the Arrhenius parameters for the rate constant. (b) Calculate the initial rate and concentration of OH and H,O after 1 ms at...
The second-order rate constant for the following gas-phase
reaction is 0.043 1/M?s. We start with 0.497 mol C2F4 in a 2.23 liter
container, with no C4F8 initially present.
C2F4 ? 1/2 C4F8
What will be the concentration of C4F8 after 2.17 hours? Enter
to 4 decimal places. HINT: You will need to figure out how much of
C2F4 was used (that is the only material that can be converted to
the product).
The second order gas phase irreversible reaction: 2.4-B is carried out in an isothermal batch reactor containing 40 kg of catalyst and with an initial volume of 60-liter. The reactor is initially filled with equal molar quantities of A and inert I at 300 K and 2.5 atm. Calculate the time needed for the concentration of product (B) to be 0.02 mole/liter if: a) the reaction takes in a constant pressure batch reactor (3 points) b) the reaction takes place...
The second order rate constant of the following gas phase reaction at 338°C was found to be 7.5 x 10-4dm-mol-15-1: H2+C2H4 → CHE Determine k2 at 113°C assuming the activation energy and the collision cross sections are constants (ignore the steric factor).
The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 → CH4 + H2 + CO is 3.2 x 10-4 5-1 at 450°C. The reaction is carried out in a constant-volume container. Initially, only dimethyl ether is present, and the pressure is 0.343 atm. What is the pressure of the system after 8.1 min? Assume ideal-gas behavior. 49) 0.29 x 0.44 atm
The second order rate constant of the following gas phase reaction at 338°C was found to be 7.5x 10'dm-mol's H2+C2Ha C2H6 Determine K2 at 113°C assuming the activation energy and the collision cross ross sections are constants (ignore the steric factor). • 6.0x10-4 M 1-1 1.2x10-7 MS1 5.0x10-5-1 4.3x10-4M-'s
12. The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K is 54.7 and the reaction is: Br2(g) +F2(g) 2 BrF(g) What is the equilibrium concentration of fluorine if the initial concentrations of bromine and fluorine were 0.125 moles/liter in a sealed container and no product was present initially? Submit Answer Tries 0/99
1)
2)
3)
4)
The equilibrium constant for the gas phase reaction 2803 (g) = 2802 (g) + O2 (g) is Keg = 7.1 x 102 at 999 K. At equilibrium,_ O only reactants are present O roughly equal amounts of products and reactants are present products predominate only products are present reactants predominate QUESTION 20 The rate law of a reaction is rate = k[X]-. The units of the rate constant are O mol L-15-2 OL mol-15-1 O mol2...
The gas phase reaction OH(g) + CH4(g) → H2O(g) + CH(g) is second order overall and first order in both reactants. The initial rate of appearance (measured at constant volume and temperature) of HO as a function of temperature is given in the table below. The initial concentration of OH and CH, is 0.500 mol m23. (a) Calculate the Arrhenius parameters for the rate constant. (b) Calculate the initial rate and concentration of OH and H,O after 1 ms at...
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