The time to fracture for a vitreous silica-glass fiber at +50 ∘C is 104 s. What...
The time to fracture for a vitreous silica-glass fiber at +50 ∘C is 104 s. What will be the time to fracture at room temperature (25 ∘C) ? Assume the activation energy is 78.6 kJ/mol.
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The time to fracture for a vitreous silica-glass fiber at +50 ∘C
is 104 s. What...
The viscosity n of a glass varies with temperature according to the relationship Qvis n =...
The viscosity n of a glass varies with temperature according to the relationship Qvis n = A expo RT where Qvis is the energy of activation for viscous flow, A is a temperature-independent constant, and R and T are, respectively, the gas constant and the absolute temperature. A plot of In versus 1/T should be nearly linear, and with a slope of Qvis/R. Using data taken from the figure below, make such a plot (i.e., In n versus 1/T) for...
An uncatalyzed reaction has a rate of 4.4 x 10-7 s–1 at room temperature (25 °C)....
An uncatalyzed reaction has a rate of 4.4 x 10-7 s–1 at room temperature (25 °C). When an enzyme is added the rate is 3.1 x 104 s–1. If the height of the activation barrier for the uncatalyzed rate is 28.6 kcal/mol, what is the height of the activation barrier for the catalyzed rate? Report your answer in terms of kcal/mol to the nearest tenths. Also, assume the pre-exponential terms for the uncatalyzed and catalyzed reactions are the same.
For the first-order reaction: Ag) — Bg) the rate constant is k-6x 104 s-at -10°C, and...
For the first-order reaction: Ag) — Bg) the rate constant is k-6x 104 s-at -10°C, and the activation energy is 64 kJ/mol. What is the rate constant at 20°C? (R-8.314 J/mol x K) 0 a. 6x 10451 b.4.3 x 1045-1 OC. 4.1 x 10851 Od. 1.2 x 10051 Oe-2.2 x 1045-1
The half-life for the reaction below was determined to be 2.14 x 104 s at 800...
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 226.00 kJ/mol N20(g)N2(8) +0(g) 4th attempt See Periodic Table See Hint What would be the half-life at 1050.43 K? 33.3
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life...
3) The rate constant of a first order reaction is 2.6 x 10+ s' at 255 °C. If the activation energy is 99.9 KJ/mol,...
3) The rate constant of a first order reaction is 2.6 x 10+ s' at 255 °C. If the activation energy is 99.9 KJ/mol, calculate the temperature at which its rate constant is 4.8 x 104 sl.
The half-life for the reaction was determined to be 2.14 × 104 s at 800 K....
The half-life for the reaction was determined to be 2.14 × 104 s at 800 K. The value of the half-life is independent of the inital concentration of N2O present. The activation energy of the reaction is 259.00 kJ/mol. N2O(g)->N2(g)+O(g) what would be the half life at 900.10K?
a.) The rate constant for the base-catalyzed hydrolysis of ethyl acetate is 1.78×103 L mol-1 s...
a.) The rate constant for the base-catalyzed hydrolysis of ethyl acetate is 1.78×103 L mol-1 s -1 at 25 °C and 1.38×104 L mol-1 s -1 at 37 °C. Calculate EA, (delta)H‡ , the Arrhenius Constant, and (delta) S ‡ . b.) The isomerization of HNC into HCN is important in the chemistry of interstellar gas clouds. HNC → HCN Has an activation energy of 210 kJ/mol and an activation entropy of -105 J mol-1 K-1 . Calculate the first-order...
For the decomposition of a peroxide, the activation energy is 17.4 kJ/mol. The rate constant at...
For the decomposition of a peroxide, the activation energy is 17.4 kJ/mol. The rate constant at 25°C is 0.027 s-1. What is the rate constant at 45°C? For the decomposition of a peroxide, the activation energy is 17.4 kJ/mol. The rate constant at 25°C is 0.027 s-1. At what temperature will the rate constant be 35% greater than the rate constant at 25°C?
The rate constant of a chemical reaction is 9.79 s-1 at a temperature of 22.4 °C....
The rate constant of a chemical reaction is 9.79 s-1 at a temperature of 22.4 °C. If the activation energy is 52.6 kJ mol-1, what is the rate constant (in s-1) at 53.6 °C?
The rate constant of a chemical reaction is 3.45 s-1 at a temperature of 25.1 °C....
The rate constant of a chemical reaction is 3.45 s-1 at a temperature of 25.1 °C. If the activation energy is 60.1 kJ mol-1, what is the rate constant (in s-1) at 52.2 °C?
The viscosity n of a glass varies with temperature according to the relationship Qvis n = A expo RT where Qvis is the energy of activation for viscous flow, A is a temperature-independent constant, and R and T are, respectively, the gas constant and the absolute temperature. A plot of In versus 1/T should be nearly linear, and with a slope of Qvis/R. Using data taken from the figure below, make such a plot (i.e., In n versus 1/T) for...
For the first-order reaction: Ag) — Bg) the rate constant is k-6x 104 s-at -10°C, and the activation energy is 64 kJ/mol. What is the rate constant at 20°C? (R-8.314 J/mol x K) 0 a. 6x 10451 b.4.3 x 1045-1 OC. 4.1 x 10851 Od. 1.2 x 10051 Oe-2.2 x 1045-1
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 226.00 kJ/mol N20(g)N2(8) +0(g) 4th attempt See Periodic Table See Hint What would be the half-life at 1050.43 K? 33.3
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life...
3) The rate constant of a first order reaction is 2.6 x 10+ s' at 255 °C. If the activation energy is 99.9 KJ/mol, calculate the temperature at which its rate constant is 4.8 x 104 sl.
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