The decomposition of iodoethane in the gas phase proceeds according to the following equation. C2H5I(g) →...

Question

Question

The decomposition of iodoethane in the gas phase proceeds according to the following equation.

C₂H₅I(g) → C₂H₄(g) + HI(g)

At 660. K, k = 7.2 ✕ 10⁻⁴ s⁻¹; at 720. K, k = 1.7 ✕ 10⁻² s⁻¹. What is the rate constant for this first-order decomposition at 336°C?

If the initial pressure of iodoethane is 880. torr at 245°C, what is the pressure of iodoethane after three half-lives?

science chemistry

Answer 1

Similar Homework Help Questions

Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows C2H5I(g) rightarrow...

Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows C2H5I(g) rightarrow C2H4(g) + HI(g) From the following data, determine the rate constant of this reaction. Begin by constructing a plot to verify that the reaction is first order.
10) Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows: C2H5I(g)...

10) Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows: C2H5I(g) → C2H4(g) + HI(g) From the following data determine the order of the reaction and the rate constant. Time (min) [C2H5I] (M) 0.0 2.00 15.0 1.82 30.0 1.64 48.0 1.42 75.0 1.10 1) Reaction order: a) 0 b) 1 c) 2 2) Rate Constant: (enter only the numerical value of the rate constant). _______
Given the following equation, C2H5I (g) ⇒ C2H4 (g) + HI (g) k= 4.0 * 10^-3...

Given the following equation, C2H5I (g) ⇒ C2H4 (g) + HI (g) k= 4.0 * 10^-3 s^ -1 at 700K a. Write the rate law. b. what is the rate of reaction when {C2H5I}=3.3x10^-4mol/L? c. if the concentration is doubled, what is the effect on the reaction? d. What is the half life? 2. Given the following equation 2C2H2=C4H4 K=0.178 L/mol at 770K a. write the rate law b. what is the rate of reaction when C2H2=0.195M c. what is...

The gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g) + ½ I2(g) is...

The gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g) + ½ I2(g) is second order in HI with a rate constant of 1.20×10-3 M-1 s-1. If the initial concentration of HI is 2.22 M, the concentration of HI will be _____________________M after 2.21×103 seconds have passed.
1. The activation energy for the gas phase decomposition of chloroethane is 254 kJ. CH3CH2Cl--->C2H4 +...

1. The activation energy for the gas phase decomposition of chloroethane is 254 kJ. CH3CH2Cl--->C2H4 + HCl The rate constant at 750 K is 7.99×10-4 /s. The rate constant will be 5.61×10-3 /s at_____ K 2. The activation energy for the gas phase decomposition of chloroethane is 254 kJ. CH3CH2Cl--->C2H4 + HCl The rate constant at 756 K is 1.09×10-3 /s. The rate constant will be___ /s at 786 K.
The decomposition of N2O5 proceeds according to the following equation: 2 N2O5 (g) -> 4 NO2...

The decomposition of N2O5 proceeds according to the following equation: 2 N2O5 (g) -> 4 NO2 (g) + O2 (g) If the rate of decomposition of N2O5 at a particular instant in a reaction vessel is 5.3 x 10-5 M/s, what is the rate of appearance of NO2?

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g)...

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g) + ½ I2(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.68×10-3 M-1 s-1 and a y-intercept of 2.66 M-1. Based on this plot, the reaction is ______ (zero/first/second) order in HI and the rate constant for the reaction is _____...
The decomposition of N2O5 proceeds according to the following equation 2 N2O5(g) → 4 NO2(g) +...

The decomposition of N2O5 proceeds according to the following equation 2 N2O5(g) → 4 NO2(g) + O2(g). The rate constant, k, for the reaction at 298 K is 2.20 x 10-3 min-1. If a reaction is set up in a vessel at 298 K, with an initial concentration of 0.278 mol L-1; what is the concentration of reactant N2O5(g) in mol/L after 40.2 minutes? Report your answer without units
The activation energy for the gas phase decomposition of ethyl acetate is 200 kJ. CH3COOC2H5 -->...

The activation energy for the gas phase decomposition of ethyl acetate is 200 kJ. CH3COOC2H5 --> CH3COOH + C2H4 The rate constant at 670 K is 8.41×10-4 /s. The rate constant will be 1.14×10-2 /s at _____ K.

The gas phase decomposition of hydrogen iodide at 700 K HI(g)%H2(g) + 12() is second order...

The gas phase decomposition of hydrogen iodide at 700 K HI(g)%H2(g) + 12() is second order in HI with a rate constant of 1.20x10-'M',' If the initial concentration of HI is 1.48 M, the concentration of HI will be M after 1.34x10 seconds have passed.