a) Given these data for the reaction , write the rate-law expression.
(Use k for the rate constant.)
Rate = _______ The specific rate constant = ___________
Expt. |
Initial [A] (M) |
Initial [B] (M) |
Initial Rate of Formation of C () |
1 | 0.15 | 0.40 | 4x10^-5 |
2 | 0.15 | 0.80 | 1.6x10^-4 |
3 | 0.30 | 1.6 | 1.3x10^-3 |
b) The rate of the elementary reaction
has been studied as a function of temperature between
300 and 2500 K. The following
data were obtained for the rate constant k:
Temperature (K) | k (L mol-1 s-1) |
---|---|
300 |
1.27×10-20 |
740 |
9.45×10-4 |
1180 |
18.4 |
1620 |
1.68×103 |
Calculate the activation energy of this reaction. ____ kJ
mol-1
Calculate the factor A in the Arrhenius equation for the
temperature dependence of the rate constant. ___ L mol-1
s-1
a) Given these data for the reaction , write the rate-law expression. (Use k for the...
The rate of the elementary reaction C2H2 + O2C2H + HO2 has been studied as a function of temperature between 300 and 2500 K. The following data were obtained for the rate constant k: Temperature (K) k (L mol-1 s-1) 300 6.25×10-45 740 1.19×10-12 1180 1.91×10-4 1620 1.07 (a) Calculate the activation energy of this reaction. kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. L mol-1 s-1
12) The rate of the elementary reaction CS2 + O2 ---> CS + SO2 has been studied as a function of temperature between 1500 and 2100 K. The following data were obtained for the rate constant k: Temperature (K) k (L mol-1 s-1) 1500 2.18×104 1620 4.82×104 1740 9.57×104 1860 1.74×105 (a) Calculate the activation energy of this reaction. ___ kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. ___...
a. Given these data for the reaction A + B → C, write the rate-law expression. Use k for the rate constant.) b. What is the value, with units, for the specific rate constant? The specific rate constant- Initial Rate of Initial [A] Initial [B] Formation of C Expt. (M) (M.s-1) 0.30 0.30 0.60 0.20 0.40 0.80 4.0 x 10-5 1.6 x 10-4 2.6 x 10-3
Given the data for the hypothetical reaction, A+B - products, determine the rate law and the value of k (without units). Initial [A] Initial [B] Rate Experiment (mol/L) (mol/L) (mol/L.s) 0.16 0.15 0.08 0.16 2 0.32 0.30 0.08 3 0.08 0.30 Please put both answers in the box below on separate lines. ... ... oo BIU Paragraph ►
QUESTION 9 Initial rate, mol/L.s Given the data below for the reaction, 2A + 2B + 4C => D + E +3 F Experiment Initial conc of A Initial conc of B. Initial conc of C, mol/L mol/L mol/L 0.1 0.1 0.2 0.3 0.3 0.4 N 0.2 2 x 10-3 4x 10-3 6 x 103 8x10-3 w A Calculate the value of k to 3 significant figures. QUESTION 7 For the reaction, 2 A(g) + 2 B(g) => C(g) +...
The Arrhenius equation for the dependence of the rate constant, k, on temperature is given by In k = + In A, where A is the frequency factor, R is the ideal gas constant, and EA is the activation energy. The rate of conversion of cyclo-propane to propene in gas phase was measured over the temperature range 750-900 K, and the rate constants that were found are reported below. Hint: think about what the following equation means In = (1,...
3. A student obtained the following data for the hydrolysis of an organic ester: Rate, k, Expt. [Esterl Ho] TK mol/Ls Vmol-s 1 0.100 0.200 288 1.04 x10 0.0521 2 0.100 0.200 298 2.02 x 10 0.101 3 0.100 0.200 308 3.68 x 10' 0.184 4 0.100 0.200 318 6.64x 10' 0.332 1 0.100 a. Prepare a plot of the rate constant as a function of temperature (attach plot); b. Prepare an Arrhenius plot, In k as a function of...
1)The rate law of a reaction is rate =k[X]³. The units of the rate constant areL mol-1 s-1mol² L-2 s-1mol L-1S-2L² mol-2 s-1mol L-1S-12)Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate =k[X]³[Y]²[Z]⁰The rate of reaction will increase by a factor of136803)What data should be plotted to show that experimental concentration data fits a first-order reaction?1 / [reactant] vs. time[reactant] vs. timeln (k) vs. Ealn (k) vs. 1 / Tln [...
The Arrhenius equation shows the relationship between the rate constant k and the temperature T in kelvins and is typically written as k=Ae−Ea/RT where R is the gas constant (8.314 J/mol⋅K), A is a constant called the frequency factor, and Ea is the activation energy for the reaction. However, a more practical form of this equation is lnk2k1=EaR(1T1−1T2) which is mathmatically equivalent to lnk1k2=EaR(1T2−1T1) where k1 and k2 are the rate constants for a single reaction at two different absolute...
The rate law for a general reaction involving reactant A is given by the equation rate = k[A]?, where rate is the rate of the reaction, k is the rate constant, [A] is the concentration of reactant A, and the exponent 2 is the order of reaction for reactant A. What is the rate constant, k, if the reaction rate at 450.°C is 1.23x10-1 mol/L.s when the concentration of A is 0.220 mol/L? 1/Mos When heated to 75°C, 1 mole...