You know two different expressions for ?G°. If a researcher
determined Keq for a reaction at several different temperatures and
then plotted lnKeq as a function of 1/T, what would the slope of
the best-fit line to the plotted data ideally be?
a) ?S°
b) ?H°/R
c) ?S°/R
d) ??S°/R
e) ??H°/R
f) ?H°
delta Go= -RT ln Keq
delta Go = delta H - T*delta S
delta H - T delta S = -RT ln Keq
ln Keq = (- delta H/ R)*1/T + delta S / R
y = mx + c
m = slope
m = -delta H/R
Answer is e ---> -delta Ho/R
You know two different expressions for ?G°. If a researcher determined Keq for a reaction at...
A student determined the value of K for the reaction 2 H2 (g) + O2 (g) → 2 H2O (g) at several different temperatures. The value for ∆S can be determined from: the slope of the curve at 25ºC from a plot of ln K versus T. the y-intercept of the line resulting from a plot of ln K versus T. the y-intercept of the line resulting from a plot of ln K versus (1/T). the slope of the line...
A student determined the value of K for the reaction 2 H2 (g) + O2 (g) → 2 H2O (g) at several different temperatures. The value for ∆S can be determined from: the slope of the curve at 25ºC from a plot of ln K versus T. the y-intercept of the line resulting from a plot of ln K versus T. the y-intercept of the line resulting from a plot of ln K versus (1/T). the slope of the line...
In a chemistry experiment that measures the kinetics of reaction at different temperatures, the activation energy of the reaction can be measured by finding the slope of the line in a ln k vs. 1/T plot. The following data are gathered from this kinetics experiment: ln k 1/T (K-1) -5.5886697 0.00339156 -4.8600624 0.00326318 -3.5719857 0.00313725 Construct a scatterplot of the ln k versus 1/T and fit a least-square regression line using the graph paper below. Compute the correlation coefficient between...
ln(k) = -E_a/R 1/T + ln(A) A plot of ln (k)versus 1/T result in a straight line with a slope = -E_a/R. The value of E_a can then be calculated using the value of R and to the slope of the line. This experiment uses the Arrhenius equation, which relates the temperature and specific reaction rate constant to determine the activation energy for the crystal violet reaction. The reaction will be performed at different temperatures. Once the order of reaction...
A student measures the reaction H2(g) + Cl2(g) <=> 2 HCl(g) concentrations at a few different temperatures and obtains the equilibrium constant. The student wants to use the van't Hoff equation to roughly determine the reaction enthalpy assuming that it does not change over the region of interest. T(K) 300 500 1000 Keq 4x1031 4x108 So the student plots the data in the Ink vs 1/T diagram and obtains a linear fitting shown below: 80 4x1018 60 In(K) 40 20...
3. The rate constant has been determined at several different temperatures. When the data is graphed as in k vs. 1/T (K-!), the slope of the line is -1.48 x 104 and the y-intercept is 24.6. What is the activation energy, E, for this reaction? a. 9.62 kJ b. 15.0 kJ c. 123 kJ d. 205 kJ e. 1214 kJ I 4. For the reaction (CH3), CBr(aq) + OH" (aq) → (CH), COH(aq) +Br"(aq) the following data were obtained at...
The rate constant for a reaction is measured as a function of time. A plot is created by graphing ln(k) on the y-axis and 1/T on the x-axis, and a best fit line with a slope of -83,871 K is obtained. Based on this data what is the activation energy of this reaction (in kJ/mol)? R= 8.314 J/(K mol)
The data in the table above were determined at 25C.
(a) Calculate G for the reaction above at 25C.
(b) Calculate Keq for the reaction above at 25C.
(c) Calculate S for the reaction above at 25C.
(d) In the table above, there are no data for H2. What are the
values of Hf, Gf, and of the absolute entropy, S, for H2 at
25C?
Using Equilibrium Constants to Determine Thermodynamic Parameters Post Lab So AHP (kJ mol (kJmol (J...
Can you please answer the question. They are the same question
but with clarification/requirements to go with it.
36. The dissolution of quartz in H2O can be represented by the following reaction: SiO2 (s) + 2H2O → H4SiO4 (aq) Rimstidt and Barnes (1980) determined the reaction rate for the dissolution of quartz as a function of temperature. Their data are listed in the following table: Temperatures and Reaction Rates for the Dissolution of Quartz T(°C) k(sec-1) 65 105 145 170...
Q4. A scientist was attempting to determine the frequency factor (A) of a reaction. From their experimental data they produced a line of best fit where In[A] = -39157(1/T) + 5.8 What was the frequency factor they determined? a. 3.92 x104 51 b. 4710 s-1 C. 5.8 s-1 d. 330 s-1 e. 10.24 5-1