A chemical reaction was conducted at varying temperatures so that the equilibrium constant, K was determined...
A chemical reaction was conducted at varying temperatures so that the equilibrium constant, K was determined at each. Thereafter it was assumed that the reaction enthalpy, DeltarxnH° was independent of temperature and a graph of 1/T (in Kelvin) vs. ln K was plotted yielding a straight line with a slope of –1586.33. What was the resulting DeltarxnH° value and was it an exothermic reaction
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A chemical reaction was conducted at varying temperatures so
that the equilibrium constant, K was determined...
A chemical reaction was conducted at several different temperatures (measured in K) and the equilibrium constant...
A chemical reaction was conducted at several different temperatures (measured in K) and the equilibrium constant was measured at each one. Plotting the data on a graph with ln K on the y-axis and 1/T on the x-axis gives a linear plot with slope = -4594.6 and y-intercept = 13.6. What is ΔrH° (in kJ mol-1) and ΔrS° (in J mol-1 K-1)?
For a given reaction, the rate constant, k, was determined at different temperatures. To obtain a...
For a given reaction, the rate constant, k, was determined at different temperatures. To obtain a linear graph, one should plot: k vs. time ln k vs. 1/T ln k vs. ln [A] k vs. 1/T ln k vs. time ln k vs [A] 1/T vs 1/[A] [A] vs T
A series of experiments were conducted where the equilibrium constant (K) was determined at various temperatures...
A series of experiments were conducted where the equilibrium constant (K) was determined at various temperatures (T). The data was then graphed (shown below). The equation of the line is listed on the graph. Use the graph to determine AS (in J/mol·K). -30 0.0031 -30.30.003 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 -31 -31.5 y = -6861.2x - 9.2495 In (K) -32 -32.5 -33 -33.5 -34 -34.5 -35 1/T in K. Answer:
A series of experiments were conducted where the equilibrium constant (K) was determined at various temperatures...
A series of experiments were conducted where the equilibrium constant (K) was determined at various temperatures (T). The data was then graphed (shown below). The equation of the line is listed on the graph. Use the graph to determine AH° (in kJ/mol). -30 0.0031 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 -30.50.003 -31 y = -6861.2x - 9.2495 -31.5 -32 -32.5 In -33 -33.5 -34 -34.5 -35 1/T in K
The equilibrium constant K for a certain reaction was measured as a function of temperature (in...
The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 times 10^4 K and a y-intercept of -14.51. Determine the value of Delta H degree for this reaction -120.6 kJ/mol -164.7 kJ/mol -112.4 kJ/mol -176.7 kJ/mol none of the above
For the gas phase decomposition of 1-chloropropane, CH3CH2CH2ClCH3CH=CH2 + HCl the rate constant has been determined...
For the gas phase decomposition of 1-chloropropane, CH3CH2CH2ClCH3CH=CH2 + HCl the rate constant has been determined at several temperatures. When ln k in s-1 is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.77×104 K and a y-intercept of 31.0. The activation energy for the gas phase decomposition of 1-chloropropane is kJ/mol.
ln(k) = -E_a/R 1/T + ln(A) A plot of ln (k)versus 1/T result in a straight...
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...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g)...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium partial pressures of all species when CO and Cl2, each at an intitial partial pressure of 1.70 atm, are introduced into an evacuated vessel at 600 K. PCO = atm PCl2 = atm PCOCl2 = atm B. The equilibrium constant, Kc, for the following reaction is 2.90×10-2 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) Calculate Kc at this temperature for...
For the gas phase isomerization of dimethyl citraconate, cis-(CH3OOC)(CH3)C=CHCOOCH3trans-(CH3OOC)(CH3)C=CHCOOCH3 the rate constant has been determined at...
For the gas phase isomerization of dimethyl citraconate, cis-(CH3OOC)(CH3)C=CHCOOCH3trans-(CH3OOC)(CH3)C=CHCOOCH3 the rate constant has been determined at several temperatures. When ln k in s-1 is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -1.26×104 K and a y-intercept of 11.5. The activation energy for the gas phase isomerization of dimethyl citraconate is __ kJ/mol.
The equilibrium constant, K, of a certain first order reaction was measured at two temperatures, T....
The equilibrium constant, K, of
a certain first order reaction was measured at two temperatures, T.
The data is shown in this table.
The equilibrium constant, K, of a certain first If you were going to graphically determine the enthalpy, AH°, for this reaction, what points would you plot? order reaction was measured at two temperatures, T. The data is shown in this table Number Number T(K)K 3253.10 725 8.77 To avoid rounding errors, use three significant figures in the...
A series of experiments were conducted where the equilibrium constant (K) was determined at various temperatures (T). The data was then graphed (shown below). The equation of the line is listed on the graph. Use the graph to determine AS (in J/mol·K). -30 0.0031 -30.30.003 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 -31 -31.5 y = -6861.2x - 9.2495 In (K) -32 -32.5 -33 -33.5 -34 -34.5 -35 1/T in K. Answer:
A series of experiments were conducted where the equilibrium constant (K) was determined at various temperatures (T). The data was then graphed (shown below). The equation of the line is listed on the graph. Use the graph to determine AH° (in kJ/mol). -30 0.0031 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 -30.50.003 -31 y = -6861.2x - 9.2495 -31.5 -32 -32.5 In -33 -33.5 -34 -34.5 -35 1/T in K
The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 times 10^4 K and a y-intercept of -14.51. Determine the value of Delta H degree for this reaction -120.6 kJ/mol -164.7 kJ/mol -112.4 kJ/mol -176.7 kJ/mol none of the above
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...
The equilibrium constant, K, of
a certain first order reaction was measured at two temperatures, T.
The data is shown in this table.
The equilibrium constant, K, of a certain first If you were going to graphically determine the enthalpy, AH°, for this reaction, what points would you plot? order reaction was measured at two temperatures, T. The data is shown in this table Number Number T(K)K 3253.10 725 8.77 To avoid rounding errors, use three significant figures in the...
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