Question

In: Chemistry

The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored...

The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ∘C we have the following values for the standard state enthalpy and free energy changes of the reaction: ΔH∘=+109.6kJ/mol ΔG∘=−30.5kJ/mol

Solutions

Expert Solution

we know G = H - T S

from above   G   =−30.5kJ/mol H = 109.6kJ/mol T = 25 + 273 K = 298 K   S = ?

−30.5kJ/mol =  109.6kJ/mol -  298 K   S

−30.5kJ/mol - 109.6kJ/mol =   -  298 K   S

140.1 kJ/mol = 298 K   S

S = 0.4701   kJ/mol k

in above raction as H =+ve it means that the value of    - T S must be greater than H so that

0 > H  - T S

and      G = - ve so that the reaction must be spontaneous or thermodynamically favored .

queen_honey_blossom answered 1 year ago
Next > < Previous

Related Solutions

The decomposition of N2O5(g) —> NO2(g) + NO3(g) proceeds as a first order reaction with a...
The decomposition of N2O5(g) —> NO2(g) + NO3(g) proceeds as a first order reaction with a half life 30.0s at a certain temperature. If the initial concentration [N2O5]0 = 0.400 M, what is the concentration after 120 seconds? A)0.050 B)0.200 C)0.025 D)0.100
The rate constant for the 1st order decomposition of N2O5 in the reaction 2N2O5 (g) ...
The rate constant for the 1st order decomposition of N2O5 in the reaction 2N2O5 (g)  4NO2 (g) + O2 (g) is k=3.38x 10-5 s-1 at 25oC. a. What is the half-life of N2O5? b. What will be the total pressure, initially 88.3 kPa for the pure N2O5 vapor, (1) 10s and (2) 10 min after initiation of the reaction? (Hint: partial pressure is proportional to concentration).
The decomposition of n2o5 is a first order reaction. N2o5 decomposes to yield no2 and o2....
The decomposition of n2o5 is a first order reaction. N2o5 decomposes to yield no2 and o2. At 48deg C the rate constant for the reaction is 1.2x10^-5s^-1. Calculate the partial pressure of no2 produced from 1.0L of 0.700M n2o5 solution at 48deg C over a period of 22 hours if the gas is collected in a 10.0L container. Show work please.
The following reaction is first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at...
The following reaction is first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. A. Calculate the rate of the reaction when [N2O5]= 5.9×10−2 M. B. What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.) C. What would the rate of the reaction be at the same...
The following reaction is first order in N2O5: N2O5(g)?NO3(g)+NO2(g) The rate constant for the reaction at...
The following reaction is first order in N2O5: N2O5(g)?NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. A) Calculate the rate of the reaction when [N2O5]= 5.4
The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If...
The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If the rate constant is 4.50 × 10−4 s−1, what is the half-life of this reaction? × 10 s in scientific notation The reaction 2A → B is second order with a rate constant of 51.0/M·min at 24°C. (a) Starting with [A]0 = 9.30 × 10−3 M, how long will it take for [A]t = 2.90 × 10−3 M? min (b) Calculate the half-life of...
A proposed mechanism for the reaction N2O5-->2NO2 +1/2O2 N2O5 k1--> NO2+NO3 <---k_1-- NO2 +NO3 --k2--> NO...
A proposed mechanism for the reaction N2O5-->2NO2 +1/2O2 N2O5 k1--> NO2+NO3 <---k_1-- NO2 +NO3 --k2--> NO +O2 +NO2 NO +NO3 - k3-->2NO2 Applying the steady-state approximation to show that the overall reaction rate is -d[N2 O5 ]/dt=k[N2 O5 ] In this process you should evaluate K in terms of K1, K_1, K2 and K3
the first order rate constant for the decomposition of N2O5, 2N2O5(g)->4NO2(g)+O2(g) at 70C is 6.82x10^-3 s^-1....
the first order rate constant for the decomposition of N2O5, 2N2O5(g)->4NO2(g)+O2(g) at 70C is 6.82x10^-3 s^-1. suppose we start with 3.00x10^-2 mol of N2O5(g) in a volume of 2.3L A) how many moles of N2O5 will remain after 3.0 min? B) how many minutes will it take for the quantity of N2O5 to drop to 1.7x10^-2 mol? C) what is the half-life of N2O5 at 70C?
The tabulated data show the concentrations of N2O5 versus time for this reaction: N2O5 (g) -->...
The tabulated data show the concentrations of N2O5 versus time for this reaction: N2O5 (g) --> NO3 (g) + NO2 (g). Time(s) [N2O5] (M) 0 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210 1a. Determine the order of the reaction by graphing: Zero Order: Time vs [N2O5] First Order: Time vs ln[N2O5] Second Order: Time vs 1/[N2O5] 1b. Determine the rate constant 1c. Predict the concentration of N2O5 at 250 seconds.
The tabulated data show the concentrations of N2O5 versus time for this reaction: N2O5 (g) -->...
The tabulated data show the concentrations of N2O5 versus time for this reaction: N2O5 (g) --> NO3 (g) + NO2 (g). Time(s) [N2O5] (M) 0 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210 1a. Determine the order of the reaction by graphing: Zero Order: Time vs [N2O5] First Order: Time vs ln[N2O5] Second Order: Time vs 1/[N2O5] 1b. Determine the rate constant 1c. Predict the concentration of N2O5 at 250 seconds.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT