what happens at the molecular level when the following reaction occurs?
N2O4(g)>2NO2(g)
What change in entropy and enthalpy occur for this reaction?
- Both entropy and enthalpy will increase
-Entropy will increase, but enthalpy will decrease
-Entropy will decrease, but enthalpy will increase
-Both entropy and enthalpy will decrease Explain
As one molecule dissociated into two molecules and therefore, entropy increases because entropy depends on number of particles, higher the number of particle, higher will be entropy.
As it is a dissociation reaction and hence energy is needed for such reaction and thus it is an endothermic reaction and hence enthalpy is positive.
Thus, both entropy and enthalpy increases
what happens at the molecular level when the following reaction occurs? N2O4(g)>2NO2(g) What change in entropy...
Given the reaction below: N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) d) You increase [NO2][NO2], but change nothing else about the system. How will this affect the value of K? Select one: a. K will decrease. b. K will increase. c. K will not change.
Calculate the Entropy of the reaction equilibrium between 2NO2 - N2O4 given the equation: Delta G = Delta H - T Delta S where: Enthalpy = -47.5 Kj/mol Gibbs free energy = -3.59 Kj/mol Temperature = 298K
N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) c) Based on the K value calculated in 4c, which of the following is true about the reaction when it is performed at 100˚C? Select one or more: a. The reaction is nonspontaneous. b. The reaction is spontaneous.
Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.870 atm, and N2O4 at a pressure of 0.0757 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished?
Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.722 atm, and N2O4 at a pressure of 0.0521 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO2= ?? atm PN2O4= ?? atm
For the following reaction : 2NO2(g) ? N2O4(g) ?H� = -58.04 kJ/mol Try to predict what happens to the system at equilibrium if: a/ The temperature is raised? b/ The pressure of the system is increased? c/ An inert gas is added to the system at constant pressure? d/ An inert gas is added to the system at constant volume? e/ A catalyst is added to the system?
The standard enthalpy of formation, ΔHf0, for N2O4 is the enthalpy change for which reaction? a. 2NO(g) + O2(g) → N2O4(g) b. 2NO2(g) → N2O4(g) c. 2N(g) + 4O(g) → N2O4(g) d. N2(g) + 2O2(g) → N2O4(g) e. N2O(g) + O3(g) → N2O4(g)
What changes will result in a loss of color for the following reaction? N2O4(g) -> 2NO2(g) dH < 0 <- colorless brown I. Increasing temperature II. Decreasing volume III. Addition of No2.
The reaction N2O4(g) ⇌ 2NO2(g) has ∆G° = 13.3 kJ/mol at 25 °C. What is the value of ∆G, in kJ/mol, for this reaction at this temperature when [N2O4] = 3.0 M and [NO2] = 0.0010 M? Enter your answer to the tenths place. Do not include units. Include the sign if appropriate! Thank you for your help!
6) When a spontaneou s, endothermic reaction occurs at constant temperature and pressure, the entropy change of the surroundings is: a) impossible to tell b) positive c) negative d) zero a) ΔG > 0 One finds that the equilibrium constant for a particular reaction increases with increasing temperature. Assuming that the standard reaction enthalpy and entropy are temperature independent, this means that: a) The standard reaction enthalpy is less than zero 8) b) The standard reaction entropy is greater than...