the following reaction occurs in a balloon containing
N2O2 gas
N2O4(g)=2NO2(g)
will the volume of the balloon increase or decrease?
assume the pressure and temperature are constant
explain your answer using an equation
the following reaction occurs in a balloon containing N2O2 gas N2O4(g)=2NO2(g) will the volume of the...
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
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?
At a particular temperature, Kp = 0.260 for the reaction N2O4 ---> <--- 2NO2 1. A flask containing only N2O4(g) at an initial pressure of 4.20 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. 2. With no change in the amount of material in the flask, the volume of the container in question is decreased to 0.400 times the original volume. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.
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
At a particular temperatur KP=0.70, for the reaction N2O4<->2NO2 a A flask containing only N2O4 at an initial pressure of 3.7 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. PARTIAL PRESSURE OF NO2 N2O4
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.
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.
5. Would you expect the volume of gas contained in a balloon to increase or decrease if it is exposed to lower temperatures? A balloon containing 3.50 L of gas at room temperature, 20 °C, is submerged into a vat of liquid nitrogen. The temperature of liquid nitrogen is 77 K. What will be the volume of the balloon at this very cold temperature? 6. A sample of CO2 gas occupies a volume of 225 mL at 25°C. If the...
Consider the reaction: N2O4(g) ⇄ 2NO2(g) Kp = 80 In which of the following systems will the reaction proceed in a direction to use up some of the NO2 (from right to left in the above equation). Partial Pressure N2O4 Partial pressure NO2 X 0.0020 atm 0.400 atm Y 0.0040 atm 0.800 atm Z 0.0040 atm 0.300 atm A. Y and Z only B. Z only C. Y only D. X, Y, and Z E. X and Y only...