please show me how you solve for the answer
eq
= 0.25 means that The Reaction is 25% Complete. Thus, at 1 bar
pressure, the Equilibrium pressure of NO2 is :
(0.25*2) = 0.5 bar.
So, the Correct option is :
please show me how you solve for the answer The graph below shows the Gibbs energy...
Consider the graph below of the Gibbs energy versus the extent of reaction, $ , for the following hypothetical reaction at 1 bar and 298 K: R(g) → P(g) X Gibbs energy 0 1 Extent of reaction, The reaction favors the reactant. At X, A,G = Mp – Mr. At X, A,G > 0. At X, Qa < KQ
please answer all or none of thses i need your help are you up
for the challenge!!!
For #10-M 3: Consider the gas phase equilibrium, 2 NO2(g)+ 40(g) N20s(g). The enthalpy change for this reaction is -170 kJ and the equilibrium constant is 2.5 at 150 °C. 10. For the above reaction, if N2(g) is added at a constant total pressure of 5 bar, (A) the equilibrium will move to the left and K will decrease the equilibrium will move...
Could you please explain and show me how to calculate this? Thank you. The reaction below was measured to have an equilibrum constant of K_p = 0.25 at a reaction temperature of 2500 K. What is the free energy change per mole of CO_2 associated with this reaction under these conditions? Answer is 29kJ CO2(g) + 1/2 O2(g) <-> CO2(g) K_p = 0.25
Please answer all, this is for physical chemistry. Thank you
T-Mobile 11:14 AM X Problem Set 2_Spring 2018.pdf 1- One gram of liquid bemzene (CH)is bumed in a bomb calorimeter. The temperature before ignition was 20826 C,and the temperature afher the combustion was 25.000 "C. This was an adiabatic calorimeter (constant volame). The heat capacity of the bomb, the water around it, and the contents of the bomb before the combustion was 10,000 JK. Calculate the ??-foe C.H.1) at 298...