Ask a New Question

Question

What is the equilibrium constant of the reaction 2NO2 (g) with 3.0 M and N2O4 with 2.5M
15 years ago

Answers

DrBob222
If those are equilibrium concentrations and the reaction is as below, then
2NO2 ==> N2O4

Keq = (N2O4)/(NO2)^2 = ??
Plug in the equilibrium concentrations and calculate.
15 years ago

Related Questions

What is the equilibrium constant "Kp" at 200 C for the reaction below: P4(s) + 6 Cl2(g) --><-- 4... What is the equilibrium constant for the reaction of ammonium ion with formate ion? I know that... What is the equilibrium constant for the reaction taking place at room temperature (T = 25◦C) in t... What is the equilibrium constant for a weak acid HA that dissociates 1% at an initial concentration... What is the equilibrium constant for 2A + 3B (double arrow) =4C Is it (C)^c/ (A)^a (B)^b What is the equilibrium constant for the redox reaction in question 3? Combining the two equations... What is the equilibrium constant in the following reaction [C][O2]/[CO2] [CO2]/[C][O2] [C]^... What is the equilibrium constant for H2CO3(aq)->2H+(aq)+CO3-2(aq)
Ask a New Question
Archives Contact Us Privacy Policy Terms of Use