5.55

Moderators: Chem_Mod, Chem_Admin

Ellis Song 4I
Posts: 102
Joined: Thu Jul 11, 2019 12:17 am

5.55

Postby Ellis Song 4I » Thu Feb 27, 2020 11:31 pm

A reaction used in the production of gaseous fuels from coal, which is mainly carbon, is C(s) 1 H2O(g) Δ CO(g) 1 H2(g).
(a) Evaluate K At 900 K, given that the standard Gibbs free energies of formation of CO(g) and H2O(g) at 900 K are 2191.28 kJ/mol and 2198.08 kJmol, respectively. (b) A sample of graphite of mass 5.20 kg and 125 g of water were placed into a 10.0-L container and heated to 900 K. What are the equilibrium concentrations?

Are we supposed to use an ICE table in part b of this problem?

Ronak Naik
Posts: 103
Joined: Sat Jul 20, 2019 12:15 am

Re: 5.55

Postby Ronak Naik » Fri Feb 28, 2020 1:59 am

Yes an ICE table is needed in part b. Once you find the moles of each substance using the given moles, use an ice table to find equilibrium concentrations.

Gurmukhi Bevli 4G
Posts: 49
Joined: Wed Nov 14, 2018 12:20 am

Re: 5.55

Postby Gurmukhi Bevli 4G » Fri Feb 28, 2020 2:46 pm

You would need to use an ICE table for part b, to find the eventual equilibrium concentrations of the substances involved.

BCaballero_4F
Posts: 94
Joined: Wed Nov 14, 2018 12:22 am

Re: 5.55

Postby BCaballero_4F » Mon Mar 02, 2020 10:31 pm

Yes you would in order to find the equilibrium concentrations


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 2 guests