Question

Consider the following system at equilibrium where $K_c$ = 10.5 and $\Delta H^\circ$ = -18.8 kJ/mol at 350 K. $2CH_2Cl_2(g) \rightleftharpoons CH_4(g) + CCl_4(g)$ The production of $CH_4(g)$ is favored by: 1. increasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. removing $CH_2Cl_2$. False 5. adding $CCl_4$. False

Name: consider the following system at equilibrium where kc 105 and delta hcirc 188 kjmol at 350 k 2ch2cl2g rightleftharpoons ch4g ccl4g the production of ch4g is favored by 1 increasing the 90687
Uploaded: 2022-06-13T07:53:09-08:00
Duration: 3 min 57 s
Channel: Sri K
Description: consider the following system at equilibrium where kc 105 and delta hcirc 188 kjmol at 350 k 2ch2cl2g rightleftharpoons ch4g ccl4g the production of ch4g is favored by 1 increasing the 90687

          Consider the following system at equilibrium where $K_c$ = 10.5 and $\Delta H^\circ$ = -18.8 kJ/mol at 350 K.

$2CH_2Cl_2(g) \rightleftharpoons CH_4(g) + CCl_4(g)$

The production of $CH_4(g)$ is favored by:

1. increasing the temperature.
2. increasing the pressure (by changing the volume).
3. increasing the volume.
4. removing $CH_2Cl_2$. False
5. adding $CCl_4$. False

consider the following system at equilibrium where kc 105 and delta hcirc 188 kjmol at 350 k 2ch2cl2g rightleftharpoons ch4g ccl4g the production of ch4g is favored by 1 increasing the 90687

Added by Alexandria J.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

06/13/2022

Step 1

$\Delta H^\circ = -18.8$ kJ/mol, which means the reaction is exothermic. Show more…

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Consider the following system at equilibrium where $K_c$ = 10.5 and $\Delta H^\circ$ = -18.8 kJ/mol at 350 K. $2CH_2Cl_2(g) \rightleftharpoons CH_4(g) + CCl_4(g)$ The production of $CH_4(g)$ is favored by: 1. increasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. removing $CH_2Cl_2$. False 5. adding $CCl_4$. False