For each event, indicate how the concentration of each species in the chemical equation will then change to reach equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration.
2CO(g) | + | O2(g) | ↽−−⇀ | 2CO2(g) | |
increasing the concentration of CO | |||||
increasing the concentration of CO2 | |||||
decreasing the volume of the system |
For each event, indicate how the concentration of each species in the chemical equation will then...
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after reactant or product is added. Click in each box to toggle in the relative change in concentration (up = increases, down = decreases, leave the box blank for no charge). 2CO(g) + O_2(g) rlhar 2CO_2(g) a) after increasing the concentration of CO b) after increasing the concentration of CO_2
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after a decrease in pressure or volume. If there is no change in the concentration of the species, leave the box blank. CH 4 ( g ) + 2 H 2 S ( g ) − ⇀ ↽ − CS 2 ( g ) + 4 H 2 ( g ) after decreasing the pressure after decreasing the volume of the reaction vessel
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after a decrease in pressure or volume.
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after increasing the pressure. $$ \mathbf{N}_{2}(g)+3 \mathbf{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) $$
short answer please Assignment Score: 0% 01 21 - HRMIN SE Hint Check Answer Question 14 of 15 > For each event stated, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Coci (aq) + 6H,O(l) = 4C (aq) + Co(H0)2(aq) increasing the concentration of...
Consider the system at equilibrium. 2CO(g)+O2(g)<--->2CO2(g)A. How will increasing the concentration of CO shift the equilibrium? B. How will increasing the concentration of Co, shift the equilibrium? C. How will adding a catalyst shift the equilibrium?
Consider the following system at equilibrium. 2co a) How will increasing the concentration of CO shift the equilibrium? O to the right O to the left O no effect b) How will increasing the concentration of CO2 shift the equilibrium? O to the right O to the left O no effect c) How will decreasing the the volume of the container shift the equilibrium? O to the right O to the left O no effect
1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which of the following will cause an INCREASEin the equilibrium concentration of CO? a. decreasing the pressure of the system at constant temperature b. adding more O2to the system c. removing CO2from the system as it is formed d. increasing the pressure of the system at constant temperature e. adding a catalyst
Given the reaction below at equilibrium in a closed container at 500oC. How would the equilibrium be influenced by the following? SnO2(g) + 2C(s)⇌ Sn(s) + 2CO2(g) ΔH = + 360.0 K A Introducing a catalyst B Increasing the T C Decreasing the T D Increasing the P by decreasing V E Increase concentration of CO2 F Decrease concentration of SnO2(g)
. Consider the chemical system: 2NO(g) + O2(g) <---> 2NO2(g) Fill in the blanks. An increase in pressure will cause the equilibrium to shift to the ___(1)___, increasing the concentration of _____(2)____ and decreasing the concentration of _____(3)___. The reaction is endothermic. A decrease in temperature will cause the equilibrium to shift to the ____(1)_____, increasing the concentration of ___(2)____, and decreasing the concentration of ____(3)____. Removal of O2 will cause the equilibrium to shift to the____(1)_____, increasing the concentration...