For the following reaction, the equilibrium constant kc is 2.0 at a certain temperature. the reaction is endothermic. what do you expect to happen to the concentration of no if the temperature is doubled? 2nobr( g) ⇌ 2no( g) + br 2( g) the change in concentration of [no] will depend on the size of the vessel. the concentration of no will increase. the concentration of no will decrease. a catalyst will be needed to make a change in concentration. there will be no change in [no].

The correct answer is : 'the concatenation of NO will increase'.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

If the temperature is increased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where increase in temperature occurs.

As, this is an endothermic reaction, increasing temperature will add more heat to the system which move equilibrium in the forward reaction with decrease in temperature. Hence, the equilibrium will shift in the right direction.

So, the concatenation of NO will increase.

hcl + naoh → h2o + nacl

explanation:

hcl + naoh → h2o + nacl   is the reaction that is correctly balanced.

however, pcl3 + h2 → ph3 +3hcl, 2ca+ 3cl2 → cacl3, and c5h12 + 5o2 → 5co2 + 6h2o are not correctly balanced.