Consider the reversible reaction, A+B⇌C+D. If the concentration of reactant B is increased, the rate of the forward reaction would:

increase

decrease

be unaffected

Increase

Explanation:

Chemical reaction:

A + B ⇄ C + D

According to the Le- Chatelier principle,

At equilibrium state when stress is applied to the system, the system will behave in such a way to nullify the stress.

The equilibrium can be disturb,

By changing the concentration

By changing the volume

By changing the pressure

By changing the temperature

In given condition the equilibrium is disturb by increasing the concentration of reactant.

When the concentration of reactant B is increased the system will proceed in forward direction in order to regain the equilibrium. Because when reactant concentration is high it means reaction is not on equilibrium state.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.