The equilibrium position will shift in order to counterbalance the change. That means the equilibrium position will shift, lowering the pressure once more.... When the pressure on a gas reaction is increased, the equilibrium moves to the side with fewer molecules.
<em>B</em><em> </em><em>i</em><em>s</em><em> </em><em>r</em><em>i</em><em>g</em><em>h</em><em>t</em><em> </em><em>a</em><em>n</em><em>s</em><em>w</em><em>e</em><em>r</em><em> </em><em>i</em><em>t</em><em>h</em><em>i</em><em>n</em><em>k</em><em> </em><em>b</em><em>r</em><em>o</em><em>/</em><em>s</em><em>i</em><em>s</em>
The correct answer should be letter choice C) There is an equal number of each type of atom on the reactant and product side. Its C) because if its trying to conserve mass, than that means save or be equally balanced so it should be even for both sides.
Answer:
rate = [NO]²[H₂]
Explanation:
2NO + H2 ⟶N2 + H2O2 (slow)
H2O2 + H2 ⟶2H2O (fast)
From the question, we are given two equations.
In chemical kinetics; that is the study of rate reactions and changes in concentration. The rate law is obtained from the slowest reaction.
This means that our focus would be on the slow reaction. Generally the rate law is obtained from the concentrations of reactants in a reaction.
This means our rate law is;
rate = [NO]²[H₂]
Answer:
the fastest would be gas, liquid would be in the middle and solid would be the slowest
Explanation:
