Answer:
C. Increase the temperature, allowing more frequent collisions of A and B with greater kinetic energy.
Explanation:
For the reaction:
A + B → 2C
You can increase the consume of A:
A. Utilize reaction conditions to convert both reactants to solids. <em>FALSE. </em>Convert both reactants in solids makes less frequent collisions doing difficult the reaction.
B. Decrease the concentration of reactant B to allow C to be produced at a greater rate. <em>FALSE. </em>The decreasing of B will make the reaction slowly.
C. Increase the temperature, allowing more frequent collisions of A and B with greater kinetic energy. <em>TRUE. </em>The increase of temperature will make more frequent collisions of A and B doing the reaction faster.
D. Increase the concentration of C to allow for more frequent collisions of A and B of higher energy
. <em>FALSE. </em>The increase of C makes less frequent collisions doing difficult the reaction.
E. Introduce a catalyst to decrease the consumption of A and B. <em>FALSE. </em>Introducing a catalyst increase the consumption of A and B.
I hope it helps!
Answer:
The letter I
Explanation:
H, I, J, K, L, M, N, O, P
Answer:
The correct answers are:
<em>c. The concentrations of the products decrease</em>
<em>d. The equilibrium constant decreases</em>
Explanation:
Changes in temperature shift the equilibrium. In this problem, the reaction is endothermic, so it absorbs heat so heat is considered as a reactant:
Reactants + heat ⇒ Products
If the temperature is decreased, the heat is decreased, so reactants are removed from the reaction at equilibrium. According to Le Chaterlier's principle, the system will try to compensate the produced change. If reactants are removed, the systems will form reactants and the equilibrium will shift toward the left (formation of more reactants). In consequence, the amount of products will be decreased.
Thus, acorrect option is: c. The concentrations of the products decrease.
Since the equilibrium constant is given by the ratio of concentration of products over concentration of reactants, if the concentration of products decrease, the equilibrium constant also decreases. So, another correct option is: d. The equilibrium constant decreases.
The balanced chemical reaction would be:
<span>2NI3 = N2 + 3I2
We use the reaction above and the molar masses of the substances involved. We start with the initial amount of NI3 reactant.
3.58 g NI3 (1 mol NI3 / 394.71 g NI3) (3 mol I2 / 2 mol NI3) = 0.0136 mol I2
Therefore, option C is the answer.</span>
