Both A and D
Because these compunds of reactant and the compounds of the product . The reactant goint to equation
Answer:
K = 8.1 x 10⁻³
Explanation:
We are told here that these gas phase reactions are both elementary processes, thus the reactions forward and reverse are both first order:
A→B Rate(forward) = k(forward) x [A]
and for
B→A Rate(reverse) = k(reverse) x [B]
At equilibrium we know the rates of the forward and reverse reaction are equal, so
k(forward) x [A] = k(reverse) x [B] for A(g)⇌B(g)
⇒ k(forward) / k(reverse) = [B] / [A] = K
4.7 x 10⁻³ s⁻1 / 5.8 x 10⁻¹ s⁻¹ = 8.1 x 10⁻³ = K
Notice how this answer is logical : the rate of the reverse reaction is greater than the forward reaction ( a factor of approximately 120 times) , and will be expecting a number for the equilibrium constant, K, smaller than one where the reactant concentration, [A], will prevail.
It is worth to mention that this is only valid for reactions which are single, elementary processes and not true for other equilibria.
C. Single-replacement
Chlorine replaces Bromine in KBr.
B. HE DETERMINED AN ELECTRONS CHARGE
Answer:
D. The volume of the container will decrease.
Explanation:
- We apply here, the general gas law of ideal gases:
<em>PV = nRT,</em>
where, P is the pressure of the gas.
V is the volume of the container.
n is the no. of moles of the gas.
R is the general gas constant.
T is the temperature of the gas.
- We are given that P is constant.
Also, n is constant as there is no added external gases.
T is decreased as the container is cooled.
So, the volume will change as the container is nonrigid.
<em>V α T.</em>
The volume is directly proportional to the temperature,
<em>Thus, as the container is cooled, the T will decrease, and the volume of the container will decrease.</em>
