Answer:
Vanadium
Explanation:
Atomic number increases, thereby changing into an atom of Vanadium
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.
Answer:
[∝] = +472
Explanation:
Specific rotation in a solution is defined as:
[∝] = ∝ / c×l
Where:
[∝] is specific rotation, ∝ is observed rotation (In degrees), c is concentration in g/mL and l is path length (In dm).
∝: +47.2°
c: 2.0g / 50mL = 0.04g/mL
l: 25cm × (1dm /10cm) = 2.5dm
Replacing:
[∝] = +47.2° / 0.04g/mL×2.5dm = <em>+472</em>
I hope it helps!
Answer:
The total heat required is 3.4 kJ
Explanation:
Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.
There is a direct proportional relationship between heat and temperature. So, the amount of heat a body receives or transmits is determined by:
Q = c * m * ΔT
where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.
In this case you know;
- c= 4
- m= 10 g
- ΔT= Tfinal - Tinitial= 10 C - 0 C= 10 C
Replacing:
Solving:
<em>Q1= 400 J</em>
On the other hand, you must determine the heat required to convert 0 ∘ C of ice to 0 ∘ C of liquid water by:
Q2=m*heat of fusion
Q2=10 g* 300
<em>Q2= 3,000 J</em>
The total heat required is:
Q= Q1 + Q2= 400 J + 3,000 J
Q= 3,400 J= 3.4 kJ (1 kJ= 1,000 J)
<u><em>The total heat required is 3.4 kJ</em></u>
Answer:
298.15 K.
Explanation:
Room temperature is generally taken to be 25 °C (around 77 °F). 0 °C is equivalent to 273.15 K, so we add 273.15 to 25 to find that room temperature is around 298.15 K