Answer:
0.00316
Explanation:
You have to use the following equation:
You are given the pH and need to find the concentration of H+. Plug in the given components and solve.
The concentration of H is 0.00316.
According to the collision theory for chemical reactions why do most reactions rates increase g
1 answer:
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Answer 1) : According to the complete question attached in the answer,
The radial wave function which is denoted by shown with orange color crosses through zero point. Also, At the the radial nodes, which are spherical shells to some radial distance away from the nucleus there no electron are found.
Also, the radial probability distribution curve denoted as shown in blue color is observed to touch zero, and shows the place of radial node.
Therefore, the total number of nodes will include both the kinds which has radial and angular nodes which will be represented by <em>'n'</em>.
It is observed that for any atomic orbital, the total number of nodes will be n-1 .
Considering the s orbital of the hydrogen, which has zero angular momentum (l); (l=0), as it has zero angular nodes.
Hence, there will be only radial nodes, which is
(n−1 = total number of radial nodes in s orbitals)
According to the image, there are 4 radial nodes shown, so n = 5 (as n-1 = 4; therefore, n = 5)
This represents the 5s orbital.
Answer 2) The radial nodes are observed in I'm seeing radial nodes at
,
,
and
.
where represents the hydorgen bohr atomic radius = 0.0529177 nm
Explanation : It is quite easy to observe the given graph and find out the approximate values of the radial nodes, it does not requires any equation to be solved. Equation can be used to find the radial nodes if it was supplied along with the question. Although by mere speculation one can find out the answer.
Answer:
Ea=5.29 × 10⁴ J/mol
Explanation:
In going from 25 °C (298 K) to 35 °C (308 K), the rate of the reaction doubles. Since the rate of the reaction depends on the rate constant (k), this implies that the rate constant doubles. We can find the activation energy (Ea) using the two-point form of the Arrhenius equation.