Answer:
Net ionic equation:
H⁺(aq) + OH⁻(aq) → H₂O(l)
Explanation:
Balanced Chemical equation:
HClO₂(aq) + NaOH(aq) → H₂O(l) + NaClO₂ (aq)
Ionic equation:
H⁺(aq) + ClO₂⁻(aq) + Na⁺(aq) + OH⁻(aq) → H₂O(l) + Na⁺(aq) + ClO₂⁻ (aq)
Net ionic equation:
H⁺(aq) + OH⁻(aq) → H₂O(l)
The ClO₂⁻(aq) and Na⁺ (aq) are spectator ions that's why these are not written in net ionic equation. The water can not be splitted into ions because it is present in liquid form.
Spectator ions:
These ions are same in both side of chemical reaction. These ions are cancel out. Their presence can not effect the equilibrium of reaction that's why these ions are omitted in net ionic equation.
Answer:
option A
![{1s}^{2} {2s}^{2} {2p}^{3}](https://tex.z-dn.net/?f=%20%7B1s%7D%5E%7B2%7D%20%20%7B2s%7D%5E%7B2%7D%20%20%7B2p%7D%5E%7B3%7D%20)
Explanation:
Atomic number of Nitrogen (N) = 7
So, no. of protons and electrons = 7
Then,
![1s {}^{2} {2s}^{2} {2p}^{3}](https://tex.z-dn.net/?f=1s%20%7B%7D%5E%7B2%7D%20%20%7B2s%7D%5E%7B2%7D%20%20%7B2p%7D%5E%7B3%7D%20)
For the molarity and the percentage of the mass of kcl are mathematically given as
%m/m = 23.1%, molarity = 3.38M
<h3>What is the molarity?</h3>
Generally, the equation for the percentage of the mass of kcl is mathematically given as
(mass of kcl/mass of solution)x 100
therefore
%m/m = (6.31/27.29)x100
%m/m = 23.1%
The molarity
(no of mol/ vol of sol)
molarity = 0.0846mol/0.0250 L
molarity = 3.38M
In conclusion, the molarity is given as
molarity = 3.38M
Read more about Molarity
brainly.com/question/9149034
Answer:
![V_2=54.0ft^3](https://tex.z-dn.net/?f=V_2%3D54.0ft%5E3)
Explanation:
Hello,
In this case, we can use the Avogadro's law in order to understand the mole-volume behavior as a directly proportional relationship:
![\frac{V_1}{n_1} =\frac{V_2}{n_2}](https://tex.z-dn.net/?f=%5Cfrac%7BV_1%7D%7Bn_1%7D%20%3D%5Cfrac%7BV_2%7D%7Bn_2%7D)
Nonetheless, here we are not given neither the identity of the gas nor its molar or atomic mass, for that reason we can apply the aforementioned equation in terms of mass as we are talking about the same gas:
![\frac{V_1}{m_1} =\frac{V_2}{m_2}](https://tex.z-dn.net/?f=%5Cfrac%7BV_1%7D%7Bm_1%7D%20%3D%5Cfrac%7BV_2%7D%7Bm_2%7D)
In such a way, the new volume turns out:
![V_2=\frac{V_1m_2}{m_1} =\frac{174ft^3*13.6lbs}{43.8lbs} \\\\V_2=54.0ft^3](https://tex.z-dn.net/?f=V_2%3D%5Cfrac%7BV_1m_2%7D%7Bm_1%7D%20%3D%5Cfrac%7B174ft%5E3%2A13.6lbs%7D%7B43.8lbs%7D%20%5C%5C%5C%5CV_2%3D54.0ft%5E3)
Best regards.
Answer:
32.8g/mole
Explanation:
Given parameters:
Mass of sample of gas = 32.8g
Volume = 22.4L
Unknown:
Molecular weight = ?
Solution:
To solve this problem we must understand that at rtp;
1 mole of gas occupies a volume of 22.4L
Number of mole of the gas = 1 mole
Now;
Mass = number of moles x molecular weight
molecular weight =
=
= 32.8g/mole