The first image has a higher frequency because the wavelengths are shorter. This means that the disarmament between two crests (tops of waves) are closer together than the other waves. Hope this helps and mark brainliest if you can! Thanks!
<u>Answer:</u> The equilibrium constant for the overall reaction is ![K_1\times (K_2)^2](https://tex.z-dn.net/?f=K_1%5Ctimes%20%28K_2%29%5E2)
<u>Explanation:</u>
The given chemical equations follows:
<u>Equation 1:</u> ![4NH_3(g)+5O_2(g)\xrightarrow[]{K_1} 4NO(g)+6H_2O(g)](https://tex.z-dn.net/?f=4NH_3%28g%29%2B5O_2%28g%29%5Cxrightarrow%5B%5D%7BK_1%7D%204NO%28g%29%2B6H_2O%28g%29)
<u>Equation 2:</u>
( × 2)
The net equation follows:
![4NH_3(g)+7O_2(g)\xrightarrow[]{K} 4NO_2(g)+6H_2O(g)](https://tex.z-dn.net/?f=4NH_3%28g%29%2B7O_2%28g%29%5Cxrightarrow%5B%5D%7BK%7D%204NO_2%28g%29%2B6H_2O%28g%29)
The equilibrium constant for the net reaction will be the multiplication of two above equations.
If the equation is multiplied by a factor of '2', the equilibrium constant of the net reaction will be the square of the equilibrium constant of respective reaction.
The value of equilibrium constant for net reaction is:
![K=K_1\times (K_2)^2](https://tex.z-dn.net/?f=K%3DK_1%5Ctimes%20%28K_2%29%5E2)
Hence, the equilibrium constant for the overall reaction is ![K_1\times (K_2)^2](https://tex.z-dn.net/?f=K_1%5Ctimes%20%28K_2%29%5E2)
Answer:
![PNCl_2](https://tex.z-dn.net/?f=PNCl_2)
Explanation:
Hello!
In this case, when determining empirical formulas by knowing the by-mass percent, we first must assume the percentages as masses so we can compute the moles of each element:
![n_P=\frac{26.73g}{30.97g/mol}=0.863mol\\\\n_N=\frac{12.09g}{14.01g/mol}=0.863mol\\\\n_C_l=\frac{61.18g}{35.45g/mol}=1.726mol](https://tex.z-dn.net/?f=n_P%3D%5Cfrac%7B26.73g%7D%7B30.97g%2Fmol%7D%3D0.863mol%5C%5C%5C%5Cn_N%3D%5Cfrac%7B12.09g%7D%7B14.01g%2Fmol%7D%3D0.863mol%5C%5C%5C%5Cn_C_l%3D%5Cfrac%7B61.18g%7D%7B35.45g%2Fmol%7D%3D1.726mol)
Now, for the determination of the subscript of each element in the empirical formula, we divide the moles by the fewest moles (P or N):
![P=\frac{0.863mol}{0.863mol}=1\\\\N= \frac{0.863mol}{0.863mol}=1\\\\Cl=\frac{1.726mol}{0.863mol}2](https://tex.z-dn.net/?f=P%3D%5Cfrac%7B0.863mol%7D%7B0.863mol%7D%3D1%5C%5C%5C%5CN%3D%20%5Cfrac%7B0.863mol%7D%7B0.863mol%7D%3D1%5C%5C%5C%5CCl%3D%5Cfrac%7B1.726mol%7D%7B0.863mol%7D2)
Thus, the empirical formula is:
![PNCl_2](https://tex.z-dn.net/?f=PNCl_2)
Regards!
Answer:
a positive charge of +1
Explanation:
The charge carried by atom depends on the number of protons and electrons present. The neutrons are not charged hence they do not contribute to the net charge of the specie.
The specie mentioned in the question has six protons and five electrons. Hence it has an excess of one positive charge hence a net charge of +1.