KE = (1/2)mv^2
m = 10.0 kg
v = 5.00 m/a
KE = (1/2)(10.0)(5.00)^2 = (1/2)(10.0)(25.0) = 125 J
C. 125 J
The reason for this is because nonmetals, have close to fulfilling an octet and need to gain few more electrons to do this, not to lose more. Nonmetals, because of the fact they need only few more electrons to satisfy their octet they would receive or share electrons to do this.
The property that nonmetals have are that they are very electronegative, they possess a strong affinity to pull electron density closer, because they possess fewer electron shells and possess even protons this allows for this.
I think the correct answer is traits. Please brainiest me! :)
Answer:
1. MgCl2 + Zn -> Mg + ZnCl2
2. 2Al + 6H2O(g) -> 2Al(OH)3 + 3H2
3. 2Cd + O2 -> 2CdO
4. I2 + KF -> it's not going to react
5. Zn + H2SO4 -> ZnSO4 + H2
6.2KBr + Cl2 -> 2KCl + Br2
7. AgNO3 + Na -> NaNO3 + Ag
8. 2NaCl + F2 -> 2NaF + Cl2
9. AgNO3 + Mg(NO3)2 + Ag
10. Ni + H2SO4 -> NiSO4 + H2
11. Al + K2SO4
12. FeCl3 + 3Mn-> 3MnCl + Fe
13. 2Na + 2H2O -> 2NaOH + H2
14. 2K + MgBr2 -> 2KBr + Mg
15. Zn + Pb(NO3)2 -> Pb + Zn(NO3)2
16. 2AlBr3+ 3Cl2 -> 2AlCl3 + 3Br2
Answer:
![r=25M^{-1}s^{-1}[A]^2](https://tex.z-dn.net/?f=r%3D25M%5E%7B-1%7Ds%5E%7B-1%7D%5BA%5D%5E2)
Explanation:
Hello there!
In this case, according to the given information for this chemical reaction, it is possible for us to set up the following general rate law and the ratio of the initial and the final (doubled concentration) condition:
![r=k[A]^n\\\\\frac{r_1}{r_2} =\frac{k[A]_1^n}{k[A]_2^n}](https://tex.z-dn.net/?f=r%3Dk%5BA%5D%5En%5C%5C%5C%5C%5Cfrac%7Br_1%7D%7Br_2%7D%20%3D%5Cfrac%7Bk%5BA%5D_1%5En%7D%7Bk%5BA%5D_2%5En%7D)
Next, we plug in the given concentrations of A, 0.2M and 0.4 M, the rates, 1.0 M/s and 4.0 M/s and cancel out the rate constants as they are the same, in order to obtain the following:
Which means this reaction is second-order with respect to A. Finally, we calculate the rate constant by using n, [A] and r, to obtain:
![k=\frac{r}{[A]^n} =\frac{1.0M/s}{(0.2M)^2}\\\\k=25M^{-1}s^{-1}](https://tex.z-dn.net/?f=k%3D%5Cfrac%7Br%7D%7B%5BA%5D%5En%7D%20%3D%5Cfrac%7B1.0M%2Fs%7D%7B%280.2M%29%5E2%7D%5C%5C%5C%5Ck%3D25M%5E%7B-1%7Ds%5E%7B-1%7D)
Thus, the rate law turns out to be:
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