Answer:
The rate equation for this reaction:
![R=k[NH_3]^0](https://tex.z-dn.net/?f=R%3Dk%5BNH_3%5D%5E0)
Explanation:
Decomposition of ammonia:

Rate law of the can be written as;
![R=k[NH_3]^x](https://tex.z-dn.net/?f=R%3Dk%5BNH_3%5D%5Ex)
1) Rate of the reaction , when ![[NH_3]=2.0\times 10^{-3} M](https://tex.z-dn.net/?f=%5BNH_3%5D%3D2.0%5Ctimes%2010%5E%7B-3%7D%20M)
..[1]
2) Rate of the reaction , when ![[NH_3]=4.0\times 10^{-3} M](https://tex.z-dn.net/?f=%5BNH_3%5D%3D4.0%5Ctimes%2010%5E%7B-3%7D%20M)
..[2]
[1] ÷ [2]
![\frac{1.5\times 10^{-6}M/s}{1.5\times 10^{-6}M/s}=\frac{k[2.0\times 10^{-3}M]^x}{k[4.0\times 10^{-3}M]^x}](https://tex.z-dn.net/?f=%5Cfrac%7B1.5%5Ctimes%2010%5E%7B-6%7DM%2Fs%7D%7B1.5%5Ctimes%2010%5E%7B-6%7DM%2Fs%7D%3D%5Cfrac%7Bk%5B2.0%5Ctimes%2010%5E%7B-3%7DM%5D%5Ex%7D%7Bk%5B4.0%5Ctimes%2010%5E%7B-3%7DM%5D%5Ex%7D)
On solving for x , we get ;
x = 0
The rate equation for this reaction:
![R=k[NH_3]^0](https://tex.z-dn.net/?f=R%3Dk%5BNH_3%5D%5E0)
Answer:
0.91 atm is the partial pressure of just hydrogen gas.
Explanation:
Vapor pressure of water , p= 0.0313 atm
Partial pressure of hydrogen gas = 
Total pressure of the water vapors and hydrogen gas = P = 715 Torr
1 atm = 715 Torr

According Dalton's law of partial pressure:



0.91 atm is the partial pressure of just hydrogen gas.
Answer:
9.9 ml of 0.200M NH₄OH(aq)
Explanation:
3NH₄OH(Iaq) + FeCl₃(aq) => NH₄Cl(aq) + Fe(OH)₃(s)
?ml of 0.200M NH₄OH(aq) reacts completely with 12ml of 0.550M FeCl₃(aq)
1 x Molarity NH₄OH x Volume Am-OH Solution(L) = 2 x Molarity FeCl₃ x Volume FeCl₃ Solution
1(0.200M)(Vol Am-OH Soln) = 3(0.550M)(0.012L)
=> Vol Am-OH Soln = 3(0.550M)(0.012L)/1(0.200M) = 0.0099 Liter = 9.9 milliliters
Answer: A 20kg Stone traveling an 10 m/s
Explanation:
The Formula for Kinetic Energy is KE = 0.5 x mv², using this equation you can then find the item with the most Kinetic Energy in Joules (J) 0.5 x 20 x 10 = 200 Joules.