I can try.
Whats the question
Substitution reaction<span> (also known as single displacement </span>reaction<span> or single </span>substitution reaction) <span>is a </span>chemical change throughout that one useful cluster in an exceedingly substance<span> is replaced by another </span>useful cluster<span>.
</span>The best example<span> of a </span>substitution reaction<span> is halogenation.
</span>
Organic compounds react at a slower rate and manufacture far more complicated<span> set of </span>product<span> than inorganic compounds.</span>
The correct answer to this question is this one:
Assuming all the barium bromide dissolved (which it should), the concentration of BaBr2 in solution should be zero: it should all dissociate into Ba+2 and 2Br- ions.
Turn those grams of BaBr2 into moles of BaBr2, then divide by the volume to get the concentration.
Recognize that every formula unit of BaBr2 has one ion of Ba+2, and 2 ions of Br-1. That means that when this substance dissociates, you'll get one concentration of Ba+2 ions, and a concentration of Br- ions TWICE as large. Whatever the concentration of Ba+2 ions is that you calculate, double it for the conentration of the Br-1 ion.
Answer:
T = 154 K
Explanation:
Given data:
Number of moles of Cl₂ = 0.07 mol
Pressure = 1.18 atm
Volume = 750 mL
Temperature = ?
Solution:
The given problem will be solve by using general gas equation, which is,
PV = nRT
R = general gas constant (0.0821 atm.L/mol.K)
Now we will convert the mL to L.
Volume = 750 mL × 1 L/1000 mL
Volume = 0.75 L
Now we will put the values in formula.
T = PV/nR
T = 1.18 atm × 0.75 L / 0.07 mol ×0.0821 atm.L/mol.K
T = 0.885/0.00575 /K
T = 154 K
Answer:
The order of the reaction is 1.
Explanation:
The rate law of the reaction ;
![R=k[N_2O_5]^x](https://tex.z-dn.net/?f=R%3Dk%5BN_2O_5%5D%5Ex)
The rate of the reaction from T = 0 s to 25 s, ![[N_2O_5]=1.000 M](https://tex.z-dn.net/?f=%5BN_2O_5%5D%3D1.000%20M)
to ![[N_2O_5]=0.822 M](https://tex.z-dn.net/?f=%5BN_2O_5%5D%3D0.822%20M)
respectively.
![0.00712 M/s=k[0.822 M]^x](https://tex.z-dn.net/?f=0.00712%20M%2Fs%3Dk%5B0.822%20M%5D%5Ex)
..[1]
The rate of the reaction from T = 25 s to 50 s, to ![[N_2O_5]=0.677 M](https://tex.z-dn.net/?f=%5BN_2O_5%5D%3D0.677%20M)
respectively.
![0.00646 M/s=k[0.677 M]^x](https://tex.z-dn.net/?f=0.00646%20M%2Fs%3Dk%5B0.677%20M%5D%5Ex)
..[2]
[1] ÷ [2]
![\frac{0.00712 M/s}{0.0058 M/s}=\frac{k[0.822 M]^x}{k[0.677 M]^x}](https://tex.z-dn.net/?f=%5Cfrac%7B0.00712%20M%2Fs%7D%7B0.0058%20M%2Fs%7D%3D%5Cfrac%7Bk%5B0.822%20M%5D%5Ex%7D%7Bk%5B0.677%20M%5D%5Ex%7D)
Solving for x:
x = 1.05 ≈ 1
The rate law of the reaction ;
![R=k[N_2O_5]^1](https://tex.z-dn.net/?f=R%3Dk%5BN_2O_5%5D%5E1)
The order of the reaction is 1.
