<h3><u>Answer</u>;</h3>
4) size
<h3><u>Explanation</u>;</h3>
- The mineral’s physical properties are used in identifying minerals and are determined by its chemical composition and crystal structure.
- <u>Streak</u> is the color of the mineral in powdered form and since it is a more accurate illustration of the mineral’s color, its is a more reliable property of minerals than color for identification.
- <u>Hardness</u> is one of the better properties of minerals to use for identifying a mineral. Hardness is a measure of the mineral’s resistance to scratching.
- <u>Density</u> may be used to identify minerals. It is used to describe the amount of matter in a certain amount of space. Substances that have more matter packed into a given space have higher densities.
Answer:
The balanced equation is:
2 HNO3 + Mg ---> Mg(NO3)2 + H2
From the equation, we can see that we need twice the moles of HNO3 than the moles of Mg
Moles of Mg:
Molar mass of Mg = 24 g/mol
Moles = Given mass / Molar Mass
Moles of Mg = 4.47 / 24 = 0.18 moles (approx)
Hence, 2(moles of Mg) = 0.36 moles of HNO3 will be consumed
Number of moles of HNO3 after the reaction is finished is the number of unreacted moles of HNO3
Unreacted moles of HNO3 = Total Moles - Moles consumed
Unreacted moles of HNO3 = 0.64 moles (approx)
Since we approximated the value of moles of Mg, the value of remaining moles of HNO3 will also be approximate
From the given options, we can see that 0.632 moles is the closest value to our answer
Therefore, 0.632 moles will remain after the reaction
Answer: Rate law=![k[A]^1[B]^2](https://tex.z-dn.net/?f=k%5BA%5D%5E1%5BB%5D%5E2)
, order with respect to A is 1, order with respect to B is 2 and total order is 3. Rate law constant is 
Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
![Rate=k[A]^x[B]^y](https://tex.z-dn.net/?f=Rate%3Dk%5BA%5D%5Ex%5BB%5D%5Ey)
k= rate constant
x = order with respect to A
y = order with respect to A
n = x+y = Total order
a) From trial 1: ![1.2\times 10^{-2}=k[0.10]^x[0.20]^y](https://tex.z-dn.net/?f=1.2%5Ctimes%2010%5E%7B-2%7D%3Dk%5B0.10%5D%5Ex%5B0.20%5D%5Ey)
(1)
From trial 2: ![4.8\times 10^{-2}=k[0.10]^x[0.40]^y](https://tex.z-dn.net/?f=4.8%5Ctimes%2010%5E%7B-2%7D%3Dk%5B0.10%5D%5Ex%5B0.40%5D%5Ey)
(2)
Dividing 2 by 1 :![\frac{4.8\times 10^{-2}}{1.2\times 10^{-2}}=\frac{k[0.10]^x[0.40]^y}{k[0.10]^x[0.20]^y}](https://tex.z-dn.net/?f=%5Cfrac%7B4.8%5Ctimes%2010%5E%7B-2%7D%7D%7B1.2%5Ctimes%2010%5E%7B-2%7D%7D%3D%5Cfrac%7Bk%5B0.10%5D%5Ex%5B0.40%5D%5Ey%7D%7Bk%5B0.10%5D%5Ex%5B0.20%5D%5Ey%7D)
therefore y=2.
b) From trial 2: (3)
From trial 3: ![9.6\times 10^{-2}=k[0.20]^x[0.40]^y](https://tex.z-dn.net/?f=9.6%5Ctimes%2010%5E%7B-2%7D%3Dk%5B0.20%5D%5Ex%5B0.40%5D%5Ey)
(4)
Dividing 4 by 3:![\frac{9.6\times 10^{-2}}{4.8\times 10^{-2}}=\frac{k[0.20]^x[0.40]^y}{k[0.10]^x[0.40]^y}](https://tex.z-dn.net/?f=%5Cfrac%7B9.6%5Ctimes%2010%5E%7B-2%7D%7D%7B4.8%5Ctimes%2010%5E%7B-2%7D%7D%3D%5Cfrac%7Bk%5B0.20%5D%5Ex%5B0.40%5D%5Ey%7D%7Bk%5B0.10%5D%5Ex%5B0.40%5D%5Ey%7D)
, x=1
Thus rate law is ![Rate=k[A]^1[B]^2](https://tex.z-dn.net/?f=Rate%3Dk%5BA%5D%5E1%5BB%5D%5E2)
Thus order with respect to A is 1 , order with respect to B is 2 and total order is 1+2=3.
c) For calculating k:
Using trial 1: ![1.2\times 10^{-2}=k[0.10]^1[0.20]^2](https://tex.z-dn.net/?f=1.2%5Ctimes%2010%5E%7B-2%7D%3Dk%5B0.10%5D%5E1%5B0.20%5D%5E2)
.
Answer:
1. 2.510kJ
2. Q = 1.5 kJ
Explanation:
Hello there!
In this case, according to the given information for this calorimetry problem, we can proceed as follows:
1. Here, we consider the following equivalence statement for converting from calories to joules and from joules to kilojoules:
Then, we perform the conversion as follows:
2. Here, we use the general heat equation:
And we plug in the given mass, specific heat and initial and final temperature to obtain:
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