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The oxidation numbers of the atoms of the specified elements in each of the given atoms are;
1) -4
1) -42) +1
1) -42) +13) 0
1) -42) +13) 04) +4
1) -42) +13) 04) +45) -2
1) -42) +13) 04) +45) -26) +1
1) -42) +13) 04) +45) -26) +17) -2
1) -42) +13) 04) +45) -26) +17) -2Atom oxidized = C
1) -42) +13) 04) +45) -26) +17) -2Atom oxidized = CAtom reduced = O
1) C in CH4
To get the oxidation number of C;
Oxidation state of hydrogen atom is +1 and so if the oxidation state of C is x, then we have;
x + 4(+1) = 0
x + 4 = 0
x = -4
2) H in CH4
Oxidation state on Carbon atom in this case is -4. Thus;
-4 + 4x = 0
4x = 4
x = +1
3) O in O2
This is oxygen gas that exists in it's free state and as such oxidation number is 0.
4) C in CO2
Oxidation state of O here is -2. Thus;
x + 2(-2) = 0
x - 4 = 0
x = +4
5) O in CO2
Oxidation state of C is +4 here. Thus;
4 + 2x = 0
2x = -4
x = -4/2
x = -2
6) H in H2O
Oxidation state of oxygen here is -2. Thus;
2x - 2 = 0
2x = 2
x = 2/2
x = +1
7) O in H2O
Oxidation state of hydrogen here is +1. Thus;
2(1) + x = 0
x = -2
Finally, oxidation number of carbon increased, then it is the atom that was oxidized while the atom reduced is the Oxygen atom.
Read more at; brainly.com/question/22816291
Answer:
1. -4
2. +1
3. 0
4. +4
5. -2
6. +1
7. -2
reduced = H
oxidized = O
Explanation:
Know oxidation rules.
- Hope this helped! Please let me know if you would like to learn this. I could show you the rules and help you work through them.
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What is the molecular geometry if you have a double bond, a single bond and 1 lone pair around the central atom?
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Answer:
6
Explanation:
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Answer:
False
Explanation:
Magnesium is the element of second group and third period. The electronic configuration of magnesium is - 2, 8, 2 or
There are 2 valence electrons of magnesium.
Only the valence electrons are shown by dots in the Lewis structure.
As, stated above, there are only two valence electrons of magnesium, so in the Lewis structure, two dots are made around the magnesium symbol.
Given that the electronic configuration is:- .
Orbital s cannot accommodate 3 electrons and also in magnesium it has . Hence, the statement is false.
Answers
Answer:
the initial temperature of the iron sample is Ti = 90,36 °C
Explanation:
Assuming the calorimeter has no heat loss to the surroundings:
Q w + Q iron = 0
Also when the T stops changing means an equilibrium has been reached and therefore, in that moment, the temperature of the water is the same that the iron ( final temperature of water= final temperature of iron = T )
Assuming Q= m*c*( T- Tir)
mc*cc*(T-Tc)+mir*cir*(T - Tir) = 0
Tir = 20.3 °C + 300 g * 4.186 J/g°C * (20.3 C - 19 °C) / ( 51.9 g * 0.449 J/g°C )
Tir = 90.36 °C
Note :
- The specific heat capacity of water is assumed 1 cal/g°C = 4.186 J/g°C
- We assume no reaction between iron and water
Final answer:
To calculate the initial temperature of the iron sample, use the equation q = m * c * T, where q is the heat absorbed or released, m is the mass of the substance, c is the specific heat capacity, and T is the change in temperature which is 90.36 °C
Explanation:
To calculate the initial temperature of the iron sample, we can use the equation:
q = m * c * T
Where q is the heat absorbed or released, m is the mass of the substance, c is the specific heat capacity, andT is the change in temperature. In this case, we know the mass of the iron sample, the specific heat capacity of iron, and the change in temperature of the water. By rearranging the equation, we can solve for the initial temperature of the iron sample.
Thus,
Tir = 20.3 °C + 300 g * 4.186 J/g°C * (20.3 C - 19 °C) / ( 51.9 g * 0.449 J/g°C )
Tir = 90.36 °C
Learn more about Calculating initial temperature here:
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B. Diethyl ether, dichloromethane, ethyl acetate, ethanol
C. Ethyl acetate, ethanol, dichloromethane, diethyl ether
D. Ethanol, ethyl acetate, diethyl ether, dichloromethane
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Answer:
B. Diethyl ether, dichloromethane, ethyl acetate, ethanol
Explanation:
The polarity of solvents can be determined by their polarity indexes. Polarity index is defined as the measure of the ability of the solvent to interact with various polar test solutes.
Diethyl ether is the least polar with a polarity index of 2.8
Dichloromethane with a polarity index of 3.1
Ethyl acetate with a polarity index of 4.3
Ethanol is the most polar with a polarity index of 5.2
The differences in polarities of these solvents is due to their structure. Polar solvents have large dipole moments because they contain bonds between atoms with very different electronegativities, such as oxygen and hydrogen.
Because of the two non-polar methyl groups in diethyl ether, it is not as polar as dichloromethane which has two electronegative chlorine atoms attached to a carbon atom. Similarly too, because diethyl ether has two strongly electronegative oxygen atoms sharing a bond with carbon, it has a larger dipole moment than dichloromethane. Ethanol has an oxygen hydrogen bond which has the largest dipole moment, thus, it is the most polar of the given solvents.