Answer:
Explanation:
One CH4 molecules = 10 electrons ( Carbon 6e + 4Hydrogen 4e)
A mole of any substance witll have = 6.023*10^23 atom/ molecuels,
One mole of any substnce is equal is nothing but its moalr mass
Molar mass of CH4 = 16.04
It mean,
16.04 g of CH4 has = 6.023*10^23 molecules of methane
but
4.2 gram of CH4 = 6.023*10^23 * 4.2 /16.04 = 1.58*10^23 molecuels of CH4
So one molecule has =10 electrons
1.58*10^23 molecuels will have = 1.58*10^23 * 10 = 1.58*10^24
Hope this help you
Answer: Option D
Explanation:
Chemotrophs can be defined as the organism which has the ability to get energy by the oxidation of electron donors present in the nearby environments.
These molecules in the environment can be organic or inorganic.These bacteria are usually called as thiobacillus denitrificans.
These bacteria reduce the nitrate into nitrite and the energy source for these bacteria is thiosulfate(sulfur).
Physical: The chemist could try to bend it to find out how malleable it is. He could also try to pull it into wires to find out how ductile it is.
Chemical: The chemist could put the metal into contact with other substances to get an idea of how reactive it is, and he could try to burn it and find out how flammable it is.
The statement which is true about the reactivity of element with 1S²2S²2P⁶3S¹ is
it is reactive because it has to lose one electron to have a full outermost energy level.
<u><em>Explanation</em></u>
- <u><em> </em></u>Element with 1S²2S²2P⁶3S¹ electron configuration is a sodium metal.
- sodium has one electron in the outermost energy level.
- for sodium to have a full outermost energy level ( 8 electrons) it loses the 1 electron in 3S¹ to form a positively charged ion. (Na⁺)
1) mass composition
N: 30.45%
O: 69.55%
-----------
100.00%
2) molar composition
Divide each element by its atomic mass
N: 30.45 / 14.00 = 2.175 mol
O: 69.55 / 16.00 = 4.346875
4) Find the smallest molar proportion
Divide both by the smaller number
N: 2.175 / 2.175 = 1
O: 4.346875 / 2.175 = 1.999 = 2
5) Empirical formula: NO2
6) mass of the empirical formula
14.00 + 2 * 16.00 = 46.00 g
7) Find the number of moles of the gas using the equation pV = nRT
=> n = pV / RT = (775/760) atm * 0.389 l / (0.0821 atm*l /K*mol * 273.15K)
=> n = 0.01769 moles
8) Find molar mass
molar mass = mass in grams / number of moles = 1.63 g / 0.01769 mol = 92.14 g / mol
9) Find how many times the mass of the empirical formula is contained in the molar mass
92.14 / 46.00 = 2.00
10) Multiply the subscripts of the empirical formula by the number found in the previous step
=> N2O4
Answer: N2O4
