A) For balanced chemical equation: 2HgO(s) → 2Hg(l) + O₂(g).
1) Mole ratio 1: n(HgO) : n(Hg) = 2 : 2 (1 : 1).
2) Mole ratio 2: n(HgO) : n(O₂) = 2 : 1.
3) Mole ratio 3: n(Hg) : n(O₂) = 2 : 1.
B) Balanced chemical equation: 4NH₃(g) + 6NO(g) → 5N₂(g) + 6H₂O(l).
1) Mole ratio 1: n(NH₃) : n(NO) = 4 : 6 (2 : 3).
2) Mole ratio 2: n(NH₃) : n(N₂) = 4 : 5.
3) Mole ratio 3: n(NH₃) : n(H₂O) = 4 : 6 (2 : 3).
4) Mole ratio 4: n(NO) : n(N₂) = 6 : 5.
5) Mole ratio 5: n(NO) : n(H₂O) = 6 : 6 (1 :1).
6) Mole ratio 6: n(N₂) : n(H₂O) = 5 : 6.
Stored energy is described as potential energy
Always. You never know what kind of chemical you’re dealing with and how powerful it is.
Answer:
<u>structural arrangements</u>
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<h2>properties of daimond: </h2><h3>appearance: transparent</h3><h3>hardness: very hard</h3><h3>thermal conductivity :very poor</h3><h3>electric conductivity: poor</h3><h3>density:</h3>
<h3>uses: jewellery and drilling</h3>
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<h2>properties of graphite:</h2>
<h3>appearance: black shiny</h3><h3>hardness: soft ,slippery to touch</h3><h3>thermal conductivity : moderate</h3><h3>electric conductivity: good</h3><h3>density:</h3>
<h3>uses:dry cell, electric arc, pencil lead, lubricant</h3>
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<h2>How Diamond and Graphite are chemically identical?</h2>
- On heating diamond or graphite in the air, they burn completely to form carbon dioxide.
- - Equal quantities of diamond and graphite when burned, produce exactly the same amount of carbon dioxide.
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<h2>Why the physical properties of diamond and graphite are so different?</h2>
Due to the difference in the arrangement of carbon atoms in diamond and graphite
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<h2>
<em><u>hope</u></em><em><u> it</u></em><em><u> helps</u></em><em><u> you</u></em><em><u><</u></em><em><u>3</u></em></h2>
Answer:
C₂H₈N₄O₆ is the molecular formula for the compound
Explanation:
Data from the problem:
13 g of C in 100 g of compound
4.3 g of H in 100 g of compound
30.4 g of N in 100 g of compound
52.2 g of O in 100 g of compound
Firstly we determine, the mass of each in 184 g of compound, which is 1 mol
(13 g / 100 g) . 184 g = 24 g C
(4.3 g / 100 g) . 184 g = 7.91 g H ≅ 8 g H
(30.4 g / 100 g) . 184 g = 56 g N
(52.2 g / 100 g) . 184 g = 96 g O
And now, we divide the mass by the molar mass of each to determine the moles:
24 g C / 12 g/mol = 2 mol C
8g H / 1 g/mol = 8 mol H
56 g N / 14 g/mol = 4 mol N
96 g O / 16 g/mol = 6 mol O
So the molecular formula of the compound is C₂H₈N₄O₆
