Answer: Spectator ions are removed
Explanation:
You did not include the options but I can tell you the product ratio.
The product ratio is the mole ratio of the products of the reaction.
From the balanced chemical equation you have all the mole ratios:
The given equation is: 2 C6H5COOH + 15O2 --> 14 CO2 + 6H2O
The mole ratios are: 2 C6H5COOH: 15 O2: 14 CO2 : 6 H2O
The products are CO2 and H2O
Their mole ratio = 14 CO2 : 6 H2O
That can be expressed as:
14 mol CO2 7 mol CO2
----------------- = -----------------
6 mol H2O 3 mol H2O
It is also the same that:
6 mol H2O : 14 mol CO2
6 mol H2O 3 mol H2O
------------------ = -------------------
14 mol CO2 7 mol CO2
So, compare your options to the ratios show above and pick the proper ratio.
Answer:
The molecular formula of mono sodium glutamate is
Explanation:
Molar mass of sodium glutamate,M = 169 g/mol
let the molecular formula be
Percentage of carbon in the M.S.G. =35.52 %
a = 5
Percentage of Hydrogen in the M.S.G. = 4.77 %
b = 8
Percentage of oxygen in the M.S.G. =37.85 %
c = 3.99 ≈ 4
Percentage of nitrogen in the M.S.G. = 8.29 %
d = 1
Percentage of sodium in the M.S.G. =13.60 %
e = 0.99 ≈ 1
The molecular formula be :
Answer:
The pressure of N₂O₄ in the reaction vessel after the reaction is 290 mmHg
Explanation:
Nitrogen gas reacts with oxygen gas to form dinitrogen tetroxide.
N₂ (g) + 2O₂ (g) → N₂O₄ (g)
Therefore since by Avogadro's law equal volumes of all gases contain equal numbers of molecules, there fore as the gases are within the same vessel, thier partial pressure is equivalent to their concentration
from the reaction, 1 mole of N₂ react with 2 moles of O₂ to produce 1 mole of N₂O₄
Thus
1 mmHg of N₂ react with 2 mmHg of O₂ to produce 1 mmHg of N₂O₄
337 mmHg N₂ ×(1 mmHg of N₂O₄/ 1 mmHg of N₂) = 337 mmHg N₂O₄
580 mmHg O₂ ×(1 mmHg of N₂O₄/ 2 mmHg of O₂) = 290 mmHg N₂O₄
As seen from the above calculation, the limting reactant is oxygen and the partial pressure of N₂O₄ = 290 mmHg
Answer:
18.0 g of mercury (11) oxide decomposes to produce 9.0 grams of mercury
Explanation:
Mercury oxide has molar mass of 216.6 g/ mol. It gas a molecular formula of HgO.
The decomposition of mercury oxide is given by the chemical equation below:
2HgO ----> 2Hg + O₂
2 moles of HgO decomposes to produce 1 mole of Hg
2 moles of HgO has a mass of 433.2 g
433.2 g of HgO produces 216.6 g of Hg
18.0 of HgO will produce 18 × 216.6/433.2 g of Hg = 9.0 g of Hg
Therefore, 18.0 g of mercury (11) oxide decomposes to produce 9.0 grams of mercury