Answer:
There are 8Si atoms and 16 O atoms per unit cell
Explanation:
From the question we are told that:
Edge length 
Density 
Generally the equation for Volume is mathematically given by
Where
Molar mass of (SiO2) for one formula unit
Therefore
Density of Si per unit length is
Molar mass of (SiO2) for one formula unit
Therefore
There are 8Si atoms and 16 O atoms per unit cell
Answer:
The correct option is B
Explanation:
The reaction is given as
The equilibrium constant for this reaction is mathematically represented as
![K_c = \frac{[concentration \ of \ product ]}{concentration \ of \ reactant } = \frac{[fructose \ 6 -phosphate]}{[Glucose \ 6 - phosphate]}](https://tex.z-dn.net/?f=K_c%20%3D%20%5Cfrac%7B%5Bconcentration%20%5C%20of%20%20%5C%20product%20%5D%7D%7Bconcentration%20%5C%20of%20%20%5C%20reactant%20%7D%20%3D%20%5Cfrac%7B%5Bfructose%20%5C%206%20-phosphate%5D%7D%7B%5BGlucose%20%5C%206%20-%20phosphate%5D%7D)
From the question we are told that
[Glucose 6-phosphate] = 2 × [fructose 6-phosphate]
So
![K_c = \frac{[fructose \ 6 -phosphate]}{[2 (fructose \ 6 -phosphate)]} = 0.5](https://tex.z-dn.net/?f=K_c%20%20%3D%20%5Cfrac%7B%5Bfructose%20%5C%206%20-phosphate%5D%7D%7B%5B2%20%28fructose%20%5C%206%20-phosphate%29%5D%7D%20%3D%200.5)
Generally change in free energy 
is mathematically represented as
Given that T = 298 K
R = 8.315 J/mol·K
Answer:
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Explanation:
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Answer:
carbon dioxide and water
Explanation:
Example: Combustion of Methane (CH₄(g))
CH₄(g) + 2O₂(g) => CO₂(g) + 2H₂O(g)**
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Note: The combustion of any hydrocarbon produces CO₂ & H₂O. That is,
Ethane (C₂H₆) + O₂ => CO₂(g) + H₂O(g)
Propane (C₃H₈) + O₂ => CO₂(g) + H₂O(g)
Butane (C₄H₁₀) + O₂ => CO₂(g) + H₂O(g)
The issue remaining is to balance the reaction equation. For these type equation balance Carbon 1st, then Hydrogen and finish with Oxygen. Balancing in this order leaves Oxygen which can be balanced using fractions. If problem requires lowest whole number ratios of elements, simply multiply entire equation by 2 to get standard equation*
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*Standard Equation is defined as the smallest whole number ratios of elements. The 'standard equation' is significant in that it is assumed to be at STP conditions; i.e., 0⁰C (=273K) & 1.0 Atmosphere pressure.
- Ethane (C₂H₆) + 7/2O₂(g) => 2CO₂(g) + 3H₂O(g)
=> 2C₂H₆ + 7O₂(g) => 4CO₂(g) + 6H₂O(g) <= Standard Form of Rxn
- Propane (C₃H₈) + 5O₂(g) => 3CO₂(g) + 4H₂O(g) <= Standard Form of Rxn (no need to balance with the '2' multiple)
- Butane (C₄H₁₀) + 13/2O₂ => 4CO₂(g) + 5H₂O(g)
=> 2C₃H₈ + 13O₂(g) => 4CO₂(g) + 5H₂O(g) <= Standard Form of Rxn
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**Also, note that water, H₂O(g), is listed as a gas. In some cases it will be listed as a liquid, H₂O(l).
