Answer:
B. The correct ratio is 3:1:1:3
Explanation:
According to this question, the following chemical equation was given:
CH3COOH + Al(OH)3 → Al(CH3COO)3 + H2O
This equation is obviously not balanced because the number of atoms of each element on both sides of the equation is not equal or the same. To balance the equation, we make use of coefficients as follows:
3CH3COOH + Al(OH)3 → Al(CH3COO)3 + 3H2O
- There are now 6 moles of C on each side
- There are now 15 moles of H on each side
- There are now 9 moles of O on each side
- There is now 1 mole of Al on each side
The correct ratio of each compound is in the order 3:1:1:3
Ep = mass x gravitational field strength (9.8N/kg) x height
Ep = 36 kg x 9.8 x 2m
Ep = 705.6 J
Since there is no weight, I would assume that this is a 100g of pure compound.
Okay so I would be changing the percentage to gram to solve for the mole.
So
40.0g C (1 mol C/12.01 g C) = 3.33 mol C
6.73g H (1 mol H/1.01 g H ) = 6.66 mol H
53.3g O (1 mol O/16.00 g O) = 3.33 mol O
With that, two of our moles is 3.33, so we consider that are our 1, as it is also the lowest. Therefore the empirical formula is CH2O
Answer:
The reaction is not at equilibrium and reaction must run in forward direction.
Explanation:
At the given interval, concentration of NO = 
Concentration of 
= 
Concentration of NOBr = 
Reaction quotient,
, for this reaction = ![\frac{[NOBr]^{2}}{[NO]^{2}[Br_{2}]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BNOBr%5D%5E%7B2%7D%7D%7B%5BNO%5D%5E%7B2%7D%5BBr_%7B2%7D%5D%7D)
species inside third bracket represents concentrations at the given interval.
So, 
So, the reaction is not at equilibrium.
As 
therefore reaction must run in forward direction to increase and make it equal to 
.
The effective speed (rms) of the oxygen gas is 293.68 m/s.
<h3>
</h3><h3>What is Root-mean-square velocity?</h3>
Root mean square velocity is the square root of the mean of squares of the velocity of individual gas molecules
![v_{rms}=\sqrt[]{\frac{3RT}{M} }](https://tex.z-dn.net/?f=v_%7Brms%7D%3D%5Csqrt%5B%5D%7B%5Cfrac%7B3RT%7D%7BM%7D%20%7D)
<em>where </em>R = universal gas constant
M = molar mass of the gas in kg/mol
T = temperature in Kelvin
According to the ideal gas law,
PV = nRT
RT = 
Substitute in the rms velocity formula,
![v_{rms} = \sqrt[]{\frac{3PV}{nM} }](https://tex.z-dn.net/?f=v_%7Brms%7D%20%3D%20%5Csqrt%5B%5D%7B%5Cfrac%7B3PV%7D%7BnM%7D%20%7D)
P = 92 kPa, V = 10 L, n = 2 moles and M = 32 x 10⁻³ kg/mol
![v_{rms} = \sqrt[]{\frac{3\times92\times10}{2\times32\times10^-^3} }](https://tex.z-dn.net/?f=v_%7Brms%7D%20%3D%20%5Csqrt%5B%5D%7B%5Cfrac%7B3%5Ctimes92%5Ctimes10%7D%7B2%5Ctimes32%5Ctimes10%5E-%5E3%7D%20%7D)
=293.68 m/s
Thus, the effective speed (rms) of O₂ gas is 293.68 m/s.
Learn more about Root-mean-square velocity:
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