The empirical formula of a compound is determined to be CH2O, and its molecular mass is found to be 90.087 g/mol. Determine the molecular formula of the compound, showing your solution.
Answer: This is actually quite simple, first we have to calculate the molar mass of empirical unit. Therefore we have 12+2*1+16 = 30. Then we solve 90/30 = 3. Finally we end up with 3*(CH2O) --> C3H6O3.
I hope it helps, Regards.
Answer:
1116 g.
Explanation:
The balanced equation for the reaction is given below:
4Na + O₂ —> 2Na₂O
From the balanced equation above,
1 mole of O₂ reacted to produce 2 moles of Na₂O.
Next, we shall determine the theoretical yield of Na₂O. This can be obtained as follow:
From the balanced equation above,
1 mole of O₂ reacted to produce 2 moles of Na₂O.
Therefore, 9 moles of O₂ will react to produce = 9 × 2 = 18 moles of Na₂O.
Finally, we shall determine the mass in 18 moles of Na₂O. This can be obtained as follow:
Mole of Na₂O = 18 moles
Molar mass of Na₂O = (23×2) + 16
= 46 + 16
= 62 g/mol
Mass of Na₂O =?
Mass = mole × molar mass
Mass of Na₂O = 18 × 62
Mass of Na₂O = 1116 g
Thus, the theoretical yield of Na₂O is 1116 g.
Answer:
1.20atm
Explanation:
Given parameters:
Partial pressure of gas 1 = 0.35atm
Partial pressure of gas 2 = 0.20atm
Partial pressure of gas 3 = 0.65atm
Unknown:
Total pressure of the gas mixture = ?
Solution:
To solve this problem, we need to recall and understand the Dalton's law of partial pressure.
Dalton's law of partial pressure states that "the total pressure of a mixture of gases is equal to the sum of the partial pressure of the constituent gases".
Total pressure =Pressure of gas(1 + 2 + 3)
The partial pressure is the pressure a gas would exert if it alone occupied the volume of the gas mixture.
Now we substitute;
Total pressure = (0.35 + 0.20 + 0.65)atm = 1.20atm
There are 1,000m is 1k. So just move the decimal one position right. 127.56m
There are 10,000cm in 1k. Move the decimal two positions right. 1275.6cm
Answer:
The percentage deviation is 
%
Explanation:
From the question we are told that
The concentration is of the solution is 
The true absorbance A = 0.7526
The percentage of transmittance due to stray light 
% 
Generally Absorbance is mathematically represented as
Where T is the percentage of true transmittance
Substituting value
%
The Apparent absorbance is mathematically represented
Substituting values
= 0.7385
The percentage by which apparent absorbance deviates from known absorbance is mathematically evaluated as
%
Since Absorbance varies directly with concentration the percentage deviation of the apparent concentration from know concentration is
%
