Based on the information given in the question, the cholesterol has:
a mass of 0.406 g
&
moles of 0.00105 mol
Now, Molecular Mass = Mass ÷ Moles
= 0.406g ÷ 0.00105mol
= 386.6667 g/mol
≈ 386.67 g/mol
Answer:
Explanation:
18.01528 g/mol. I googled this, but it would be 16 for O plus 2 for the 2 H's. 18 g/mol divided by 12.5g=1.44 mol of H20.
1.44mol*
molecules/mol= 8.6688*10^23.
Radioactive decay is expressed by the following formula:
![N_{t} = N_{0} e^{-lambda * t}](https://tex.z-dn.net/?f=%20N_%7Bt%7D%20%3D%20%20N_%7B0%7D%20%20e%5E%7B-lambda%20%2A%20t%7D%20%20%20)
N₀ is the initial number of undecayed atoms.
Nt is the number of undecayed atoms remaining after time t
λ is the decay constant.
The relationship between λ and the half life time t1/2 is:
λ =
![\frac{0.693}{ t_{1/2} }](https://tex.z-dn.net/?f=%20%5Cfrac%7B0.693%7D%7B%20t_%7B1%2F2%7D%20%7D%20)
= 0.693 / 5.27 = 0.1315
![y^{-1}](https://tex.z-dn.net/?f=%20y%5E%7B-1%7D%20)
Taking natural logs for both sides of the decay expression:
ln Nt = ln N₀ - λ t
ln Nt = ln 199 - (0.1315 x 20)
= 5.293 - 2.63 = 2.66
From which:
Nt = 14.29 g
Answer:
Electrical current drives nonspontaneous reactions in electrolytic cells.
Explanation:
Electrochemical cells are cells that produce electrical energy from chemical energy.
There are two types of electrochemical cells; voltaic cells and electrolytic cells.
A voltaic cell is an electrochemical cell in which electrical energy is produced from spontaneous chemical process while an electrolytic cell is an electrochemical cell where electrical energy is produced from nonspontaneous chemical processes. Current is needed to drive these nonspontaneous chemical processes in an electrolytic cell.
An increase in the number of gas molecules in the same volume container increase pressure
a decrease in container volume increases gas pressure
an increase in temperature of gas in a rigid container increases the pressure