Answer: 18 atoms
Explanation: the reactant contains 6O2 and 6O and this gives a total of 18
The answer is C ionic bonds
Answer:
the grams of H2O is 351g are processed form 9.75moles of H2
Answer:
D is the answer to this problem
Answer:
![\Delta S_{sys}=0.020kJ=20J](https://tex.z-dn.net/?f=%5CDelta%20S_%7Bsys%7D%3D0.020kJ%3D20J)
Explanation:
Hello!
In this case, given the required energy to vaporize 1.00 mol of ethanol as the enthalpy of vaporization:
![\Delta H_{vap}=\frac{38.6kJ}{1.00mol}=38.6kJ/mol](https://tex.z-dn.net/?f=%5CDelta%20H_%7Bvap%7D%3D%5Cfrac%7B38.6kJ%7D%7B1.00mol%7D%3D38.6kJ%2Fmol)
We can compute the entropy of the system for the vaporization of 8.00 g of ethanol, by first computing the moles:
![n_{et}=8.00g*\frac{1mol}{46.07g} =0.174mol](https://tex.z-dn.net/?f=n_%7Bet%7D%3D8.00g%2A%5Cfrac%7B1mol%7D%7B46.07g%7D%20%3D0.174mol)
And then setting up the following expression:
![\Delta S_{sys}=\frac{n_{et}*\Delta H_{vap}}{T}](https://tex.z-dn.net/?f=%5CDelta%20S_%7Bsys%7D%3D%5Cfrac%7Bn_%7Bet%7D%2A%5CDelta%20H_%7Bvap%7D%7D%7BT%7D)
Whereas the temperature is in kelvins; thus, we obtain:
![\Delta S_{sys}=\frac{0.174mol*38.6\frac{kJ}{mol} }{79.6+273.15K}\\\\\Delta S_{sys}=0.020kJ=20J](https://tex.z-dn.net/?f=%5CDelta%20S_%7Bsys%7D%3D%5Cfrac%7B0.174mol%2A38.6%5Cfrac%7BkJ%7D%7Bmol%7D%20%7D%7B79.6%2B273.15K%7D%5C%5C%5C%5C%5CDelta%20S_%7Bsys%7D%3D0.020kJ%3D20J)
Best regards!