Answer:
I think it is 1115 kJ but I don't see the answer
Explanation:
Answer: i don't know
Explanation:
u gave no information on what you're asking
Answer: Heat of vaporization is 41094 Joules
Explanation:
The vapor pressure is determined by Clausius Clapeyron equation:
where,
= initial pressure at 429 K = 760 torr
= final pressure at 415 K = 515 torr
= enthalpy of vaporisation = ?
R = gas constant = 8.314 J/mole.K
= initial temperature = 429 K
= final temperature = 515 K
Now put all the given values in this formula, we get
![\log (\frac{515}{760}=\frac{\Delta H}{2.303\times 8.314J/mole.K}[\frac{1}{429K}-\frac{1}{415K}]](https://tex.z-dn.net/?f=%5Clog%20%28%5Cfrac%7B515%7D%7B760%7D%3D%5Cfrac%7B%5CDelta%20H%7D%7B2.303%5Ctimes%208.314J%2Fmole.K%7D%5B%5Cfrac%7B1%7D%7B429K%7D-%5Cfrac%7B1%7D%7B415K%7D%5D)
Thus the heat of vaporization is 41094 Joules
Electrostatic forces work on anything that is charged.
<span>Usually only protons and electrons, but also some other elementary particles.
</span>d. a proton attracting an electron
<span>1.67 x 10^-3 moles
Calculate the molar mass of C9H8O4
Carbon = 12.0107
Hydrogen = 1.00794
Oxygen = 15.999
C9H8O4 = 9 * 12.0107 + 8 * 1.00794 + 4 * 15.999 = 180.1558
Now divide the mass you have by the molar mass
0.300 g / 180.1558 g/mole = 1.665225 x 10^-3
Round to 3 significant figures
1.67 x 10^-3</span>
