Answer: 78.3 torr
Explanation:
According to Raoult's law, the vapor pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the vapor pressure of that component in the pure state.
and ![p_2=x_2P_2^0](https://tex.z-dn.net/?f=p_2%3Dx_2P_2%5E0)
where, x = mole fraction
in solution
= pressure in the pure state
According to Dalton's law, the total pressure is the sum of individual pressures.
![p_{total}=p_1+p_2](https://tex.z-dn.net/?f=p_%7Btotal%7D%3Dp_1%2Bp_2)
![p_{total}=x_Ap_A^0+x_BP_B^0](https://tex.z-dn.net/?f=p_%7Btotal%7D%3Dx_Ap_A%5E0%2Bx_BP_B%5E0)
moles of ethanol= ![\frac{\text{Given mass}}{\text {Molar mass}}=\frac{80g}{46g/mol}=1.7moles](https://tex.z-dn.net/?f=%5Cfrac%7B%5Ctext%7BGiven%20mass%7D%7D%7B%5Ctext%20%7BMolar%20mass%7D%7D%3D%5Cfrac%7B80g%7D%7B46g%2Fmol%7D%3D1.7moles)
moles of methanol= ![\frac{\text{Given mass}}{\text {Molar mass}}=\frac{97g}{32g/mol}=3.0moles](https://tex.z-dn.net/?f=%5Cfrac%7B%5Ctext%7BGiven%20mass%7D%7D%7B%5Ctext%20%7BMolar%20mass%7D%7D%3D%5Cfrac%7B97g%7D%7B32g%2Fmol%7D%3D3.0moles)
Total moles = moles of ethanol + moles of methanol = 1.7 +3.0 = 4.7
,
,
![p_{ethanol}^0=44.6torr](https://tex.z-dn.net/?f=p_%7Bethanol%7D%5E0%3D44.6torr)
![p_{methanol}^0=97.7torr](https://tex.z-dn.net/?f=p_%7Bmethanol%7D%5E0%3D97.7torr)
![p_{total}=0.36\times 44.6+0.64\times 97.7=78.3torr](https://tex.z-dn.net/?f=p_%7Btotal%7D%3D0.36%5Ctimes%2044.6%2B0.64%5Ctimes%2097.7%3D78.3torr)
Thus the vapor pressure of a mixture of 80 g of ethanol and 97 g of methanol at 293 K is 78.3 torr.
Its Phosphorus with a negative 3 charge.
Number of moles = 2.12 mol C3H8.
1 mol C3H8 = 6.02 × 1023 molecules C3H8.
<span>1 molecule C3H8 = </span>11 atoms.
(3 carbon atoms<span> and 8 hydrogen atoms)</span>
Answer:
try c atom i hope this helps!! : )
Explanation: