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Andru [333]
3 years ago
6

At 293 K, methanol has a vapor pressure of 97.7 Torr and ethanol has a vapor pressure of 44.6 Torr. What would be the vapor pres

sure of a mixture of 80 g of ethanol and 97 g of methanol at 293 K?
Chemistry
1 answer:
Bad White [126]3 years ago
8 0

Answer: The vapor pressure of a mixture of 80 g of ethanol and 97 g of methanol at 293 K is 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.

p_1=x_1p_1^0 and p_2=x_2P_2^0

where, x = mole fraction in solution  

p^0 = pressure in the pure state

According to Dalton's law, the total pressure is the sum of individual pressures.

p_{total}=p_1+p_2p_{total}=x_Ap_A^0+x_BP_B^0

moles of ethanol=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{80g}{46g/mol}=1.7moles

moles of methanol= \frac{\text{Given mass}}{\text {Molar mass}}=\frac{97g}{32g/mol}=3.0moles

Total moles = moles of ethanol + moles of methanol = 1.7 +3.0 = 4.7

x_{ethanol}=\frac{1.7}{4.7}=0.36,

x_{methanol}=1-x_{ethanol}=1-0.36=0.64

p_{ethanol}^0=44.6torr

p_{methanol}^0=97.7torr

p_{total}=0.36\times 44.6+0.64\times 97.7=78.3torr

Thus the vapor pressure of a mixture of 80 g of ethanol and 97 g of methanol at 293 K is 78.3 torr.

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5 0
3 years ago
Consider the reaction, C2H4(g) + H2(g) - C2H6(8), where AH = -137 kJ. How many kilojoules are released when 3.5 mol of CH4
antiseptic1488 [7]

Answer: 480 kJ of energy is released when 3.5 mol of C_2H_4 reacts.

Explanation:

The balanced chemical reaction is:

C_2H_4(g)+H_2(g)\rightarrow C_2H_6(g)  \Delta H=-137kJ

Thus it is given that the reaction is exothermic (heat energy is released) as enthalpy change for the reaction is negative.

1 mole of C_2H_4 on reacting gives = 137 kJ of energy

Thus 3.5 moles  of C_2H_4 on reacting gives = \frac{137}{1}\times 3.5=480 kJ of energy

Thus 480 kJ of energy is released when 3.5 mol of C_2H_4 reacts.

7 0
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