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Arada [10]
3 years ago
7

calculate the enthalpy change for converting 1.00 mol of liquid water at 100 C to water vapor at 145 degree celsius for water Δ

H vaporization=40.7kj/mol and the specfic heat of water vapor is 1.84j/g-K
Chemistry
1 answer:
Svetllana [295]3 years ago
8 0

Answer:

q1 = mCpΔT

    = 18.016g × 1.84J/g.K × (418.15-373.15)

     = 1491.72 J

q2 = n×ΔH vap

     =  1mol ×44.0kJ/mol

     = 44KJ

∴ qtotal = q1+ q2

             = 1.498kJ + 44.0kJ

             = 45.498KJ

Explanation: The heat flow can be separated into steps.all that is being observed at a constant pressure,the heat flow is equal to the enthalpy.

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Explanation:

Hello.

In this case, we first need to take into account that the density of each metal A and B is computed by dividing the mass over the volume of each metal which is actually computed by substracting the volume of water from the volume of the water and the solid:

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Next, we compute the densities as shown below:

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In such a way, A is denser is B as it's volume for the same mass is smaller.

Best regards.

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Hope It helps

Have A Nice Day : )

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