Posted by **Sarah** on Monday, February 4, 2013 at 6:29pm.

What is the value of q when 8.21g of water vaporizes at 373 K? The enthalpy of condensation of water at 373 K is -40.7 kJ/mol.

I tried using the equation q= m x Cs x Delta T, but I never got the right answer which is 18.5 kJ apparently, so I need to find out what I did wrong.

## Answer This Question

## Related Questions

- chemistry - The heat of vaporization of liquid water at 373 K is 40.7 kJ/mol. ...
- chemistry thermodynamics - calculate the w, q, delta H, and delta U for the ...
- Chemistry - Calculate the entropy change accompanying conversion of 1 mole of ...
- physics - 18g of liquid water is placed in a flexible bag, the air is excluded, ...
- Physical Chemistry - Calculate the difference between H and U ...
- Chemistry - H2O(l) = H2O(g) deltaHvap = + 40.7kJ shows the change in enthalpy ...
- chemistry - A sample of 1.00 mol H2O(g) is condensed isothermally and reversibly...
- chemistry - When 0.373 g of compound X is burned completely in a bomb ...
- Chemistry - Are my answers correct? C6H14 + 19/2 O2 -> 6 CO2 + 7H2O enthalpy ...
- chemistry - for the vaporization of water at 1.00 atm, delta H=43.54 kj/mol at ...

More Related Questions