The atomic radius decreases
The answer is 53.8 kJ.
Solution:There are two major steps in converting ice to liquid water. It begins with a phase change when ice melts at 0.0°C, and then a temperature change when the liquid water rises in temperature from zero to 32°C.
The amount of heat involved with the phase change melting is given by
q = (mass of water) (ΔHfus)
= (115.0 g)(334 J/g)
= 38410 J = 38.41 kJ
The amount of heat involved with temperature change is
q = mcΔT
= (115.0g)(4.184J/g°C)(32°C - 0.0°C)
= 15397.12 J = 15.39712 kJ
Summing up the two values gives the total heat required to convert ice to liquid water:
q = 38.41 kJ + 15.39712 kJ= 53.8 kJ
Hello!
The pressure of the Ideal Gas when the volume is 1,45 L and the temperature is 298 K is
1,82 atm.
To solve this problem we need to apply the
Ideal Gas Law for the initial conditions and the final ones, clearing the equation for the number of moles (n) and the ideal gas constant (R) which remain constant:

Now we match n*R for the initial conditions (1) and the final ones (2), clearing the equation for P₂

Have a nice day!