Condensation is the change of water from its gaseous form (water vapor) into liquid water. Condensation generally occurs in the atmosphere when warm air rises, cools and looses its capacity to hold water vapor. As a result, excess water vapor condenses to form cloud droplets.
Answer:
Ionization energy is a measure of the difficulty involved in removing an electron from an atom or ion or the tendency of an atom or ion to surrender an electron.
Explanation:
Answer:
<h2>0.06 % </h2>
Explanation:
The percentage error of a certain measurement can be found by using the formula

From the question
error = 500 - 499.7 = 0.3
actual volume = 500 mL
We have

We have the final answer as
<h3>0.06 % </h3>
Hope this helps you
Answer:
C
Explanation: a is incorrect since the lower the ph = more acidic and b is incorrect because it produces hydronium ion and d I’m not sure what it is but I no that base recieve the protons
Answer : The internal energy change is -2805.8 kJ/mol
Explanation :
First we have to calculate the heat gained by the calorimeter.

where,
q = heat gained = ?
c = specific heat = 
= final temperature = 
= initial temperature = 
Now put all the given values in the above formula, we get:


Now we have to calculate the enthalpy change during the reaction.

where,
= enthalpy change = ?
q = heat gained = 23.4 kJ
n = number of moles fructose = 

Therefore, the enthalpy change during the reaction is -2805.8 kJ/mole
Now we have to calculate the internal energy change for the combustion of 1.501 g of fructose.
Formula used :

or,

where,
= change in enthalpy = 
= change in internal energy = ?
= change in moles = 0 (from the reaction)
R = gas constant = 8.314 J/mol.K
T = temperature = 
Now put all the given values in the above formula, we get:




Therefore, the internal energy change is -2805.8 kJ/mol