CH and O is the reactants while CO and H2O is the products
Answer:
When energy is removed in liquid water then it will solidify since heat is given off by the system to its surrounding. It is an exothermic process where the enthalpy decreases since heat is taken off. So liquid water becomes ice in an exothermic process.
Explanation:
Answer:
The enthalpy change during the reaction is -199. kJ/mol.
Explanation:
Mass of solution = m
Volume of solution = 100.0 mL
Density of solution = d = 1.00 g/mL
First we have to calculate the heat gained by the solution in coffee-cup calorimeter.
where,
m = mass of solution = 100 g
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 = 2.242 kJ
n = number of moles fructose = 
Therefore, the enthalpy change during the reaction is -199. kJ/mol.
Answer:
The reaction is spontaneous when T> 0.98 Kelvin OR T> -272.17°C
Explanation:
Step 1: Data given
ΔH = 131.3 kJ/mol = 131300 J/mol
ΔS = 133.6 J/K*mol
T = 298K
Step 2: The balanced equation
C (s) + H2O (g) --> CO (g) + H2 (g)
Step 3: ΔG
For a reaction to be spontaneous, ΔG should be <0
When ΔG > 0 the reaction is spontaneous in the reverse direction.
ΔG = ΔH - TΔS
Since ΔG<0
ΔH - TΔS <0
Step 4: Calculate T where the reaction is spontaneous
ΔH - TΔS <0
131300 J/mol - T*133.6 J/K*mol <0
- T*133.6 J/K*mol < -131300 J/mol
-T <-131300 /133.6
-T< -982.8 Kelvin
T> 982.8 Kelvin OR T> 709.6°C
The reaction is spontaneous when T> 982.8 Kelvin OR T> 709.6°C
At 298 K this reaction C (s) + H2O (g) --> CO (g) + H2 (g) is <u>not spontaneous</u>
