If 5.400 g of c6h6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °c, what is the final temp
2 answers:
The final temperature of the water : <u>30.506 °C</u>
<h3>Further explanation </h3>The law of conservation of energy can be applied to heat changes, i.e. the heat received / absorbed is the same as the heat released
Qin = Qout
Heat can be calculated using the formula:
Q = mc∆T
m = mass, g
∆T = temperature difference, °C / K
From reaction:
2C₆H₆ (l) + 15O₂ (g) ⟶12CO₂ (g) + 6H₂O (l) +6542 kJ, heat released by +6542 kJ to burn 2 moles of C₆H₆
If there are 5.400 g of C₆H₆ then the number of moles:
mol = mass: molar mass C₆H₆
mol = 5.4 : 78
mol C₆H₆ = 0.0692
so the heat released in combustion 0.0692 mol C₆H₆:
the heat produced from the burning is added to 5691 g of water at 21 C
So :
Q = m . c . ∆T (specific heat of water = 4,186 joules / gram ° C)
226353 = 5691 . 4.186.∆T
the difference between temperature and heat
Specific heat
relationships among temperature, heat, and thermal energy.
When heat is added to a substance
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Answer:
a) The equilibrium will shift in the right direction.
b) The new equilibrium concentrations after reestablishment of the equilibrium :
Explanation:
a) Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.
This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.
On increase in amount of reactant
If the reactant is increased, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where more product formation is taking place. As the number of moles of is increasing .So, the equilibrium will shift in the right direction.
b)
Concentration of = 0.195 M
Concentration of =
Concentration of =
On adding more to 0.370 M at equilibrium :
Initially
0.370 M
At equilibrium:
(0.370-x)M
The equilibrium constant of the reaction =
The equilibrium expression is given as:
On solving for x:
x = 0.0233 M
The new equilibrium concentrations after reestablishment of the equilibrium :