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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The question is incomplete, the complete question is:
Consider the reaction:
At equilibrium, the concentrations are as follows. [NOCl] = 1.4 × 10–2 M [NO] = 1.2 × 10–3 M [Cl2] = 2.2 × 10–3 M What is the value of Keq for the reaction expressed in scientific notation?
A) 1.6 × 10–5
B) 6.2 × 10–4
C) 6.2 × 10+4
D) 1.6 × 10+5
<u>Answer:</u> The correct option is A)
<u>Explanation:</u>
The equilibrium constant is defined as the ratio of the concentration of products to the concentration of reactants raised to the power of the stoichiometric coefficient of each. It is represented by the term
For the given chemical equation:
The expression for equilibrium constant will be:
Given values:
Putting values in above expression, we get:
Hence, the correct option is A)