Answer : The correct option is, (D) 3600 kJ
Explanation :
Mass of octane = 75 g
Molar mass of octane = 114.23 g/mole
Enthalpy of combustion = -5500 kJ/mol
First we have to calculate the moles of octane.
Now we have to calculate the heat released in the reaction.
As, 1 mole of octane released heat = -5500 kJ
So, 0.656 mole of octane released heat = 0.656 × (-5500 kJ)
= -3608 kJ
≈ -3600 kJ
Therefore, the heat released in the reaction is 3600 kJ
The question is incomplete, here is the complete question:
The equilibrium constant for the reaction
N₂O₄(g)⇌2NO₂ at 2°C is Kc = 2.0
If each yellow sphere represents 1 mol of N₂O₄(g) and each gray sphere 1 mol of NO₂ which of the following 1.0 L containers represents the equilibrium mixture at 2°C?
The image is attached below.
<u>Answer:</u> The system which represents the equilibrium having value of is system (b)
<u>Explanation:</u>
Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
For a general chemical reaction:
The expression for is written as:
For the given chemical equation:
The expression of for above equation follows:
.......(1)
We are given:
Volume of the container = 1.0 L
Value of = 2.0
Molarity of the substance is calculated by using the equation:
For the given images:
Number of Gray spheres = 8 moles
Number of yellow spheres = 4 moles
Putting values in expression 1, we get:
Number of Gray spheres = 4 moles
Number of yellow spheres = 8 moles
Putting values in expression 1, we get:
Number of Gray spheres = 6 moles
Number of yellow spheres = 6 moles
Putting values in expression 1, we get:
Number of Gray spheres = 2 moles
Number of yellow spheres = 8 moles
Putting values in expression 1, we get:
Hence, the system which represents the equilibrium having value of is system (b)
