∆g for these initial partial pressures is 10,403.31 KJ.
ΔG gets increasingly positive as a product gas's partial pressure is raised. ΔG becomes more negative as the partial pressure of a reactant gas increases.
∆g = RT ln (q/k)
In this equation: R = 8.314 J mol⁻¹ K⁻¹ or 0.008314 kJ mol⁻¹ K⁻¹
K = 325
If ΔG < 0, then K > Q, and the reaction must proceed to the right to reach equilibrium.
∴∆g = RT ln (q/k)
= 8.314 × 298 ln ( 5 / 325)
= 2477.57 ln 0.015
= 2477.57 × (-4.199)
= 10,403.31 KJ
Products are preferred over reactants at equilibrium if G° 0 and both the products and reactants are in their standard states. When reactants are preferred above products in equilibrium, however, if G° > 0, K 1. At equilibrium, neither reactants nor products are preferred if G° = 0, hence K = 1.
Therefore, ∆g for these initial partial pressures is 10,403.31 KJ.
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vector A has magnitude 12 m and direction +y
so we can say

vector B has magnitude 33 m and direction - x

Now the resultant of vector A and B is given as

now for direction of the two vectors resultant will be given as


so it is inclined at 160 degree counterclockwise from + x axis
magnitude of A and B will be


so magnitude will be 35.11 m
Answer:
2500 J
Explanation:
We can solve the problem by using the first law of thermodynamics:

where
Uf is the final internal energy of the system
Ui is the initial internal energy
Q is the heat added to the system
W is the work done by the system
In this problem, we have:
Q = +1000 J (heat that enters the system)
W = +500 J (work done by the system)
Ui = 2000 J (initial internal energy)
Using these numbers, we can re-arrange the equation to calculate the final internal energy:
