Answer:
K= 1.25*10⁻⁵ (any of the options) , but if the problem's statement is wrong and D → C, K₂ = [C]/[D] = 2*10³ then K= 8*10¹⁴ (option F)
Explanation:
for
2 A + 3 D → 3 C + 2 B
K= [C]³*[B]² /([A]²*[D]³) = ([B]/[A])²* ([C][/D])³
where
2 A → 2 B , K₁ = [B]²/[A]² = ([B]/[A])² =1*10⁵
and
C → D, K₂ = [D]/[C] = 2*10³
therefore
K=K₁* (1/K₂)³=K₁/K₂³ = 1*10⁵ / (2*10³)³ = 1.25*10⁻⁵
K= 1.25*10⁻⁵
but if the problem's statement is wrong and
D → C, K₂ = [C]/[D] = 2*10³
then
K=K₁*K₂³=K₁*K₂³ = 1*10⁵ * (2*10³)³ =8*10¹⁴
K= 8*10¹⁴
Its structure is Au with one dot on top
The differential change in entropy of a system is
given as: <span>
<span>dS = (∂S/∂T)_V dT </span>
We also know that </span>
<span>(∂S/∂T)_V = n*Cv/T, </span>
Where Cv is the molar heat capacity at constant
volume, and n is the number of moles. Combining the 2 equations:<span>
dS = n*Cv/T dT
Since Cv is constant as stated in the problem, therefore we
integrate the differential equation. Leading us to:
ΔS = n*Cv*ln(Tfinal/Tinitial)
<span>We are given that: V =
18L volume at P=2 kPa and T=298.15K. </span></span>
Using the ideal gas law to find the number of
moles of gas: <span>
n = p*V/R*T = (2kPa)*(18L)/((298.15K)*(8.314 L*kPa/(mol*K)))
n = 1.45*10^-2 mol
Going back to the entropy change:
ΔS = (1.45*10^-2 mol)*(20.17 J/(K*mol))*ln(1073.15/298.15)
<span>
<span>ΔS = 0.375 J/K</span></span></span>
Most substances in the food we eat need further digestion and must travel into the intestine before being absorbed. ... Chyme is then squirted down into the small intestine, where digestion of food continues so the body can absorb the nutrients into the bloodstream.
Hopes this helps:)
