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lesantik [10]
3 years ago
5

At some temperature for the equilibrium PX3(g) + X2(g) # PX5(g) the equilibrium constant is 0.74. At the same temperature the eq

uilibrium constant for PX5(9) + PX3(g) X2(g) is​
Chemistry
1 answer:
mariarad [96]3 years ago
4 0

Answer: The equilibrium constant for PX_5(g)\rightarrow PX_3(g)+X_2(g) is 1.35

Explanation:

Equilibrium constant 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 K_c  

For the given chemical reaction:

PX_3(g)+X_2(g)\rightarrow PX_5(g)

The expression for K_c is written as:

K_c=\frac{[PX_5]^1}{[PX_3]^1[X_2]^1}

0.74=\frac{[PX_5]^1}{[PX_3]^1[X_2]^1}

For the reverse chemical reaction:

PX_5(g)\rightarrow PX_3(g)+X_2(g)

The expression for K_c' is written as:

K_c'=\frac{[PX_3]^1[X_2]^1}{[PX_5]^1}

K_c'=\frac{1}{K_c}=\frac{1}{0.74}=1.35

The equilibrium constant for PX_5(g)\rightarrow PX_3(g)+X_2(g) is 1.35

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3 years ago
How many moles of H2SO4 are present in 0.500 L of a 0.150 M H2SO4 solution?
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Answer: 0.075

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An ideal gas sealed in a rigid 4.86-L cylinder, initially at pressure Pi=10.90 atm, is cooled until the pressure in the cylinder
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\Delta H=-11897J

Explanation:

Hello,

In this case, it is widely known that for isochoric processes, the change in the enthalpy is computed by:

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Whereas the change in the internal energy is computed by:

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So we compute the initial and final temperatures for one mole of the ideal gas:

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