Question

A reaction has a K = 1.0 x 10^-3 at 35 ^oC and 2.5 x 10^-2 at 25 ^oC. The reaction is

		Exothermic
		Cannot tell.
		Gaseous
		Endothermic

1 points   

QUESTION 2

A particular reaction had K = 0.0800 at 25^oC. Calculate ∆G^o in kJ (or kJ/mol).

1 points   

QUESTION 3

A reaction has a DG^o of 22.3 kJ (or kJ/mol) at 25^oC. Calculate K.

1 points   

QUESTION 4

For a particular reaction, K = 0.00133 at 25^oC and K = 0.0133 at 125^oC. Calculate ∆H^o in kJ (or kJ/mol).

1 points   

QUESTION 5

If a reaction has a K = 0.100 at 500. ^oK and a ∆H^o = -25.2 kJ (or kJ/mol), what would K be at 600. ^oK. [Note: I use ^oK here to distinguish temperature from the symbol for the equilibrium constant, but that is old-fashioned.]

Answer 1

1)

Here K is increasing as temperature decreased

SO, forward reaction is favoured as temperature decreases

we are decreasing temperature here

so, according to Le Chatelier's principle,

equilibrium will move in direction which release heat

hence, forward reaction must release heat

It is exotehrmic

Answer: Exothermic

2)

T= 25.0 oC

= (25.0+273) K

= 298 K

we have below equation to be used:

deltaG = -R*T*ln Kc

= - 8.314*298* ln(8*10^-2)

= 6257.6746 J/mol

= 6.26 KJ/mol

Answer: 6.26 KJ/mol

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