For which delta h degree_rxn = -890.3 kj/mol, deltas degree_rxn = -243.0 j/mol -

Question

For which delta h degree_rxn = -890.3 kj/mol, deltas degree_rxn = -243.0 j/mol - K, and delta g degree _rxn = -817.9 kj/mol at 298.15 K Which one of the following statement is false? The equilibrium constant in tems of activities K>> 1 at 298.15 K. The equilibrium constant at any temperature can be calculated using K=wxp (-delta g degree_rxn/RT) delta g degree_rxn = -817.9 kj/mol with The reaction is exothermic. At standard state the reaction becomes non-spontaneous at an elevated temperature. It is unlikely that there is any limiting reactant found if we wait long enough What equation. encountered prior to Chapter 11, if any, is similar in form to the van't Hoff equation for chemical equilibrium? The van't Hoff equation for osmotic pressure Hess's law The Ambones equation The Rydberg equation None of the above Consider the heterogeneous inorganic reaction Fe_2N(s) + 3/2 H_2(g) e 2Fe(s) + NH_3(g), with equilibrium constant in terms of activities K = 3.852 at 700. K. Using the van't Hoff Equation for Chemical Equilibrium determine the change in standard molar enthalpy for this reaction, delta h degree _rxn (in kj/mol) if for this reaction K = 1 564 at 800 K. What is the oxidation state of carbon in sodium carbonate? -2 -1 0 +1 +4 Assign the oxidation state for each element in the following compounds CH_4 Fe_2O_3 LiOH H_2SO_4 Which one, if any, of the following statements correctly describes what happens in a hydrogen fuel cell, where the unbalanced reaction H_2(g) rightarrow H_2O(l) occurs? Both H and O are reduced.

Explanation / Answer

6) false statement is

The equilibrium constant in terms of activities K>>>1 at 298.15 K.

7 )

Arrhenius equation. K = Ae^(-Ea/RT)

8)

ln (K2/K1) = - Ho /R[1/T 2 -1/T1]

2.303 log (3.852/1.564) = -Ho/8.314 [1/700 -1/800]

Ho = -(8.314× log(2.463)×560000)/100

=18,225.95 J/mol = 18.23 kJ/mol

Go = -RT ln K

= - 8.314 ×700 × 2.303 log 3.852 = -7849.95J/mol = -7.85 kJ/mol

Go = Ho - TSo

TSo = Ho - Go

So = (Ho - Go)/T

So = (18.23 - 7.85)/700 = 0.01483 kJ/mol = 14.83 J/mol

1) +4

Na2CO3

Na = +1 , O = -2   

Let oxidation state of C = X

X + {(2×+1) - (3×-2)} = 0

X = + 4

2)CH4 : C= +4 , H= +1

Fe2O3: Fe = +2 , O = -2

LiOH : Li = +1 , O = -2 , H = +1

H2SO4 : H = +1 , S= +6 , O = -2

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