The following reaction reaches equilibrium in a 2.0-L flask. Answer the questions below based upon the reaction and data given. Data is collected at 25°C.
NH4Br(s) ? NH3(g) + HBr(g)
–314.4, –45.9, –36.3 delta H^0 f, kj/mol
94.6 , , 193 , 198.59 S^0, J/mol
–203.0 , –16, , –53.5 delta G^0 f, kj/mol
( In case you cant tell, The numbers going down are (NH4Br -314.4, 94.6, -203.0) (NH3 -45.9, 193, -16) (HBr -36.3, 198.59, -53.5)
1.Is the reaction exothermic or endothermic. Explain!
2.Is there an increase in entropy or a decrease in entropy. Explain!
3.What is the at 25°C? Is this a spontaneous reaction or nonspontaneous reaction at 25°C? Explain!
4.What is the delta G^0 rxn at 400°C? Is this a spontaneous reaction or nonspontaneous reaction at 400°C? Explain!
5.What effect does an increase in temperature have on the spontaneity. Explain!
6.At what temperature does the spontaneity change? Explain!
7.What is the value of the equilibrium constant at 400°C?
NH4Br(s) ? NH3(g) + HBr(g)
–314.4, –45.9, –36.3 delta H^0 f, kj/mol
94.6 , , 193 , 198.59 S^0, J/mol
–203.0 , –16, , –53.5 delta G^0 f, kj/mol
( In case you cant tell, The numbers going down are (NH4Br -314.4, 94.6, -203.0) (NH3 -45.9, 193, -16) (HBr -36.3, 198.59, -53.5)
1.Is the reaction exothermic or endothermic. Explain!
2.Is there an increase in entropy or a decrease in entropy. Explain!
3.What is the at 25°C? Is this a spontaneous reaction or nonspontaneous reaction at 25°C? Explain!
4.What is the delta G^0 rxn at 400°C? Is this a spontaneous reaction or nonspontaneous reaction at 400°C? Explain!
5.What effect does an increase in temperature have on the spontaneity. Explain!
6.At what temperature does the spontaneity change? Explain!
7.What is the value of the equilibrium constant at 400°C?