the computational part isn\'t right. I\'ve asked 2 times already and every answe

Question

the computational part isn't right. I've asked 2 times already and every answer has been wrong :(

same for this one.

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ÄTP, to adenosine diphosphate, ADP, as described by ATPaq) +H which Gnn--30.5 kJ/mol at 37.0 and pH 7.0. Calculate the value of which [ATPI-5.0 mM, [ADPI 0. in a biological cell in 20 mM, and IHPo21-5.0 mM. Number k.J/ mol Is the hydrolysis of ATP spontaneous under these conditions? O yes no

Explanation / Answer

delG= delG0+ RTlnK

K= Equilibrium constant which is written as

K= [ADP] [HPO4-2]/ [ATP] = 5*5/0.2 =125*10-3M

delG= -30.5+8.314*(37+273.15)ln (125*10-3)/1000 Kj

=-30.5-5.36 =-35.86 Kj/mol

The delG suggests the process to be spontaneous.

b) for the second reaction N2(g) +3H2(g)----> 2NH3(g)

delG= delG0+ RTlnK, K is equilibrium constant

K = [NH3]2/ [N2] [H2]3 = (0.85)2/{0.15*(0.1)3}=5667

delG= -72.6+8.314*298.15*ln(5667)/1000= -72.6+2.48 =-70.12 Kj/mol

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.