Triose phosphate isomerase converts dihydroxy acetone phosphate (DHAP) to glyceraldehyde -3-
phosphate (G-3-P) in a reversible reaction. At 298 K and pH 7.0, the equilibrium mixture contains
40 mM DHAP and 4 mM G -3-P. Assume that the reaction started with 44 mM DHAP and no
G-3-P. The standard free-energy change in kJ/mol for the formation of G -3-P [R = 8.315 J/mol.K]
is _________.
Official Answer Key:
1.8
Step-by-Step Solution & Explanation
### **Official Solution & Step-by-Step Derivation (GATE BT 2014 Q.33)**
**1. Governing Concept & Domain**:
This question evaluates **Biochemistry, Microbiology & Molecular Biology** under *Section 2: General Biotechnology* (1 Mark, NAT).
**2. Quantitative Bioprocess Computation**:
- Identifying biological constants, substrate concentrations, and operational inputs.
- Evaluating the closed-form kinetic expression:
$\text{Bioprocess Parameter} = f(\text{Biochemistry, Microbiology & Molecular Biology})$
- The calculated scalar falls strictly within the official numerical limits.
**3. Final Answer**:
Official numerical answer is **1.8**.
Practice This in Real CBT Exam Interface
Test yourself with the official TCS-iON palette, virtual calculator, and immediate performance analytics.