Good evening. I hope you are well. My chemistry question is attached to this message as a JPG. **Phosphorus Trihydride (PH₃) Formation and Equilibrium**Phosphorus trihydride (PH₃) is a chemical compound isoelectronic with ammonia (NH₃). It serves as a precursor in synthesizing various organophosphorus compounds used as insecticides and pesticides. PH₃ can be formed by the following reaction:\[ \text{P}_4(g) + 6 \text{H}_2(g) \rightleftharpoons 4 \text{PH}_3(g) \quad (2.1) \]**a) Expression for K, the Thermodynamic Equilibrium Constant**To find the expression for the equilibrium constant \( K \) for the reaction:\[ K = \frac{[\text{PH}_3]^4}{[\text{P}_4][\text{H}_2]^6} \]**b) Calculation of Numerical Value for K**Assume \( T = 25.0^\circ C \), the temperature at which the thermodynamic data are provided:| Substance | \( \Delta H_f^\circ \) (kJ/mol) | \( \Delta G_f^\circ \) (kJ/mol) | \( S^\circ \) (J/mol·K) ||-----------|---------------------------------|---------------------------------|------------------------|| H₂(g) | 0.0 | 0.0 | 130.6 || P₄(g) | 58.9 | 24.5 | 279.9 || PH₃(g) | 5.4 | 13.4 | 210.1 |**c) Effect of Temperature Increase on Equilibrium Constant****Prompt:** If the temperature is increased to \( T = 50.0^\circ C \), will the numerical value for \( K \) increase, decrease, or stay the same? Briefly justify your answer.**Answer:** The equilibrium constant \( K \) is influenced by temperature changes according to the van 't Hoff equation. If the reaction is exothermic, increasing the temperature will decrease the value of \( K \). If it is endothermic, \( K \) will increase. In this case, you would apply the reaction enthalpies to determine whether the reaction is endothermic or exothermic, which is suggested by

According to rate law For equation rate of reaction = rate constant k x (reactant)^a rate constant…

2) Phosphorus trihydride (PH3) is a chemical compound that is isoelectronic with ammonia (NH3). It is a precursor in the synthesis of a variety of organophosphorus compounds that are used as insecticides and pesticides. PH3 can be formed by the following reaction: P.(g) + 6 H2(g) 5 4 PH:(g) (2.1) a) Give the expression for K, the thermodynamic equilibrium constant for the above reaction. b) Using the information below, find the numerical value for K for the above reaction. Assume T = 25. °C, the temperature at which the thermodynamic data are given. substance AH°; (kJ/mol) AG°: (kJ/mol) S° (J/mol·K) H2(g) P.(g) PH:(g) 0.0 58.9 5.4 0.0 130.6 279.9 24.5 13.4 210.1 c) If the temperature is increased to T = 50.0 °C, will the numerical value for K increase, decrease, or stay the same? Briefly justify your answer.

2) Phosphorus trihydride (PH3) is a chemical compound that is isoelectronic with ammonia (NH3). It is a precursor in the synthesis of a variety of organophosphorus compounds that are used as insecticides and pesticides. PH3 can be formed by the following reaction: P.(g) + 6 H2(g) 5 4 PH:(g) (2.1) a) Give the expression for K, the thermodynamic equilibrium constant for the above reaction. b) Using the information below, find the numerical value for K for the above reaction. Assume T = 25. °C, the temperature at which the thermodynamic data are given. substance AH°; (kJ/mol) AG°: (kJ/mol) S° (J/mol·K) H2(g) P.(g) PH:(g) 0.0 58.9 5.4 0.0 130.6 279.9 24.5 13.4 210.1 c) If the temperature is increased to T = 50.0 °C, will the numerical value for K increase, decrease, or stay the same? Briefly justify your answer.

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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