The Δ?fus of platinum is 22.18 kJ⋅mol−1 , and its Δ?fus is 10.86 J⋅mol−1⋅K−1 . What is the melting point of platinum? ?=_____ ∘C
The Δ?fus of platinum is 22.18 kJ⋅mol−1 , and its Δ?fus is 10.86 J⋅mol−1⋅K−1 . What...
Consider the data in the table. Compound Melting point (°C) Δ H fus (kJ/mol) Boiling point (°C) Δ H vap (kJ/mol) HF −83.11 4.577 19.54 25.18 HCl −114.3 1.991 −84.9 17.53 HBr −86.96 2.406 −67.0 19.27 HI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ S fus and Δ S vap for HBr . Δ S fus = J / ( K ⋅ mol) Δ S v a p = J / ( K ⋅ mol)...
The following information is given for lead at latm: AH yap(1740 °C) -178 kJ/mol AH fus(328 °C) = 4.77 kJ/mol boiling point = 1740 °C melting point = 328 °C specific heat solid= 0.130 J/gºC specific heat liquid = 0.138 J/gºC What is AH in kJ for the process of freezing a 26.3 g sample of liquid lead at its normal melting point of 328 °C. The following information is given for silver at latm: AHvap(2212 °C) = 254 kJ/mol...
Using the following data, Metal | Tn (K) | Δ irus (kJ/mol) | To (K) Li 454 2.99 Na 371 2.60 | ay,ap (kJ/mol) 1615 134.7 1156 89.6 1033 77.1 95669 942 66 K 336 2.33 Rb 312 2.34 Cs 302 2.10 calculate AStus and ASvap for Li. Number Number AS 6.95 AS74.6 J- K mol J. K-1- mol fus
For a particular reaction at 172.4 °C, Δ?=−269.73 kJ/mol ΔG=−269.73 kJ/mol, and Δ?=970.33 J/(mol⋅K) Calculate ΔG for this reaction at 14.3 °C.
For a particular reaction at 157.9 °C, Δ?=−346.08 kJ/mol, and Δ?=996.11 J/(mol⋅K) . Calculate ΔG for this reaction at −46.1 °C. Δ?=
For a particular reaction at 124.8 °C, Δ?=−841.80 kJ/mol , and Δ?=646.52 J/(mol⋅K) . Calculate ΔG for this reaction at 11.9 °C.
For a process that has Δ?∘= 40 kJ/mol and Δ?∘ = 200 J/Kmol, what is the lowest temperature that the process will be spontaneous? For a process that has ΔΗ.-40 kJ/mol and AS-200 ง/Kmol, what is the lowest temperature that the process will be spontaneous? Select one: a. 200 °C b.-150 °C С. 200 K d. 350 K e. 300 K
For a particular reaction at 227.0C, Δ?=−1398.89 kJ/mol, and Δ?=300.75 J/(mol⋅K) Calculate ΔG for this reaction at −7.5 °C
The ΔHvap of a certain compound is 26.98 kJ⋅mol−1 and its ΔSvap is 53.55 J⋅mol−1⋅K−1. What is the boiling point of this compound? boiling point: ? C
HI has a normal boiling point of −36°C, and its ∆Hvap is 22.18 kJ/mol. Calculate the molar entropy of vaporization (∆Svap).