For the reaction N2O3(g) → NO(g) + NO2(g) ΔG° = -4.78 J/mol. Calculate K at 25°C.
A. 1.023
B. 1.002
C. 1.010
D. 0.9484
For the reaction N2O3(g) → NO(g) + NO2(g) ΔG° = -4.78 J/mol. Calculate K at 25°C....
For the reaction N2O3(g) NO(g)+NO2(g) Delta G^ =-4.78 J/mol . Calculate K at 25°C
For the reaction: N2O3(g) → NO(g) + NO2(g) at 298 K AG° = -4.78 kJ/mol RXN. Compute K for this reaction. a) 1.01 Ob) 0.998 O c) 0.948 O d) 6.89 Oe) 10.23
For a particular reaction at 205.1205.1 °C, ΔG=−45.90 kJ/molΔG=−45.90 kJ/mol, and ΔS=395.61 J/(mol⋅K)ΔS=395.61 J/(mol⋅K). Calculate ΔG for this reaction at −6.1−6.1 °C.
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 the dimerization of nitrogen dioxide, ΔG° = −4.7 kJ at 25°C. 2 NO2(g) ⟶ N2O4(g) Calculate ΔG for this reaction if the partial pressures of NO2 and N2O4 are both 0.38 atm. (R = 8.31 × 10−3 kJ/K) a. -10.86 kJ b. -11.36 kJ c. -15.12 kJ d. -11.07 kJ e. -7.10 kJ
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 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 227.0C, Δ?=−1398.89 kJ/mol, and Δ?=300.75 J/(mol⋅K) Calculate ΔG for this reaction at −7.5 °C
Calculate ΔG at 25°C for the following reaction: CO(g) + 2H2(g) → CH3OH(l) ΔG°rxn = -2.9x104 J/mol when the carbon monoxide has an initial pressure of 5.0 atm and hydrogen gas of 3.0 atm.
Calculate ΔG°(in kJ/mol) for the reaction NO2(g) + H2O(l) --> HNO3(l) + NO(g). ( unbalanced) Substance ΔGfo(kJ/mol) NO2(g) 51.8 NO(g) 86.7 HNO3(l) -79.9 H2O(l) -237.2 Write answer to two significant figures and correct sign.