Given:
NO (g) + O2 (g) → 2 NO2 (g) ΔΗ = -114.2 k
Calculate AH for this equation:
NO2 (g)→½NO (g) + ½O2 (g)
Given: NO (g) + O2(g) → 2 NO2 (g) AH = -114.2 kJ Calculate AH for this equation: 2 NO2(g) + NO(g) + O2 (g) Note: Your answer should be in kJ
Given: NO (g) + O2(g) +2 NO2 (g) AH = -114.2 kJ Calculate AH for this equation: 2 NO(g) + 2O2(g) →4 NO2 (g) Note: Your answer should be in kJ
(6) (1 point) Using the data below, NO(g) + NO2(g) + N203(9) NO(g) + NO2(g) + O2(g) → N205(9) 2 NO2(g) + N20 (9) 2 NO(g) + O2(g) → 2 NO2(g) N205(9) + N2O5(s) AH° = -39.8 kJ AH° = -112.5 kJ AH° = -57.2 kJ AH° = -114.2 kJ AH° = -54.1 kJ compute the heat of reaction for, N2039) + N2O5(s) + 2 N204(9). (6) (1 point) Using the data below, NO(g) + NO2(g) + N203(9) NO(g) +...
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 270.0 K is Assume that AH° and AS are independent of temperature. Submit Answer Try Another Version 3 item attempts remaining elefchces to access important values if needed for this question, Consider the reaction 2CO2(g) + 5H2(g)CH2(g) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if...
1. Consider the following thermochemical equation. NO (g) +O3 (g) → NO2 (g) + O2(g) ΔΗ--1 99 kJ a) This reaction is i. endothermic ii. exothermic b) Calculate the amount of energy (kJ) released when 8.50 g of NO (g) is reacted with an excess of ozone, O3
Given the following reactions: 1. Ν. (g) + 3 ΗΣ (g). + 2 NH3 (g) ΔΗ, 2. 2 NH3 (g) + 4 HO (g) + 2 NO, (g) + 7 H. (g) ΔΗ 3. 2 HO (g) + 2 H. (g) + O2 (g) ΔΗ3 What is the AH for N2 (g) + 202 (g) → 2 NO2 (g) in terms of ΔΗ, ΔΗ2, ΔΗ3? Ο- ΔΗ, - ΔΗ, + 2 ΔΗ3 ΟΔΗ, Η ΔΗ) + ΔΗ3 ΟΔΗ, + ΔΗ)...
Please show how to solve it. Given the thermochemical equation: 2NO2 (g)2N0(g) 02(g) ΔΗ-=114 k what is the AH for the reaction NO(g) +1½ 02(g)- NO2(g)? + -114 kJ -57 kJ +57 kJ +114 kJ
2- For the reaction 2NO(g) + O2(g)2NO2(g) H° = -114.2 kJ and S° = -146.5 J/K The equilibrium constant for this reaction at 289.0 K is ---------- . Assume that H° and S° are independent of temperature.
calculate the deltaH given that NO2 is 33.9 kJ mol^-1 For the reaction, 7. = -114.14 kJ mol 2NO(g) + O2(g) -> 2NO2(g), AH Calculate AH of gaseous nitrogen that AH of NO2(g) is 33.9 kJ mol. monoxide, given
The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.7E+2 M–2s–1. What is the rate of reaction when the initial concentrations of NO and O2 are 1.95E-2 M and 1.40E-2 M, respectively? 5.32E-6 M/s 2.50E-3 M/s 1.80E-3 M/s 0.128 M/s -2.50E-3 M/s