Given the following data,
2 O3(g) ----> 3
O2(g) ∆rH
= -377.00 kJ mol-1
O2(g) ----> 2
O(g) ∆rH
= 545.00 kJ mol-1
NO(g) + O3(g) ----> NO2(g) +
O2(g) ∆rH
= -124.00 kJ mol-1
Determine ∆rH for the reaction,
NO(g) + O(g) ----> NO2(g) ∆rH = ? kJ mol-1
Given the following data, 2 O3(g) ----> 3 O2(g) ∆rH = -377.00 kJ mol-1 O2(g) ----> 2...
Given the following data: 2O3(g) 3O2(g) -427 kJ O2(g) 2O(g) 495 kJ NO(g) + O3(g) NO2(g) + O2 -199kJ Calculate (in kJ) for the reaction: NO(g) + O(g) NO2(g)
Assume the reaction 3 O2(g) <===> 2 O3(g) (Delta H° =285 kJ/mol) is at equilibrium. What effect will each of the following have (explain each)? a) adding more O2 b) adding more O3 c) removing O3 d) increasing pressure in the container e) adding an inert gas f) increasing the temperature in the container
determine delta H for Cl(g) + O3(g) —> ClO(g) +O2(g) 2 O3(g) -> 3 O2(g). H=-29.90 kj/mol ClO(g) + O3(g) -> Cl(g) + 2 O2(g). H=+24.18 kj/mol report to 4 sigfigs
For the following reaction 3 O2 (g) → 2 O3 (g) ΔH = +286 kJ What is the ΔH when 16.0 g of O3 are produced
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
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. Blank 1 b. Determine the temperature(oC) at which the reaction is at equilibrium.
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
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 3 O2 (g) ⇌ 2 O3 (g) The conditions for this reaction are: PO2 = 1.64 bar PO3 = 1.28 bar .
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. b. Determine the temperature(oC) at which the reaction is at equilibrium.
18. Consider the following data. 2 NO(g) N2(g) + O2(g) H = -180.7 kJ 2 NO(g) + O2(g) 2 NO2(g) H = -113.1 kJ 2 N2(g) + O2(g) 2 N2O(g) H = +163.2 kJ Use Hess's law to calculate H for the reaction below. 3 NO(g) N2O(g) + NO2(g) H = ______________ kJ