Which of these would be the correct equation to accompany the heat of formation value for NO2(g), AHNO2 (g) = 34 kJ/mol...
The AG = 51.0 kJ/mol, for the formation of NO2. Calculate the Kp value at 25°C for the reaction: 2 O2 (g) + N2 (g) → 2 NO2 (g) RT AGE=Lnk Slovo - 18.34 (293) '=-RT Lnk RT slegt/mol $1,000/00 -20.58 25+273= 278 78e-20.88 13 2X10 115x107 Kp = 1.18 X10-
Calculate the standard enthalpy of formation of NO(g) (in kJ/mol) from the following data. N2(g) + 2 O2(g) → 2 NO2(g) ΔH⁰298 = 66.4 kJ 2 NO(g) + O2(g) → 2 NO2(g) ΔH⁰298 = −116.2 kJ
Standard Enthalpies of Formation, in kJ/mol N2(g) 0 NO2(g) +33.2 NH3(g) -45.9 H2O(l) -285.8 NO(g) +90.3 N2O(g) -82.1 H2O(g) -241.8 Use the data above to calculate ΔH for the reaction: 6 NO2(g) + 8 NH3(g) => 7 N2(g) + 12 H2O(g) ΔH = ?
Determine the amount of heat (in kJ) given off when 1.26 × 104 g of NO2 are produced according to the equation 2 NO(g) + O2(g) → 2 NO2(g) ∆H = –114.6 kJ/mol The molar mass of NO2 is 46.01 g/mol.
The standard heat of formation for UF6(g) is -2.11x103 kJ/mol at 298 K. Write the formation equation for UF6(g) that goes with this value of AH°. Use the pull-down boxes to specify states. Write fractions with a slash, such as 1/2 for one half. Ifa box is not needed leave it blank Submit Answer
The standard heat of formation for CCl4(g) is -103 kJ/mol at 298 K. Write the formation equation for CCl4(9) that goes with this value of ΔΗ. Enter carbon as C($). Use the pull-down boxes to specify states. Write fractions with a slash, such as 1/2 for one half. If a box is not needed leave it blank. Submit Answer
Using the provided table and the equation below, determine the heat of formation for KCIO2. 2 KCIO: (s) 2 KCIO2 (s) + O2 (g) AH° = 296.2 kJ/mol Substance kJ/mol AHi" (kJ/mol) KCIO3 (s) -391.2 1 3 2 4 5 6 с O2 (g) 0 7 8 9 +/- 0 X 100
Heat of Formation Calculations: 32) Use a standard enthalpies of formation (Ho) table to determine the change in enthalpy for each of these reactions Hrxn [n. Ho(products) - n. Ho(products)] CO (g): -110.5 kJ/mol; CO2 (g): -393.5 kJ/mol CH4 (g): -890.4 kJ/mol H2O (l): -285.8 kJ/mol; H2O (g): -241.8 kJ/mol H2S (g): -20.6 kJ/mol; NO: -90.2 kJ/mol NO2: +33.9 kJ/mol; HCl (g): -92.3 kJ/mol NaOH (s): -426.7 kJ/mol; SO2 (g): -296.8 kJ/mol a) CH4(g) + 2 O2(g) ---> CO2(g) +...
Write the thermochemical equation that would be used to represent the standard heat of formation of sodium bicarbonate, NaHCO3(s). Na(s) + H2(g) + C(s) + H20(1) NaHCO3(s) AH° = -947.7 kJ/mol Na2O(s) + H2O(g) + CO2(g) + O2(g) + NaHCO3(s) AH = -947.7 kJ/mol O Na(s) + 0.5H2(g) + C(s) + 1.502(g) + NaHCO3(s) AH = -947.7 kJ/mol Na2CO3(s) + H20(1) - NaHCO3(s) AH = -947.7 kJ/mol
8) For which one of the following reactions is AHⓇxn equal to the heat of formation of the product? A) N2(g) + 3H2(g) + 2NH3 (8) B)(1/2)N2(g) + O2(g) → NO2(g) C) 6C(s) + 6H (g) → C6H6 (1) D) P (8) + 4H (g) + Br(g) - PH4Br (1) E) 12C (g) + 11H2(g) + 110 (g) → C6H22011 (8) (8) - PH4Br (1) A 9) The AE of a system that releases 12.4 J of heat and does...