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.
Determine the amount of heat (in kJ) given off when 1.26 × 104 g of NO2...
determine the amount of heat (in KJ) given off when 1.26 x10^3 of NO2 are produced according to the equation 2NO(g) + O2(g) ---2NO2(g) delta H= -114.6 kj/mol
determine the amount of heat (in kj) given off when 4.53 * 10^4 g of ammonia is produced according to the equation below. assume that the reaction takes place under standard - state conditions at 25 celsius. N2(g) + 3H2(g) ---> 2NH3 ?H= -92.6 kJ/mol enter the answser in scientific notation
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given off, when 1.26 x 104 g of ammonia ( NH3 ) are produced according to the equation : N2 (g) + 3 H2 (g) → 2 NH3 (g) ....... AH ºrx = - 92.6 kJ Assume that the reaction occurs at Standard State conditions at 25 C. ANSWER : Total Heat Given Off: _ (units ?) 6. Standard Enthalpy of Formation and Reaction :...
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(l) For C6H12(l), ΔH°f = –151.9 kJ/mol (5 points) Substance ∆H°f , kJ/mol C6H12(l) –151.9 O2(g) 0 H2O(l) –285.8 CO2(g) –393.5 2).Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according to the equation N2(g) + 3H2(g) → 2NH3(g) ΔH°= –92.6 kJ/mol Assume that the reaction takes place under standard conditions at 25oC.
CHE 1211- General Chemistry 1 (Fall 17 Section 262 Heidi K d Homework-Chapter 5 0.00 points Check my work Be sure to answer all parts. Determine the amount of heat (in kJ) given off when 1.52 x 10 g of NO2 is produced according to the following equation: 2 NO(g) + O2(g) → 2NO2(g) Enter your answer in scientific notation. AH--114.6 kJ/mol kJ
Given the balanced chemical equation, 2 H(g) → H2(g) ΔH0rxn = −436 kJ/mol Determine the mass (in grams) of H(g) produced when 823 kJ of heat is released.
Which of these would be the correct equation to accompany the heat of formation value for NO2(g), AHNO2 (g) = 34 kJ/mol? NO2 (1) ► NO2 (8) ON (g) + O2(g) → NO2 (g) N2(g) + 2 O2(g) → 2 NO2 (g) OYN2 (g) + O2(g) → NO2 (g)
Given the following thermochemical equation, calculate the amount of heat (in kJ) that is released when 35.0 g of Na2O2 completely react with excess amount of water . 2 Na2O2 (s) + 2 H2O (l) → 4 NaOH (aq) + O2 (g) Δ H = - 126 kJ
What mass of ethane, C2H6, must be burned to provide 6.30 x 104 kJ of heat according to the given thermochemical equation: 2 C2H6 (g) + 7 O2 (g) -> 4 CO2 (g) + 6 H2O (l) ΔHrxn = -3119 kJ
Determine the amount of heat, in kJ, required to heat 41 g of solid Ca at 851C to 1,397 C. Melting Point = 851C Boiling Point = 14870 Molar Heat Capacities: Csolid = 26.2 J/mol C Cliquid = 31.0 J/mol AH_fusion = 9.33 kJ/mol AH_vaporization = 162 kJ/mol Determine the amount of heat, in kJ, required to convert 24 g of solid Ca at 116 C to its melting point of 851C. Melting Point = 851C Boiling Point = 1487C...