Potassium chlorate, a common oxidizing agent in fireworks and matchheads, undergoes decomposition when heated: 4 KCIO3(s)...
Potassium chlorate, a common oxidizing agent in fireworks and matchheads, undergoes decomposition when heated 4 KCIO3(s) + 3 KC1O4(s) + KC1(s) AH°rxn-144.3 kJ/mol, AS rxn--36.8 J/mol K. Calculate AGºrxn for this reaction. AGⓇ rxn=
8. Potassium chlorate is a common oxidizing agent in match heads and in fireworks. When heated, it goes through a solid-state disproportionation reaction. Calculate and state if the reaction is spontaneous or not? AG sys at 298 K, given AHºsys = -144.0 kJ and ASºsys = -37.0 J/K. (5 points) 4KCIO3(s) + 3KCIO4(s) + KCl(s)
Potassium chlorate (KCIO3) is often used to generate oxygen according to its decomposition reaction (shown below): A.9 2KCI (s) +302(g) 2KCIO3(s) AH (kJ mol) S (JK mol) KCIO3 (s) KCI (s) 397.8 143.1 -435.9 82.6 O2 (g) 0 205.0 Use the thermochemical data provided above to calculate the standard change in Gibbs Energy (AG for this reaction at a temperature of 298K AH 88.6 kJ (A) 4G. AH-TOs (B) -88.6 kJ (C) -223.4 kJ (D) +223.4 kJ (E) 266.1 kJ...
Gummy bears decompose rapidly and explosively in molten potassium chlorate. Both decomposition and combustion reactions happen simultaneously according to the balanced equation: C12H22011(s) + 8 KClO3(1) --> 12 CO2(g) + 11 H2O(g) + 8 KCl(aq) Using the AHºf values below, calculate the standard enthalpy change for this reaction. (Report your answer in standard notation.) C12H22011 (8) KCIO3 (1) CO2 (g) H2O (g) KCl (aq) A Hºf (kJ/mol) -2225.5 -397.73 -393.51 -241.82 -436.7 AH° rxn = * kJ
Gummy bears decompose rapidly and explosively in molten potassium chlorate Both decomposition and combustion reactions happen simultaneously according to the balanced equation CH,2011(s) + 8 KCIO3(1) -->12 COX) +11 H2O(g) + 8 KCl(aq) Use the free energy of formation values below to calculate AG CH2011) KCIO, (1) CO, (2) H:0 () KCI(Q) AGⓇ, (kJ/mol) -1544.6 -296 25 -394 36 -228 57 409 14 AG
Gummy bears decompose rapidly and explosively in molten potassium chlorate. Both decomposition and combustion reactions happen simultaneously according to the balanced equation C2H2011(s) + 8 KCIO,(0) -> 12 CO () +11 H2O(g) +8 KCl(aq) Using the values below, calculate the standard entropy change for this reaction (Report your new in standard notation) C12H2011 (8) KCIO, (1) CO, H,0 KCI () S (J/mol K) 3602 143.1 213.74 15883 82 59 AS =
4. Using Hess's Law, calculate the enthalpy of formation of potassium chlorate: K (s) + Cl2 (g) + 3/2 02 (g) →KCIO: (s) AH = ? kJ Based on the enthalpy changes for the following reactions: 2 K (8) + Cl2 (g) → 2 KCI (3) AH - 874.0 kJ KCIO: (s) + 3 Mg (8) ► KCl (s) + 3 Mg0 (8) AHxx. - 1852.0 kJ MgO (3) ► Mg (s) + O2(g) AHan = +602.0 kJ
thermometer coffee cups containing reaction mixture When a 7.89-9 sample of solid potassium chlorate dissolves in 32.0 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 20.00 °C to 3.899 °C. Calculate AH in kl/mol KCIOy for the solution process. KCIO,(s) - K*(aq) + CIO,'(aq) The specific heat of water is 4.18 3/ok Aucution - Kl/mol KCO,
this is a lab of Percentage of Oxygen in Potassium Chlorate Percentage of Oxygen in Potassium Chlorate Purpose of the lab Te esperimentar e te m o rgen in een constante decoration of poche Introduction The thermal decomposition of potassium chore can be described by the following 2KCIO 2 Cl +30 Ent epeal tehnic p e cale from the KCIO We poschodecomposes simply by heating the reaction is very Actitud is a m a ture accent the reaction, we not...
AH-116.4 kJ/mol 4. Consider the following reaction: NH.NO, (s) N20 (8) + 2 H20 (g) Calculate AGⓇ for the reaction. Substance S” (J/mol K) NH.NO, (3) 151 N:0 (8) 220 H:0 (9) 183 5. The first step in the commercial production of titanium metal is the reaction of Tio: with chlorine an graphite: TiO2 (s) + 2 Cl: (g) + 2C (5) Tici: (1) + 2 CO(g) Calculate AGº for the reaction. Substance AG? (kJ/mol Substance AG® (kJ/mol) C(s) TiCl...