Chemistry / Chemie - 124
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| Nitroglycerin, C3H5(NO3)3, is a powerful explosive that forms four different gases when detonated: | Nitrogliserien, C3H5(NO3)3, is 'n kragtige plofstof wat vier verskillende gasse vorm wanneer dit ontplof: |
| 2 C3H5(NO3)3(ℓ) → 3 N2(g) + 6 CO2(g) + 5 H2O(g) ΔHo = -2842.1 kJ | |
Calculate the standard enthaly of formation (in kJ.mol-1) of CO2 if ΔfHo[C3H5(NO3)3(ℓ)] = -364.0 kJ.mol-1 and ΔfHo[H2O(g)] = -241.8 kJ.mol-1. (Please round your answer off to 1 decimal figure.) | Bereken die standaard vormingsentalpie (in kJ.mol-1) van CO2 indien ΔfHo[C3H5(NO3)3(ℓ)] = -364.0 kJ.mol-1 en ΔfHo[H2O(g)] = -241.8 kJ.mol-1. (Rond asb jou antwoord af tot 1 desimale syfer.) |
| The first step in the production of nitric acid from ammonia involves the oxidation of NH3 according to the balanced reaction below: | Die eerste stap in die produksie van salpetersuur vanaf ammoniak behels die oksidasie van NH3 volgens die gebalanseerde reaksie hieronder: |
| 4 NH3(g) + 5 O2 (g) → 4 NO(g) + 6 H2O(g) | |
How much energy is evolved or absorbed as heat in the oxidation of 10.1 g of NH3 if ΔfHo[NH3(g) = -45.9 kJ.mol-1, ΔfHo[NO(g)] = 90.3 kJ.mol-1 and ΔfHo[H2O(g)] = -241.8 kJ.mol-1. | Hoeveel energie word as hitte vrygestel of geabsorbeer tydens die oksidasie van 10.1 g NH3 indien ΔfHo[NH3(g)] = -45.9 kJ.mol-1, ΔfHo[NO(g)] = 90.3 kJ.mol-1 and ΔfHo[H2O(g)] = -241.8 kJ.mol-1. |
| The reaction below is _____, and therefore heat is _____. | Die reaksie hieronder is _____, en dus word hitte _____. |
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(ℓ) | ΔH° = − 890 kJ
| How many kilojoules are equivalent to 885 calories? | Hoeveel kjoule is gelyk aan 885 kalorieë? |
1 cal = 4.2 J
| Calculate the value of ΔU for a system that performs 112 kJ of work on its surroundings and gains itself 61 kJ of heat. | Bereken die waarde van ΔU vir 'n sisteem wat 112 kJ arbeid op die omgewing verrig maar self met 61 kJ aan warmte toeneem |
| Which of the following thermodynamic quantities are state functions | Watter van die volgende thermodinamiese groothede is toestandfunksies? |
| For which of the following is DfH° equal to zero at 25°C? | Vir watter van die volgende is die DfH° gelyk aan nul by 25°C? |
| Use Hess’s Law to determine the heat of reaction for the process. | Gebruik Hess se Wet om die reaksiewarmte vir die proses te bepaal. |
Fe2O3(s) → 2 Fe(s) + 3/2 O2(g)
i. 2 Fe(s) + 6 H2O(ℓ) → 2 Fe(OH)3(s) + 3 H2(g) | ΔH° = +321.8 kJii. H2(g) + ½ O2(g) → H2O(ℓ) | ΔH° = -285.8 kJiii. 2 Fe(OH)3(s) → Fe2O3(s) + 3 H2O(ℓ) | ΔH° = -288.6 kJ
| Magnesium pieces (0.492 g) react in dilute acidic solution (134 mL) as follows: | Magnesiumstukke (0.492 g) reageer in verdunde suuroplossing (134 mL) soos volg: |
| Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) | |
The temperature of the solution increases from 22.2 °C to 44.8 °C. Determine the enthalpy change for the reaction in kJ per mol Mg(s) that reacts. (Assume that the specific heat capacity of the solution, and density of HCl(aq) can be approximated by the values for pure water. Furthermore, no heat energy is exchanged with the calorimeter). | Die temperatuur van die oplossing styg van 22.2 °C tot 44.8 °C. Bepaal die entalpieverandering vir die reaksie in kJ per mol Mg(s) wat reageer. (Neem aan dat die spesifieke hittekapasiteit van die oplossing en die digtheid van HCl(aq) benader kan word deur die waardes vir suiwer water te gebruik. Verder word geen hitte-energie met die kalorimeter uitgeruil nie). |
| What is the resulting temperature when 20 g of water at 88°C is mixed with 21 g of water at 18°C? | Wat is die finale temperatuur as 20 g water by 88°C gemeng word met 21 g water by 18°C? |
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