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Calculate the change in enthalpy for the following reaction, using the appropriate standard enthalpies of formation given below. ΔfH°[FeCℓ3(s)] = -412 kJ mol-1 ΔfH°[FeCℓ2(s)] = -360 kJ mol-1 ΔfH°[HCℓ(aq)] = -167.1 kJ mol-1 ΔfH°[HCℓ(g)] = -127 kJ mol-1 | Bereken die entalpie-verandering vir die volgende reaksie met behulp van die toepaslike standaard vormingsentalpieë hieronder. ΔfH°[FeCℓ3(s)] = -412 kJ mol-1 ΔfH°[FeCℓ2(s)] = -360 kJ mol-1 ΔfH°[HCℓ(aq)] = -167.1 kJ mol-1 ΔfH°[HCℓ(g)] = -127 kJ mol-1 |
2 FeCℓ2(s) + 2 HCℓ(g) → 2 FeCℓ3(s) + H2(g)
| For which one of the following reactions is ΔrxnH° equal to the heat of formation (ΔfH°) of the product? | Vir watter van die volgende reaksies is ΔrxnH° gelyk aan die vormingswarmte (ΔfH°) van die produk? |
| 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