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What is the ΔH°vap of a liquid that has a vapor pressure of 624 torr at 85.2°C and a boiling point of 93.2°C at 1 atm? Answer in J/mol
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- An engine generates 15.7 g of nitric oxide gas during a laboratory test. How much heat was absorbed in producing this NO? 46.93 kJ 85,015.5 kJ 49.85 J 94.4 kJ N₂(g) + O₂(g) NO(g): : AH° = 180.5 kJConsider the following information. 2 H₂S(g) +3 O2(g) → 2 SO2(g) + 2 H₂O(g) H2S(g) O2(g) 205.2 SO2(g) 248.2 H₂O(g) 188.8 S°(J/mol K) 205.8 (1) Calculate the AS 'rxn. (2) Calculate the AG rxn at 298K. The answer to (1) is [Select] The answer to (2) is [Select] AH f = -1.036 x 106 JDetermine the amount of heat lost or gained by 2.50 moles of gaseous water in a closed container, with the pressure kept at 1 atm and the temperature changing from 130 °C to 30 °C, given the following: C (H,O6) = 33.1 J/mol·K C (H,Ou) = 75.4 J/mol·K C (H,Og) = 37.6 J/mol·K (). ΔΗΟ, vap = 40.7 kJ/mol ΔΗ' fus = 6.02 kJ/mol (s).
- The amount of heat required to convert one mole of a substance from liquid to gas is known as the heat of vaporization. For instance the heat of vaporization of water is 44.00 kJ/mol (see below). H2O(l) ⟶⟶ H2O(g) ΔH=44.00kJΔH=44.00kJ An experiment was conducted to determine the heat of vaporization of methanol (CH4O). It was determined that 10.34 kJ of heat are required to convert 10.00 grams of methanol from liquid to gas. Based on these experimental results calculate the heat of vaporization (kJ/mol) of methanol. Do not type units into your answer. CH4O(l) ⟶⟶ CH4O(g) ΔH=?14) 500.0 mL of steam (density = 0.589 g/L) at 100.0°C is mixed with 5.000 mL of liquid mercury (density = 13.6 g/mL) at -20.0°C. What is the final temperature and state of each substance? (Note: the boiling point of mercury is above 100°C.) Specific heat of Hg(1) = 0.138 J/g °C Specific heat of H₂O(1) = 4.18 J/g-°C Heat of vaporization of H₂O (at 100°C) = 40.7 kJ/molIs the following process exothermic or endothermic? 2H(g) ⟶⟶ H2(g)
- In CHEM 151 class, engineering students examine the heat release in a phase transition process. In a typical experiment, a 70 g of steam at 120°C is converted to a liquid water at 50 °C. What will students calculate the heat release in this experiment? (Specific heat of water = Specific heat of steam = 4.18 J/°C.g; ΔHvap = -ΔHcond= –40.79 kJ/mol; R=8.314 J/mol.K; H2O=18.02 g/mol)The normal boiling point of water is 100°C (373 K) at 1.00 atm. Calculate the boiling point of water in °C if a pressure of 2.00 atm is applied on its surface? (AHvap = 40.6 kJ/mol; R = 8.314 J/mol.K)2:41 PM Mon Jan 30 Question 15 of 20 What amount of heat (in kJ) is required to convert 10.1 g of an unknown liquid (MM = 67.44 g/mol) at 43.5 °C to a gas at 128.2 °C? (specific heat capacity of liquid = 1.18 J/g °C; specific heat capacity of gas = 0.792 J/g °C; AHvap = 30.1 kJ/mol; normal boiling point, Tb = 97.4 °C) Tap here or pull up for additional resources +
- 7:02 AM Wed Feb 1 Question 14.c of 26 Consider the heating curve provided for 1.00 mole of a substance that begins as a solid at -14.8 °C and ends as a gas at 121.1 °C. Specific heat capacities: solid = 145.6 J/ mol °C, liquid=97.25 J/mol °C, gas = 68.49 J/mol. °C Step C: What quantity of heat energy (in kJ) must be absorbed to increase the temperature of the liquid from the melting temperature to the boiling temperature? Learn More in OpenStax5. What amount of heat (in kJ) is required to convert 10.1 g of an s (1) unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 1.58 J/(g-°C) s (g) 0.932 J/(g-°C) 93.5 °C? 57.3 °C AHa 22.5 kH/molCalcium carbonate can decompose into calcium oxide and carbon dioxide: CaCO3(s) 2 CaO(s) + CO2(g) AH; -1206.9 -635.1 -393.5 (kJ/mol) S° 92.9 39.8 213.7 (J/mol K) Pressure of CO2(g) is 1.0 atm. Assuming that AH° and AS° are independent of temperature, at what temperature will this reaction be at equilibrium? 298 K 25°C 1100K 1100 °C O O O O