CHEMISTRY 105 REVIEW WORKSHEET FOR EXAM 2This is a cooperative assignment to work with other students. It will not be collected or graded. You should be able to answer all questions on this worksheet without reference to your text, labmanual, or notes. But this worksheet should not be your sole study material. If you require onecomprehensive review of the material on the exam, use the homework. This worksheet will bedistributed in tutorial and posted on the course web site. The answer key will be posted onThursday morning. Until then, your TA can confirm or correct your answers. 1. Calculate the value of ÄE for the following reactions:a) A reaction absorbs 6.92kJ of heat and does 1.42kJ of work on its surroundingsb) A reaction releases 4.67kJ of heat and does 2.88kJ of work on its surroundingsc) A system absorbs 801.2 J of heat and expands from a volume of 1.504 L to a volume of5.120 L against a constant pressure of 2.008 atm.d) A system with a heat capacity of 61.52 J/EC changes volume from 9.225 L to 4.500 Lagainst a constant pressure of 3.820 atm while changing temperature from 20.18 EC to36.21 EC. 2. Calculate the heat energy required to raise the temperature of 250.0mL of water from 23.2ECto 75.9EC.3. 75.00 g of hot iron metal are placed in 150.00 g of 23.20 EC water. The metal cools and thewater heats up until both are 37.43 EC. What was the initial temperature of the iron?2[Specific heats: Fe (s) = 0.4492 J/gAEC, H O (l) = 4.184 J/gAEC] Assume no loss of heat energyto the surroundings.4. Draw the heating curve for 100.00 g of X starting -80.0EC and ending at 320.0 EC.if X has thefusfollowing properties: melting point = 12.6 EC, boiling point = 176.4 EC, ÄH = 1.056 kJ/g,vap s s sÄH = 3.543 kJ/g, c (s) = 1.855 J/gAEC, c (l) = 1.282 J/gAEC, c (g) = 0.6307 J/gAEC5. How much energy is required heat 454g of lead from 25°C to 327°C and then completely meltfusthe lead? For lead c = 0.159J/g°C and ÄH = 24.7J/g.6. 42.00g of cesium chloride are dissolved in 100.0mL of water at an initial temperature of25.40EC. The temperature of the solution is 9.10EC. What is the heat of solution of cesiumchloride?3 2 2 27. Given: 4 NH (g) + 7 O (g) 4 NO (g) + 6 H O ÄH° = -1132kJa) What is the total enthalpy change if 25.00g of oxygen are consumed in this reaction?b) If all the heat obtained by the combustion of 7.25g of ammonia were applied to a copperblock with a mass of 2.50 kg at an initial temperature of 25.0°C, what is the final temperature ofpthe copper block? [C of copper is 0.385 J/g°C]8. Isooctane is is a liquid with a density of 0.6878g/mL. It burns in oxygen to produce carbon8 18 2 2 2dioxide and water: 2 C H (l) + 25 O (g) 16 CO (g) + 18 H O (g) ÄH=-10922 kJIf 350.0mL of isooctane are burned, what is the quantity of heat that is evolved?7 129. 0.3650 g of a compound with the formula C H are combusted in a bomb calorimeter with aheat capacity of 308.8 J/EC. The temperature increases from 18.02 EC to 36.77 EC. What is thevalue of ÄE for the combustion of this compound?10. Write the balanced chemical equations that correspond to the following standard enthalpychanges:f 3 combustion 5 12a) ÄHE (NH ) b) ÄHE (C H O)11. Calculate the heat of formation for strontium carbonate from the following:22 Sr (s) +O (g) 2 SrO (s) ÄH=-1184 kJ2 3SrO (s) + CO (g) SrCO (s) ÄH=-234 kJ2 2C (s) + O (g) CO (g) ÄH=-394 kJ12 22 1112. The enthalpy of combustion of sucrose (C H O ) is -5.18x10 kJ/mole. The enthalpy of3formation of carbon dioxide gas is -393.5kJ/mol. The enthalpy of formation of water vapor is -241.8kJ/mol. Use this information to calculate the heat of formation of sucrose. Show ALLwork.13. 1.003 kg sample of carbon dioxide is sealed in a steel container with an internal volume of142.7L. If the tank and it’s contents are maintained at a temperature of 35.0EC, what is thepressure inside the tank?14. What is the density of a sample of nitrogen gas at -52.6EC and 0.880 atm?15. A sample of a compound is boiled and the vapor fills a 5.000L flask at a temperature of145.0EC and a pressure of 698.2 torr. The flask is cooled to condense the vapor back to theliquid state (the flask is sealed during cooling to prevent loss). The mass of the flask and thecondensed liquid is 727.90g. The mass of the empty flask is 708.07g. What is the molar mass ofthe gas?16. Potassium chlorate decomposes upon heating to form potassium chloride and oxygen gas. a. Write a balanced chemical equation for this process.b. If 83.69g of potassium chlorate are is heated and the reaction goes to completion, whatvolume of oxygen gas (at 22.0EC and 1.042 atm) is produced?17. What volume of carbon dioxide gas, at 23.5EC and 800.0 torr will react with 6.500L of2 2 3 20.556M of lithium hydroxide? 2 LiOH (aq) + CO (g) Li CO (aq) + H O (l) 18. A mixture of gasses is found to be 25.50% hydrogen and 18.75% argon by volume. The restof the gas is nitrogen with a partial pressure of 1393.75 torr. Determine the following:a) The mole fraction of nitrogenb) The partial pressure of hydrogenc) the mass% of argon in this mixture19. Consider three gas samples. Each has 0.100 mole of gas sealed in a 5.00L flask at atemperature of 298K. The gas samples are helium, carbon dioxide, and chlorine Compare thefollowing properties for these gas samples [state which sample would have the larger value andexplain your reasoning]:a) Pressure, b) Average kinetic energy, c) Average molecular speed, d) Gas Density20. The following diagrams depict a mixture of nitrogen, neon, and water vapor sealed in a50.00L container at a temperature of 20.0°C. Each atom or molecule of gas represents 1.000 molof that atom or molecule. Determine the following for each mixture: a) the mole fraction of eachgas, b) the % volume of each gas, c) the partial pressure of each gas.21. For the gasses sulfur dioxide, oxygen, argon:a) calculate the density of each gas at 50.0°C and 1.200atm.b) Rank these gasses in order of increasing rate of effusion22. A 0.100 mole sample of ammonia gas diffuses across a room in 103.4 s at 25.0 EC. Howlong would be required for a 0.100 mol sample of sulfur dichloride gas to diffuse across the roomat 25.0 EC?23. Nitrogen gas can be generated by the decomposition of sodium azide:3 22 NaN (s) 2 Na (s) + 3 N (g)This reaction is