2 iii Increasing the temperature will increase the AMOUNT of calcium hydroxide

# 2 iii increasing the temperature will increase the

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/2iii) Increasing the temperature will increase the AMOUNT of calcium hydroxide that willdissolve./2iv) Increasing the temperature will increase the RATE at which calcium hydroxide willdissolve./2 CHEM 105Exam 2Fall 20169) a) Methane gas (CH4) is used as a fuel source for mechanical devices. Hydrogen gasreacts with graphite to produce methane. Use the following thermochemical equationsto determine the ΔHroof the reaction to produce methane gas.(1)C(s, graphite) + O2(g) → CO2(g)ΔHo= -393.5 kJ/mol(2)CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)ΔHo= -890.3 kJ/mol(3)H2(g) + 0.5 O2(g) → H2O(l)ΔHo= -285.8 kJ/mol/8b) If 4.0 moles of methane are combusted (reaction 2 above) and the heat is transferred toa water bath containing 100. g of water at 25oC, what is the final temperature of the waterafter the reaction? The heat capacity of water is 4.18 J g-1K-1./6c) For reactions 1-3 in part (a), which of the reactions are redox reactions?/4d) For one of the reactions in part (a) that you identified as a redox reaction, identify the:oxidizing agent:reducing agent:/4 CHEM 105Exam 2Fall 201610) a) Five samples of argon gas are described in the table below. Rank the samples inorder of increasing average kinetic energy (1 (lowest) to 5 (highest)).AmountPressureTemperaturerank2.0 mol1.9 atm-48.oC1.7 mol2.6 atm-73.oC1.4 mol3.0 atm-87.oC1.9 mol1.2 atm-63.oC1.2 mol1.5 atm-66.oC/4b) Determine the molar volume of the 1stargon sample on the list (1.9 atm and -48.oC).c) Consider two 10. L flasks. One flask is filled with N2(g) at 1.0 atm and 298 K. The second/6flask if filled with an equal mass of O2(g). If the temperature of the O2(g) flask is adjusteduntil the root-mean-square velocity of both gases is equal, what is the temperature of theO2(g) flask?/6d) If the two flasks in part (c) are mixed together and allowed to reach a constanttemperature, which gas will have the higher partial pressure? Explain how you knowwithout calculation./4 CHEM 105Exam 2Fall 201611) For a-c, please write the formula equation, complete ionic, and net ionic equation foreach of the following reactions and label the reaction type (precipitation, redox, or acid-base).a)Ammonia (NH3) reacts with hydrobromic acid.Formula equation:Complete ionic equation:Net ionic equation:Equation type/8b)Manganese(II) nitrate reacts with lead(II) nitrate to produce manganese(III) nitrateand lead(I) nitrate. The chemical symbol of manganese and lead are Mn and Pb,respectively.Formula equation:Complete ionic equation:Net ionic equation:Equation type/8c)Sodium bromide reacts with lead(II) nitrate.Formula equation:Complete ionic equation:Net ionic equation:Equation type/8d) Using a description of a solvated ion on the molecular level, explain in completesentences why spectator ions are canceled out when writing a net ionic reaction./4 CHEM 105Exam 2Fall 2016NameQuestionScoreOut of1-7/148/169/2210/2011/28Total100 Constants and equations: Speed of light: c = 2.997x108ms-1Plank’s constant: h=6.626x10-34J∙s 1 J = 1 kg∙m2∙s-2charge of an e-: e = 1.602x10-19C mass of e-: me=9.11x10-31kg mass of p+: mp=1.67x10-27kg 𝐸𝐸=ℎ ∙ 𝜈𝜈Avogadro’s constant: NA= 6.022x1023mol-1DeBroglie Relation: 𝜆𝜆=𝑚𝑚∙v=𝑝𝑝𝐸𝐸=2.18 × 10−18𝐽𝐽 ∙ �𝑍𝑍2𝑛𝑛2∆𝐸𝐸=2.18 × 10−18  #### You've reached the end of your free preview.

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