CHEMISTRY 1111 LAB MANUAL >C<
1st Edition
ISBN: 9781307092097
Author: Chang
Publisher: MCG/CREATE
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Textbook Question
Chapter 6, Problem 6.116QP
(a) A person drinks four glasses of cold water (3.0°C) every day. The volume of each glass is 2.5 × 102 mL. How much heat (in kJ) does the body have to supply to raise the temperature of the water to 37°C, the body temperature? (b) How much heat would your body lose if you were to ingest 8.0 × 102 g of snow at 0°C to quench thirst? (The amount of heat necessary to melt snow is 6.01 kJ/mol.)
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Obtain 2-methylbutanoic acid by malonic or acetylacetic synthesis (indicate the formulas of the compounds involved).
EFFICIENTS
SAMPLE READINGS
CONCENTRATIONS
Pigiadient)
TOMATO SAUCE (REGULAR)
TOMATO (REDUCED SALT)
TOMATO SAUCE (REGULAR)
TOMATO (REDUCED SALT)
58
6.274
3.898
301.7
151.2
14150
5.277
3.865
348.9
254.8
B
5.136
3.639
193.7
85.9
605
4.655
3.041
308.6
199.6
05
5.135
3.664
339.5
241.4
0139
4.676
3.662
160.6
87.6
90148
5.086
3.677
337.7
242.5
0092
6.348
3.775
464.7
186.4
PART3
5.081
3.908
223.5
155.8
5.558
3.861
370.5
257.1
4.922
3.66
326.6
242.9
4.752
3.641
327.5
253.3
50
5.018
3.815
336.1
256.0
84
4.959
3.605
317.9
216.6
38
4.96
3.652
203.8
108.7
$3
5.052
3.664
329.8
239.0
17
5.043
3.767
221.9
149.7
052
5.058
3.614
331.7
236.4
5.051
4.005
211.7
152.1
62
5.047
3.637
309.6
222.7
5.298
3.977
223.4
148.7
5.38
4.24
353.7
278.2
5
5.033
4.044
334.6
268.7
995
4.706
3.621
305.6
234.4
04
4.816
3.728
340.0
262.7
16
4.828
4.496
304.3
283.2
0.011
4.993
3.865
244.7
143.6
AVERAGE
STDEV
COUNT
95% CI Confidence Interval (mmol/L)
[Na+] (mg/100 mL)
95% Na+ Confidence Interval (mg/100 mL)
If we have two compounds: acetone (CH₃COCH₃) and acetic acid (CH₃COOH), applying heat to them produces an aldol condensation of the two compounds. If this is correct, draw the formula for the final product.
Chapter 6 Solutions
CHEMISTRY 1111 LAB MANUAL >C<
Ch. 6.2 - Classify each of the following as an open system,...Ch. 6.3 - A gas expands from 264 mL to 971 mL at constant...Ch. 6.3 - A gas expands and does P-V work on the...Ch. 6.3 - Two ideal gases at the same temperature and...Ch. 6.4 - Calculate the heat evolved when 266 g of white...Ch. 6.4 - What is U for the formation of 1 mole of CO at 1...Ch. 6.4 - Which of the constant-pressure processes shown...Ch. 6.5 - An iron bar of mass 869 g cools from 94C to 5C....Ch. 6.5 - A quantity of 1.922 g of methanol (CH3OH) was...Ch. 6.5 - A 30.14-g stainless steel ball bearing at 117.82C...
Ch. 6.5 - A quantity of 4.00 102 mL of 0.600 M HNO3 is...Ch. 6.5 - A 1-g sample of Al and a 1-g sample of Fe are...Ch. 6.6 - Which of the following does not have Hfo=0 at 25C?...Ch. 6.6 - Calculate the standard enthalpy of formation of...Ch. 6.6 - Benzene (C6H6) burns in air to produce carbon...Ch. 6.6 - Explain why reactions involving reactant compounds...Ch. 6.7 - Use the data in Appendix 2 to calculate the heat...Ch. 6 - Define these terms: system, surroundings, open...Ch. 6 - What is heat? How does heat differ from thermal...Ch. 6 - What are the units for energy commonly employed in...Ch. 6 - A truck initially traveling at 60 km per hour is...Ch. 6 - These are various forms of energy: chemical, heat,...Ch. 6 - Define these terms: thermochemistry, exothermic...Ch. 6 - Stoichiometry is based on the law of conservation...Ch. 6 - Describe two exothermic processes and two...Ch. 6 - Decomposition reactions are usually endothermic,...Ch. 6 - On what law is the first law of thermodynamics...Ch. 6 - Explain what is meant by a state function. Give...Ch. 6 - The internal energy of an ideal gas depends only...Ch. 6 - Consider these changes: (a) Hg(l)Hg(g) (b)...Ch. 6 - A sample of nitrogen gas expands in volume from...Ch. 6 - A gas expands in volume from 26.7 mL to 89.3 mL at...Ch. 6 - A gas expands and does P-V work on the...Ch. 6 - The work done to compress a gas is 74 J. As a...Ch. 6 - Calculate the work done when 50.0 g of tin...Ch. 6 - Calculate the work done in joules when 1.0 mole of...Ch. 6 - Prob. 6.21QPCh. 6 - In writing thermochemical equations, why is it...Ch. 6 - Explain the meaning of this thermochemical...Ch. 6 - Consider this reaction:...Ch. 6 - The first step in the industrial recovery of zinc...Ch. 6 - Determine the amount of heat (in kJ) given off...Ch. 6 - Consider the reaction...Ch. 6 - Consider the reaction...Ch. 6 - What is the difference between specific heat and...Ch. 6 - Define calorimetry and describe two commonly used...Ch. 6 - Consider the following data: Metal Al Cu Mass (g)...Ch. 6 - A piece of silver of mass 362 g has a heat...Ch. 6 - A 6.22-kg piece of copper metal is heated from...Ch. 6 - Calculate the amount of heat liberated (in kJ)...Ch. 6 - A sheet of gold weighing 10.0 g and at a...Ch. 6 - To a sample of water at 23.4C in a...Ch. 6 - A 0.1375-g sample of solid magnesium is burned in...Ch. 6 - A quantity of 85.0 mL of 0.900 M HCl is mixed with...Ch. 6 - What is meant by the standard-state condition?Ch. 6 - How are the standard enthalpies of an element and...Ch. 6 - What is meant by the standard enthalpy of a...Ch. 6 - Write the equation for calculating the enthalpy of...Ch. 6 - State Hesss law. Explain, with one example, the...Ch. 6 - Describe how chemists use Hesss law to determine...Ch. 6 - Which of the following standard enthalpy of...Ch. 6 - The Hfo values of the two allotropes of oxygen, O2...Ch. 6 - Which is the more negative quantity at 25C: Hfo...Ch. 6 - Predict the value of Hfo (greater than, less than,...Ch. 6 - In general, compounds with negative Hfo values are...Ch. 6 - Suggest ways (with appropriate equations) that...Ch. 6 - Calculate the heat of decomposition for this...Ch. 6 - The standard enthalpies of formation of ions in...Ch. 6 - Calculate the heats of combustion for the...Ch. 6 - Calculate the heats of combustion for the...Ch. 6 - Methanol, ethanol, and n-propanol are three common...Ch. 6 - The standard enthalpy change for the following...Ch. 6 - From the standard enthalpies of formation,...Ch. 6 - Pentaborane-9, B5H9, is a colorless, highly...Ch. 6 - Determine the amount of heat (in kJ) given off...Ch. 6 - At 850C, CaCO3 undergoes substantial decomposition...Ch. 6 - From these data,...Ch. 6 - From the following data,...Ch. 6 - From the following heats of combustion,...Ch. 6 - Calculate the standard enthalpy change for the...Ch. 6 - Prob. 6.65QPCh. 6 - Why is the lattice energy of a solid always a...Ch. 6 - Consider two ionic compounds A and B. A has a...Ch. 6 - Mg2+ is a smaller cation than Na+ and also carries...Ch. 6 - Why is it dangerous to add water to a concentrated...Ch. 6 - Which of the following does not have Hfo=O at 25C?...Ch. 6 - Calculate the expansion work done when 3.70 moles...Ch. 6 - Prob. 6.73QPCh. 6 - Given the thermochemical equations:...Ch. 6 - The standard enthalpy change H for the thermal...Ch. 6 - Hydrazine, N2H4, decomposes according to the...Ch. 6 - A quantity of 2.00 102 mL of 0.862 M HCl is mixed...Ch. 6 - A 3.53-g sample of ammonium nitrate (NH4NO3) was...Ch. 6 - Consider the reaction...Ch. 6 - Prob. 6.80QPCh. 6 - Prob. 6.81QPCh. 6 - A 2.10-mole sample of crystalline acetic acid,...Ch. 6 - Prob. 6.83QPCh. 6 - You are given the following data:...Ch. 6 - A gaseous mixture consists of 28.4 mole percent of...Ch. 6 - When 2.740 g of Ba reacts with O2 at 298 K and 1...Ch. 6 - Methanol (CH3OH) is an organic solvent and is also...Ch. 6 - A 44.0-g sample of an unknown metal at 99.0C was...Ch. 6 - Using the data in Appendix 2, calculate the...Ch. 6 - Producer gas (carbon monoxide) is prepared by...Ch. 6 - Prob. 6.91QPCh. 6 - Prob. 6.92QPCh. 6 - Ethanol (C2H5OH) and gasoline (assumed to be all...Ch. 6 - The combustion of what volume of ethane (C2H6),...Ch. 6 - Prob. 6.95QPCh. 6 - Prob. 6.96QPCh. 6 - Explain the cooling effect experienced when...Ch. 6 - For which of the following reactions does...Ch. 6 - Prob. 6.99QPCh. 6 - A quantity of 0.020 mole of a gas initially at...Ch. 6 - Prob. 6.101QPCh. 6 - Prob. 6.102QPCh. 6 - Prob. 6.103QPCh. 6 - Prob. 6.104QPCh. 6 - A person ate 0.50 pound of cheese (an energy...Ch. 6 - Prob. 6.106QPCh. 6 - Prob. 6.107QPCh. 6 - The enthalpy of combustion of benzoic acid...Ch. 6 - Prob. 6.109QPCh. 6 - Prob. 6.110QPCh. 6 - Glaubers salt, sodium sulfate decahydrate (Na2SO4 ...Ch. 6 - A balloon 16 m in diameter is inflated with helium...Ch. 6 - Acetylene (C2H2) can be hydrogenated (reacting...Ch. 6 - Prob. 6.114QPCh. 6 - An excess of zinc metal is added to 50.0 mL of a...Ch. 6 - (a) A person drinks four glasses of cold water...Ch. 6 - Prob. 6.118QPCh. 6 - Why are cold, damp air and hot, humid air more...Ch. 6 - Prob. 6.120QPCh. 6 - Prob. 6.121QPCh. 6 - Prob. 6.122QPCh. 6 - Prob. 6.123QPCh. 6 - Determine the standard enthalpy of formation of...Ch. 6 - Prob. 6.125QPCh. 6 - Ice at 0C is placed in a Styrofoam cup containing...Ch. 6 - Prob. 6.127QPCh. 6 - Prob. 6.128QPCh. 6 - Calculate the internal energy of a Goodyear blimp...Ch. 6 - Prob. 6.131QPCh. 6 - Acetylene (C2H2) can be made by reacting calcium...Ch. 6 - The average temperature in deserts is high during...Ch. 6 - From a thermochemical point of view, explain why a...Ch. 6 - Calculate the U for the following reaction at 298...Ch. 6 - Lime is a term that includes calcium oxide (CaO,...Ch. 6 - A 4.117-g impure sample of glucose (C6H12O6) was...Ch. 6 - Construct a table with the headings q, w, U, and...Ch. 6 - The combustion of 0.4196 g of a hydrocarbon...Ch. 6 - Metabolic activity in the human body releases...Ch. 6 - Give an example for each of the following...Ch. 6 - From the following data, calculate the heat of...Ch. 6 - Starting at A, an ideal gas undergoes a cyclic...Ch. 6 - For reactions in condensed phases (liquids and...Ch. 6 - The diagrams (a)(d) represent various physical and...Ch. 6 - A 20.3-g sample of an unknown metal and a 28.5-g...Ch. 6 - Prob. 6.148QPCh. 6 - Prob. 6.149QPCh. 6 - The fastest serve in tennis is about 150 mph. Can...Ch. 6 - Prob. 6.151QPCh. 6 - It has been estimated that 3 trillion standard...Ch. 6 - Prob. 6.153QPCh. 6 - Prob. 6.154QPCh. 6 - Prob. 6.155QPCh. 6 - We hear a lot about how the burning of...
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