Inorganic Chemistry
5th Edition
ISBN: 9781292134147
Author: Housecroft, Catherine E.
Publisher: Pearson,
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Chapter 1, Problem 42P
The sign convention for
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When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.
When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.
Which experimental number must be initialled by the Lab TA for the first run of Part 1 of the experiment?
a) the heat capacity of the calorimeter
b) Mass of sample
c) Ti
d) The molarity of the HCl
e) Tf
Predict products for the Following organic rxn/s by
writing the structurels of the correct products. Write
above the line provided"
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4 CH 3 11
3 CH 3 (CH2) 4 C-H + CH3OH
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2
Chapter 1 Solutions
Inorganic Chemistry
Ch. 1 - Chromium has four isotopes C2450r, C2452r, C2453r...Ch. 1 - Prob. 2PCh. 1 - Using the list of naturally occurring isotopes in...Ch. 1 - Hydrogen possesses three isotopes, but tritium ,...Ch. 1 - (a) By using the data in appendix 5, account for...Ch. 1 - Calculate the corresponding wavelength of...Ch. 1 - State which of the following n'n transitions in...Ch. 1 - Calculate the energy (in kJ per mole of photons)...Ch. 1 - 1.9 Four of the lines in Balmer series are at...Ch. 1 - 1.10 Using the Bohr model, determine the values of...
Ch. 1 - 1.11 How is the (a) energy and (b) size of an ns...Ch. 1 - 1.12 Write down a set of quantum numbers that...Ch. 1 - Do the three 4p atomic orbitals possess the same...Ch. 1 - How many radial nodes does each of the following...Ch. 1 - 1.15 Comment on the differences between plots of...Ch. 1 - 1.16 Write down the sets of quantum numbers that...Ch. 1 - Write down the three sets of quantum numbers that...Ch. 1 - How many atomic orbitals make up the set with n=4...Ch. 1 - Prob. 19PCh. 1 - (a) Will a plot of R(r) for the 1s atomic orbital...Ch. 1 - Prob. 21PCh. 1 - Prob. 22PCh. 1 - Write down the six sets of quantum numbers that...Ch. 1 - For a neutral atom, X, the following atomic...Ch. 1 - Using the concepts of shielding and penetration,...Ch. 1 - For each of the following atoms, write down a...Ch. 1 - 1.27 Draw energy level diagrams (see Fig. 1.15) to...Ch. 1 - 1.28 Write down the ground state electronic...Ch. 1 - Write down (with reasoning) the ground state...Ch. 1 - Draw energy level diagrams to show the ground...Ch. 1 - The ground state electronic configuration of a...Ch. 1 - (a) Write down an equation that defines the...Ch. 1 - 1.33 The first four ionization energies of an atom...Ch. 1 - 1.34 In Fig. 1.16, identify the trend in the first...Ch. 1 - 1.35 Figure 1.17 shows the values of for the...Ch. 1 - Using the data in Table 1.5, determine a value for...Ch. 1 - Prob. 37PCh. 1 - What is the evidence that the aufbau principle is...Ch. 1 - The first list in the table on the left contains...Ch. 1 - Prob. 40PCh. 1 - Using data from appendix 8, construct a graph to...Ch. 1 - The sign convention for electron affinity can...Ch. 1 - Prob. 43PCh. 1 - 1.45 Figure 1.18 shows the emission spectrum of...
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- When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.arrow_forwardQ6: Using acetic acid as the acid, write the balanced chemical equation for the protonation of the two bases shown (on the -NH2). Include curved arrows to show the mechanism. O₂N- O₂N. -NH2 -NH2 a) Which of the two Bronsted bases above is the stronger base? Why? b) Identify the conjugate acids and conjugate bases for the reactants. c) Identify the Lewis acids and bases in the reactions.arrow_forwardQ5: For the two reactions below: a) Use curved electron-pushing arrows to show the mechanism for the reaction in the forward direction. Redraw the compounds to explicitly illustrate all bonds that are broken and all bonds that are formed. b) Label Bronsted acids and bases in the left side of the reactions. c) For reaction A, which anionic species is the weakest base? Which neutral compound is the stronger acid? Is the forward or reverse reaction favored? d) Label Lewis acids and bases, nucleophiles and electrophiles in the left side of the reactions. A. 용 CH3OH я хон CH3O OH B. HBr CH3ONa NaBr CH3OHarrow_forward
- potential energy Br b) Translate the Newman projection below to its wedge-and-dash drawing. F H. OH CH3 CI c) Isopentane (2-methylbutane) is a compound containing a branched carbon chain. Draw a Newman projection of six conformations about the C2-C3 bond of isopentane. On the curve of potential energy versus angle of internal rotation for isopentane, label each energy maximum and minimum with one of the conformations. 0° 。 F A B D C angle of internal rotation E F 360° (=0°) JDownlarrow_forwardQ7: Identify the functional groups in these molecules a) CH 3 b) Aspirin: HO 'N' Capsaicin HO O CH3 CH 3arrow_forwardQ2: Name the following alkanesarrow_forward
- 1. Complete the following table in your laboratory notebook. Substance Formula Methanol CH3OH Ethanol C2H5OH 1-Propanol C3H7OH 1-Butanol C4H9OH Pentane C5H12 Hexane C6H14 Water H₂O Acetone C3H60 Structural Formula Molecular Weight (g/mol) Hydrogen Bond (Yes or No)arrow_forwardQ1: Compare the relative acidity in each pair of compounds. Briefly explain. (a) CH3OH vs NH 3 (b) HF vs CH3COOH (c) NH3 vs CH4 (d) HCI vs HI (e) CH3COOH vs CH3SH (f) H₂C=CH2 vs CH3 CH3 (g) compare the acidity of the two bolded hydrogens O. H N- (h) compare the acidity of the two bolded hydrogens, draw resonance structures to explain H H Harrow_forwardQ3: Rank the following molecules in order of decreasing boiling point: (a) 3-methylheptane; (b) octane; (c) 2,4-dimethylhexane; (d) 2,2,4-trimethylpentane.arrow_forward
- Q5: Conformations of Alkanes a) Draw a Newman Projection of the compound below about the C2-C3 bond. H3C Cli... H IIIH Br CH3arrow_forwardThe ability of atoms to associate with each other depends ona) the electronic structure and its spatial orientation.b) the electron affinity.c) The other two answers are correct.arrow_forwardWhat is the final volume after you reach the final temperature? I put 1.73 but the answer is wrong not sure why The initial volume of gas is 1.60 LL , the initial temperature of the gas is 23.0 °C°C , and the system is in equilibrium with an external pressure of 1.2 bar (given by the sum of a 1 bar atmospheric pressure and a 0.2 bar pressure due to a brick that rests on top of the piston). Then, as you did in Exercise 1, you heat the gas slowly until the temperature reaches 48.2 °Carrow_forward
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