FUND.OF GEN CHEM CHAP 1-13 W/ACCESS
16th Edition
ISBN: 9781323406038
Author: McMurry
Publisher: PEARSON C
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Chapter 7, Problem 7.31AP
Interpretation Introduction
Interpretation:
The process where the entropy of the given system increases among the given options has to be determined.
Concept Introduction:
Entropy
If the disorder increases in a system, then
If the disorder decreases in a system, then
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Students have asked these similar questions
(A) how much energy is necessary to heat 7.0 kg of water from room temperature (20 degrees Celsius) to its boiling point? (Assume no energy loss)
(b) if electrical energy were used, how much would this cost at 45 cent per kWh?
Label the following statements true or false: (c) A nonspontaneous reaction will proceed spontaneously in the reverse direction. (d) A spontaneous process can occur with a large decrease in entropy.
(1) Label the following statements as true or false and
briefly explain your answer:
(a) A spontaneous process always happens very
quickly.
(b) A spontaneous process can occur with a large
decrease in entropy.
(2) Consider a reaction with DH
=
3.6 kcal/mole and
DS = 11.9 cal/(mol*K). Is the reaction spontaneous
(a) @ 10 °C and (b) @ 80 °C? Show your work.
(3) Calculate the DG for the reaction A + B
C+
D at 25 °C when the equilibrium concentrations are
[A] = 10 mM, [B] = 15 mM, [C] = 3 mM, and [D] = 5
mM. What is the DG for this reaction? Is the
reaction exergonic or endergonic under standard
conditions? Show your work.
(4) Using a chemical drawing program (e.g.
ChemSketch or Marvin Sketch), please illustrate an
example of 2 reducing and 2 non-reducing
sugars. Be sure to indicate the REDUCING END of
the 2 reducing sugars (NOTE: most programs
include templates with the hexoses and pentoses
pre-drawn, feel free to use these templates).
(5) There are several qualitative chemical tests…
Chapter 7 Solutions
FUND.OF GEN CHEM CHAP 1-13 W/ACCESS
Ch. 7.1 - Classify each of the following as having potential...Ch. 7.2 - Based on bond energies, which atmospheric gas in...Ch. 7.3 - Prob. 7.1CIAPCh. 7.3 - How many Calories (i.e., kilocalories) are in a...Ch. 7.3 - Prob. 7.3PCh. 7.3 - Prob. 7.4PCh. 7.3 - Prob. 7.5PCh. 7.3 - Prob. 7.6PCh. 7.4 - Prob. 7.7PCh. 7.4 - Prob. 7.8KCP
Ch. 7.5 - The reaction between iron and oxygen to form rust...Ch. 7.6 - Prob. 7.10PCh. 7.8 - Prob. 7.11PCh. 7.8 - Prob. 7.12PCh. 7.8 - Prob. 7.13PCh. 7.8 - The following diagrams represent two similar...Ch. 7.9 - Prob. 7.3CIAPCh. 7.9 - Prob. 7.4CIAPCh. 7.9 - Is the yield of SO3 at equilibrium favored by a...Ch. 7.9 - Prob. 7.16PCh. 7.9 - Prob. 7.17PCh. 7 - What are the signs of H, S, and G for the...Ch. 7 - Prob. 7.19UKCCh. 7 - Prob. 7.20UKCCh. 7 - Two curves are shown in the following energy...Ch. 7 - Prob. 7.22UKCCh. 7 - Prob. 7.23APCh. 7 - Prob. 7.24APCh. 7 - Prob. 7.25APCh. 7 - Prob. 7.26APCh. 7 - Acetylene (H C C H) is the fuel used in welding...Ch. 7 - Prob. 7.28APCh. 7 - Prob. 7.29APCh. 7 - Prob. 7.30APCh. 7 - Prob. 7.31APCh. 7 - Prob. 7.32APCh. 7 - Prob. 7.33APCh. 7 - Prob. 7.34APCh. 7 - Why are most spontaneous reactions exothermic?Ch. 7 - Prob. 7.36APCh. 7 - Prob. 7.37APCh. 7 - Prob. 7.38APCh. 7 - Prob. 7.39APCh. 7 - Prob. 7.40APCh. 7 - Prob. 7.41APCh. 7 - Prob. 7.42APCh. 7 - Prob. 7.43APCh. 7 - Prob. 7.44APCh. 7 - Prob. 7.45APCh. 7 - Prob. 7.46APCh. 7 - Prob. 7.47APCh. 7 - Prob. 7.48APCh. 7 - What is meant by the term chemical equilibrium?...Ch. 7 - Prob. 7.50APCh. 7 - Prob. 7.51APCh. 7 - Prob. 7.52APCh. 7 - Prob. 7.53APCh. 7 - Prob. 7.54APCh. 7 - Use your answer from Problem 7.53 to calculate the...Ch. 7 - Use your answer from Problem 7.54 to calculate the...Ch. 7 - Prob. 7.57APCh. 7 - Prob. 7.58APCh. 7 - Prob. 7.59APCh. 7 - Prob. 7.60APCh. 7 - Prob. 7.61APCh. 7 - Prob. 7.62APCh. 7 - Prob. 7.63APCh. 7 - Prob. 7.64APCh. 7 - Prob. 7.65APCh. 7 - Prob. 7.66APCh. 7 - For the unbalanced combustion reaction shown, 1...Ch. 7 - Prob. 7.68CPCh. 7 - Prob. 7.69CPCh. 7 - Prob. 7.70CPCh. 7 - Urea is a metabolic waste product that decomposes...Ch. 7 - Prob. 7.72CPCh. 7 - Prob. 7.73CPCh. 7 - Methanol, CH3OH, is used as race car fuel. (a)...Ch. 7 - Prob. 7.75CPCh. 7 - Prob. 7.76CPCh. 7 - Prob. 7.77CPCh. 7 - Prob. 7.78GPCh. 7 - Prob. 7.79GPCh. 7 - Prob. 7.80GP
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- Entropy increase A) with every reaction B) only in open systems C) only under certain reaction conditions D) only in the physical world. This cannot happen in cells otherwise cells would lose their needed energyarrow_forwardWhich of the following statements is true? (a) The largerthe Q, the larger the ΔG°. (b) If Q = 0, the system is at equilibrium.(c) If a reaction is spontaneous under standardconditions, it is spontaneous under all conditions. (d) Thefree-energy change for a reaction is independent of temperature.(e) If Q > 1, ΔG > ΔG°.arrow_forwardTell whether the entropy of the following reactions will be negative, positive or zero. b) NaNO3 + H2O -> Na^+ + NO3^- c) 4H + O2 <-> 2 H2O d) 4HO2 <-> 2H2O + O2 a) Solid Carbon Dioxide <-> Gas Carbon Dioxidearrow_forward
- endothermic reactions absorb energy from their surroundings. If chemicals for an endothermic reaction are added to water, the water's temperature drops (the water gets colder! Ever use a first aid "cold pack", where you squeeze a pouch to release chemicals inside and the pouch becomes ice cold? That's an endothermic reaction!) For endothermic reactions, when you use the equation Q = m x C x (delta T), the "Q" is a negative number because the water LOSES energy. The answer is negative because the water temperature drops, the CHANGE registered on the thermometer is negative. Type a negative number to answer this question: if your water starts at 19 degrees Celsius, and a couple of minutes after adding chemicals the water temperature becomes 15 degrees, the value of "delta T" is degrees Celsius. *arrow_forwardWhich of the following correctly explains why the vapor pressure of water has to be included in the calculations? Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater vapor has to be added to Pdry gas. Overview of the experiment:arrow_forward(i)Define initial velocity (ii) Describe how you would calculate initial velocity from a graph of product concentration against time for a chemical reactionarrow_forward
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- Define the following terms. (i) Rate constant (k) (ii) Activation energy (Ea)arrow_forwardLabel the following statements true or false: (a) A reaction is said to be spontaneous when it can proceed in either the forward or reverse direction. (b) A spontaneous process always happens very quickly.arrow_forwardThe enzyme E catalyzes the chemical reaction, X ⇌ Y. Imagine two different cases, a) initial concentration of X is low, and b) initial concentration of X is high. Now, if you start adding X, the initial velocity will increase until it reaches its maximum level. In which case, the initial velocity will increase linearly with an increase in the concentration of X? why?arrow_forward
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