An athlete is given 100 g of Glucose (C_6 H_12 O_6) of energy equivalent to 1560 kJ. He utilises 50 % of this gained energy in the event. In order to avoid storage of energy in the body, calculate the mass of water he would need to perspire. The enthalpy of evaporation of water is 44 kJ/mole.
Calculate "delta" S for the following reaction: H2(g) + Br2(l) --> 2HBr(g) given: S[H2(g)] = 0.131 kJ/K S[Br2(l)] = 0.152 kJ/K S[HBr(g)] = 0.199kJ/K a. 0.482 kJ/K b. 0.681 kJ/K c. 0.115 kJ/K d. -0.084 kJ/K e. 0.084 kJ/K
What is the relationship between 'delta' G and E (cell voltage)? 'delta' G = ?
Multiple choice question about the affect on Standard Gibbs free energy when the reactant or product pressure is increased.
In a gas phase reaction, what is the effect of increasing reactant or product pressure on the standard Gibbs free energy? a. Delta G increases due to decreased entropy b. Delta G decreases due to decreased entropy c. Delta G increases due to increased enthalpy d. Delta G may either increase or decrease e. De
If delta G is negative at all temperatures, then which of the following statements must be true? a. Delta H > 0 and delta S > 0 b. Delta H > 0 and delta S < 0 c. Delta H < 0 and delta S > 0 d. Delta H < 0 and delta S < 0 e. None of the above
Predict the signs of delta S and delta H for the melting of ice at 300K? a. Delta H > 0 and delta S > 0 b. Delta H > 0 and delta S < 0 c. Delta H < 0 and delta S > 0 d. Delta H < 0 and delta S < 0 e. Not enough information provided to answer question
Calculate "delta" S for the following reaction: H2(g) + Br2(l) --> 2HBr(g) Given: S[H2(g)] = 0.131 kJ/K S[Br2(l)] = 0.152 kJ/K S[HBr(g)] = 0.199kJ/K a. 0.482 kJ/K b. 0.681 kJ/K c. 0.115 kJ/K d. -0.084 kJ/K e. 0.084 kJ/K
Which of the following are conditions for the standard Gibbs free energy? a. Ions or molecules in solution are present at one molar concentrations b. the temperature of the system is at 298K c. gases are present at one atmosphere partial pressure d. answers a and c are correct e. answers a, b, and c are corre
Which of the following is true for the combustion of hydrogen gas? a. "change in" H > 0 b. "change in" H < 0 c. "change in" S > 0 d. "change in" G > 0 at 300K e. "change in" G > 0 at all temperatures
Which of the following is true for the freezing of water at 298K? a. "change in" H < 0 b. "change in" H > 0 c. "change in" S = 0 d. "change in" S > 0 e. both answers a and d are correct
Which of these statements is false? a. For a given material, a gas would have a greater entropy than the solid. b. For a given material, a liquid would have a greater entropy than the gas. c. At 0 K, an ordered pure crystalline solid has an entropy of zero. d. For a given material, the liquid has a greater entropy than the
If "change in" G > 0, then a. K=0 b. K>0 c. K<0 d. K>1 e. K<1
The change in G and the change in H are equal: a. At O degrees Cesius b. At O degrees K c. When concentrations equal 1M and partal pressure equal 1 atm d. When all reactants and products are in the same phase e. When the reaction is exothermic
Which of the following reactions is likely to have the most positive change in entropy? a. N2(g)+3H2-->2NH3(g) b. CaO(s)+CO2--->CaCO3(s) c. N2(g)+2O2(g)-->2NO2(g) d. C(s)+)O2(g)-->CO2(g) e. 2C(s)+O2(g)-->2CO(g)
Which of the following has the least entropy? a. H20(s) b. H20(l) c. H20(g) d. Answers a and b have the same entropy e. Answers a, b, and c have the same entropy
Understanding "equation of state" (ie. PV=nRT) for an ideal gas, and using equation of state to predict changes in pressure, volume, and temperature.
In an industrial process, nitrogen has to be heated to 500 K in a vessel of constant volume. If it enters the vessel at a pressure of 100 atm and a temperature of 300 K, what pressure does it exert at the working temperature?
Working with heats of formation to calculate the amount of grams required to release a specific amount of heat.
Glucose reacts with oxygen to form carbon dioxide and water: If the heat of formation of glucose, carbon dioxide, and water are -1273.3 kJ mol-1, -393.5 kJ mol-1 and -285.8kJ mol-1. How many grams of glucose must react in order to release (1.00)(10^3)kJ of heat?
Calculate the bond energy of the reaction: 2 H2 + O2 ---> 2 H2O
The reaction of 4.49 g of carbon and 9.21 g of oxygen, produced carbon dioxide, and 113.2 kJ of heat. What is the enthalpy of formation of carbon dioxide?
Find the work done, w, when a system absorbs 104 J of heat and its internal energy decreases by 55 J.
Copper has a specific heat of 0.382 J g-1 degrees Celsius -1. The temperature of an unknown mass of copper increases by 4.50 degrees Celsius when it absorbs 3.97 J of heat. What is the mass of copper?
What mass of water rises by 15 degrees Celsius when it absorbs 2646 Joules?
Delta G sub f for Al203 = -1582 kJ/mol delta H sub f for Al203 = -1676 kJ/mol 1. Calculate absolue entropy for S for oxygen (g) if: S for Al(s) = 164 J/mol K S for Al2O3 (s) = 51.0 J/mol K 2. Calculate the heat required to raise the temperature of 35.0 g of aluminum from 800 degrees C to 2600 degrees C 3. To c
Chemistry review problems, please see the attachment.
When calculating the amount of heat emitted (q): In which of these situations should you add the weight of what is added to the water, to the weight of the water itself? - 17g stick of boiled metal added to water in a calorimeter. or - 2g of NaOH added to water to measure the heat of dissolving.
I'm having problems understanding the ideas in the topic of thermal chemistry and would appreciate any sort of overview of the main concepts you could provide.
If you boil water are you increasing delta H (heat), delta E (energy), or delta S (entropy)?
Liquid methanol has a heat capacity of 81.6 J/(K mol). How much heat is required to raise the temperature of 20.0 g of liquid methanol from 25 C to 40.0 C?
Considering the Reaction: 2H2O(l) => 2H2(g) + O2 (g) This reaction has dispersal of matter since a liquid produces two gases, yet the reaction is not spontaneous. Why is this so?
Understanding how the equilibrium constant (Keq) relates to enthalpy change. Introductory thermodynamics. Attachment in Word.
Which reaction is more exothermic? A reaction with Keq=500 or a reaction with Keq=0.002?