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12 Dec 2019

Part B

Sometimes, however, proteins denature as temperature is decreased. How might this be explained?

Check all that apply.

In cases of cold denaturation, the sign on ÎS is dominated by the hydrophobic effect and is therefore positive.

In these cases, ÎH must be negative for the process to become favorable as temperature decreases.

In cases of cold denaturation, the sign on ÎS is dominated by the hydrophobic effect and is therefore negative.

In these cases, ÎH must be positive for the process to become favorable as temperature decreases.

Clathrate cage formation would account for the sign of ÎH being negative (favorable) for cold denaturation.

Clathrate cage formation would account for the sign of ÎH being positive (favorable) for cold denaturation.

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Trinidad TremblayLv2

13 Dec 2019

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Related questions

Show your work for all calculations.

1. When 1.104 grams of iron metal are mixed with 26.023 grams of hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2 Â°C to a maximum of 33.5 Â°C. The reaction that occurs is given below.

2Fe(s)+6HCl(aq) â 2FeCl3 (aq)+3H2 (g)

a) Determine the amount of heat (in J) absorbed by the reaction mixture. Assume that the specific heat capacity of the mixture is the same as the specific heat capacity of water.

b) How much heat (in J) was released by the reaction that occurred?

c) Is this reaction exothermic or endothermic? Is ÎHreaction positive or negative?

d) Under constant pressure conditions (as used in this experiment), the heat released by the reaction equals the reaction enthalpy, qreleased = ÎHreaction. Determine ÎHreaction in Joules per gram of metal used (J/g).

e) Determine ÎHreaction in kilojoules per mole of metal used (kJ/mol).

f) Determine ÎHreaction in kilojoules per mole for the balanced reaction equation provided (kJ/mol). ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼

2. Consider the following three reactions:

2Fe(s)+6HCl(aq) â 2FeCl3 (aq)+3H2 (g) ÎHA

Fe2O3 (s)+6HCl(aq) â 2FeCl3 (aq)+3H2O(l) ÎHB

2H2 (g) + O2 (g) â 2H2O(l) ÎHC

Show how these equations must be summed together according to Hessâs Law to determine ÎH for the combustion of iron (target equation shown below). Also show clearly how the ÎH values of each of the three reactions must be manipulated to determine the enthalpy of combustion of iron.

4Fe(s)+3O2 (g) â 2Fe2O3 (s) ÎH=?

3. Using tabulated ÎHfÂ° values in the text, determine the enthalpy change (in kJ/mol) that occurs during the formation of water from its elements as described by the equation:

2H2 (g) + O2 (g) â 2H2O(l) ÎH=?

1) The first-order rate constant for the reaction of methyl chloride (CH₃Cl) with water to produce methanol (CH₃OH) and hydrochloric acid (HCl) is 3.32 Ã10^â10 s^â1 at 25Â°C. Calculate the rate constant at 58.3Â°C if the activation energy is 116 kJ/mol.

(Enter your answer in scientific notation.)answer

2)Given the same reactant concentrations, the reaction

CO(g) + Cl₂(g) â COCl₂(g)at 259Â°C is 272 times as fast as the same reaction at 147Â°

C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.

kJ/mol answer

3)For a certain reaction, the frequency factor A is 7.5 Ã10⁹ s^â1 and the activation energy is 24.5 kJ/mol.

What is the rate constant for the reaction at 92Â°C

(Enter your answer in scientific notation.) answer

4)The rate constant of a first-order reaction is 3.25 Ã10^â4 s^â1 at 350.Â°C. If the activation energy is 107 kJ/mol,

calculate the temperature at which its rate constant is 9.85 Ã10^â4 s^â1.

5)The rate at which tree crickets chirp is 1.80 Ã10² per minute at 29Â°C but only 37.9 per minute at 6.5

Â°C. From these data, calculate the activation energy for the chirping process.

kJ/mol answer

6)Consider the following elementary step

X + 2Y âXY₂

If the initial rate of formation of XY₂ is 0.0076 M/s and the initial concentrations of X and Y are 0.38 Mand 0.64 M, what is the rate constant for the reaction?

M^â2s^{â1 answer}

⁷⁾The activation energy for the decomposition of hydrogen peroxide is 59.0 kJ/mol. When the reaction is catalyzed by the enzyme catalase, it is 6.00 kJ/mol.

2H₂O₂(aq) â2H₂O(l) + O₂(g)

Calculate the temperature that would cause the nonenzymatic catalysis to proceed as rapidly as the enzyme-catalyzed decomposition at 20.0Â°C. Assume the frequency factor, A, to be the same in both cases. Report your answer to 3 significant figures.

8)The activation energy (E_a) for the reaction

2N₂O(g) â 2N₂(g) + O₂(g) ÎH