1.What mode of decay is probable for 41/18 Ar ? What mode of decay is probable for ? a.electron capture b. beta emission C.positron emission D.alpha emission

2.

The standard cell potential, E°_cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Calculate the standard free energy change, ΔG°, in kJ for this reaction and determine if it is spontaneous or nonspontaneous at 25°C.

A.−2.57 × 10² kJ, nonspontaneous B. −2.57 × 10² kJ, spontaneous C. −1.28 × 10² kJ, spontaneous D. +2.57 × 10² kJ, nonspontaneous

3. List the given metal ions in order of increasing strength as oxidizing agents, based on the following standard reduction potentials, E°_red .

How much heat (in kJ) is required to warm 13.0 g of ice, initially at -13.0 ∘C, to steam at 114.0 ∘C? The heat capacity of ice is 2.09 J/g⋅∘C and that of steam is 2.01 J/g⋅∘C.

Calculate the pH of an aqueous solution of 0.225 M salicylic acid, which has a Ka =1.0 x 10^-3

An explanation will be appreciated, a simple answer won't really help. Thank you!

Write equations for the reactions investigated. Label Sn1 or Sn2.

1)Butyl bromide in 15%NaI-acetone

2)Butyl bromide in 1%ethanolic silver nitrate

?????3)Butyl chloride in 15% NaI-acetone

4) Butyl chloride in 1% ethanolic silver nitrate

5)Sec-butyl chloride in 15%NaI-acetone

6) Sec-butyl chloride in 1% ethanolic silver nitrate

7) Tert-butyl chloride in 15%NaI-acetone

8) Tert-butyl chloride in 1% ethanolic silver nitrate

9) Crotyl chloride in 15% NaI-acetone

10) Crotyl chloride in 1% ethanolic silver nitrate

Any help would be appreciated! I will rate your response in return!

Consider the titration of a 25.0 −mL sample of 0.180 M CH3NH2 with 0.155 M HBr. Determine each of the following.

A. initial pH

B. volume of added acid required to reach the equivalence point

C. pH at 6.0 mL of added acid

D. pH at one-half of the equivalence point

E. pH at the equivalence point

F. pH after adding 6.0 mL of acid beyond the equivalence point

What is the pH at the equivalence point when 25.00 mL of a 0.150 M solution of acetic acid (CH3COOH) is titrated with 0.10 M NaOH to its end point?

1. household vinegar is 5% of acetic acid. give the formula for acetic acid. show work please!e

2. how could you distinguish solid barium chloride from solid barium sulfat?

do you think washing soda Na2CO3, could be used for the same purpose as baking soda NaHCO3? would Na2CO3 react with HCl ? write the chemocal equation. write the chemical equation for the reaction of NaHCO3 with HCl.

Post-Lab Questions

Which data point can you obtain with greater accuracy from your graph-the pK values from the "legs" or the isoelectric point from the point of inflection? Explain your answer.

Now that we know it os first order

What is the value of the rate constant for this reaction?

Q1, The total entropy change of a system and its surrounding is (a) in a(n) (b) process.

1. (a) larger than zero; (b) reversible
2. (a) smaller than zero; (b) reversible
3. (a) equal to zero; (b) reversible
4. (a) equal to zero; (b) irreversible
5. (a) smaller than zero; (b) irreversible

Q2, Standard enthalpy change (ΔH°) of a process involving gases is the enthalpy change of process at

1. 1 atm and 298K.
2. 1 atm and 273K.
3. 273K.
4. 1 atm.
5. 298K.

Q3, The following values are noticed on the phase diagram of CO2: at its triple point:
T3 =216.8 K and P3 =5.11 atm; at its critical point: Tc =304.2 K and Pc =72.9 atm.

Which of the statements below about CO2 is correct?

1. CO2 can exist as liquid at atmospheric pressure if it is brought to a temperature low enough.
2. CO2 cannot exist in liquid phase at atmospheric pressure.

3. CO2 cannot exist as solid if its temperature is higher than its triple point temperature T3.
4. CO2 is said to be in supercritical condition if it is brought to a temperature higher than 304.2 K at atmospheric pressure
5. CO2 cannot exist as vapour if its temperature is brought to lower than its triple point temperature 216.8K.

Q4, For a pure substance:

1. its Gibbs energy always increases with the pressure at constant temperature.
2. its Gibbs energy always increases with the temperature at constant pressure.
3. its Gibbs energy always increases when the substance changes from solid to liquid or from liquid to vapour.
4. its Gibbs energy always decreases when the substance changes from vapour to liquid or from liquid to solid.
5. its Gibbs energy remains unchanged in a reversible phase change process.

MgSO4•7H2O is an example of hydrate, a substance that has fixed mass percent of water in the compound. Calculate the mass percent (%) composition of water in MgSO4•7H2O. (show your work.)

You are a studen in Organic Chemsitry lab and you are tasked with the job to make 202 ppm solution of Rhodamine B (MM = 479.02 g/mol). How many moles of dye do you need to add to a 250 mL beaker of water to prepare this solution?

The automobile fuel called E85 consists of 85 % ethanol and 15 % gasoline. E85 can be used in so-called "flex-fuel" vehicles (FFVs), which can use gasoline, ethanol, or a mix as fuels. Assume that gasoline consists of a mixture of octanes (different isomers of C8H18), that the average heat of combustion of C8H18(l) is 5400 kJ/mol, and that gasoline has an average density of 0.70 g/mL. The density of ethanol is 0.79 g/mL.

For Part A, start with the given L of gasoline and use the density of the gasoline as well as the molar mass of  C8H18 to determine the moles of gasoline. Once you have found the moles of gasoline you will use the provided heat of combustion to determine the energy produced. You do not need to use Appendix C because you are using the provided heat of combustion.

For Part B, do the same with the ethanol. You will use the heat of combustion for ethanol from the extra credit homework problem 5.79. If you did not do the that homework problem, you will need to write the balanced equation for the combustion of ethanol paying attention to the phases. Use the phase of gas for the water. Then calculate the heat of the combustion reaction from the heats of formation in Table C.

For Part C, you will need to use a weighted average. This is the same formula we used to determine the average atomic mass.

For Part D, you are starting with the given gallons of gasoline and will need to use the heat of combustion produced for the given liters of gasoline as a conversion factor to determine the energy produced from the given gallons. The heat of combustion produced from the liters of gasoline is from Part A. Now take the energy produced from the gallons of gas and use that as the given. Using the heat of combustion produced for the liters of E85 from Part C, determine the gallons of E85 necessary to produce that much energy.

For Part E, you will use the gallons of gasoline

A)By using the information given as well as data in Appendix C, calculate the energy produced by combustion of 2.0 L of gasoline

B)By using the information given as well as data in Appendix C, compare the energy produced by combustion of 2.0 L of ethanol. Consider that water is in the gaseous state.

c)Assume that the density and heat of combustion of E85 can be obtained by using 85 % of the values for ethanol and 15 % of the values for gasoline. How much energy could be released by the combustion of 2.0 L of E85?

E)If gasoline costs $ 3.10 per gallon in the United States, what is the break-even price per gallon of E85 if the same amount of energy is to be delivered?

A solution containing 28.60 mg of an unknown protein per 29.0 mL solution was found to have an osmotic pressure of 3.80 torr at 15 ∘C. What is the molar mass of the protein?

Please show details on how to get to the answer: