I crushed acetamide and heated until melted, i let it cool and started again.

A. Describe your results for the melting point of acetamide. Were your results consistent? What was the range of values?

B. The published melting point of acetamide is 81°C, calculate the percent error between your experimental values and the published (theoretical) value. Show your work.

C. Describe what occurs to the particles of a substance when the substance melts. Explain why this occurs.

D. When performing this experiment, when is the acetamide in a condensed phase? Explain your answer.

E. Based on your observations of acetamide when it reformed a solid after melting, does acetamide form a crystalline or amorphous solid? Explain the difference between these two terms as part of your answer.

F. Give some examples of how it might be useful to know the melting or boiling points of a substance. Think in terms of both scientific and commercial/industrial settings.

G. Describe any possible sources of error for this exercise.

Calculate the pH change when a) 100 mL of 0.0500M NaOH and b) 100 mL of 0.0500 M HCL are added to a 400.0 mL of a solution that contains .300 M ammonium chloride and .300 M ammonia (Kb,= 1.76 x 10^-5) Show work to get a good rating please

The full three-dimensional Schrödinger equation is

−ℏ22m(∂2∂x2ψ(x,y,z)+∂2∂y2ψ(x,y,z)+∂2∂z2ψ(x,y,z))+U(x,y,z)ψ(x,y,z)=Eψ(x,y,z).

By using the substitutions from the introduction, this becomes

−ℏ22m(∂2∂x2ψxψyψz+∂2∂y2ψxψyψz+∂2∂z2ψxψyψz)+(Ux+Uy+Uz)ψxψyψz=Eψxψyψz

What is ∂2∂x2ψxψyψz? To make entering the expression easier, use D2x in place of d2ψxdx2, D2y in place of d2ψydy2, and D2z in place of d2ψzdz2.

Answer in terms of ψx,ψy,ψz,D2x,D2y,andD2z

The Arrhenius equation shows the relationship between the rate constant k and the temperature T in kelvins and is typically written as

k=Ae−Ea/RT

where R is the gas constant (8.314 J/mol⋅K), A is a constant called the frequency factor, and Eais the activation energy for the reaction.

However, a more practical form of this equation is

lnk2k1=EaR(1T1−1T2)

which is mathmatically equivalent to

lnk1k2=EaR(1T2−1T1)

where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures (T1 and T2).

Part A

The activation energy of a certain reaction is 46.7 kJ/mol . At 26  ∘C , the rate constant is 0.0120s−1. At what temperature in degrees Celsius would this reaction go twice as fast?

Express your answer with the appropriate units.

Part B

Given that the initial rate constant is 0.0120s−1 at an initial temperature of 26  ∘C , what would the rate constant be at a temperature of 180  ∘C for the same reaction described in Part A?

Express your answer with the appropriate units.

PLEASE explain Spectrophotometry and what is soo important about 400nm

PLEASE explain how absorbance and beer's law relate

Relate Beer’s law to the equation of a line on a standard curve.

Why is the line forced through zero on the standard curve?

What does the R2 value for the graph says about the experiment?

Suppose 8.00 g of calcium chloride are mixed with 6.00 g potassium hydroxide. What is in the container after the reaction?

The answer is below but please explain how to solve this problem.

Answer: no potassium hydroxide left; 2.86 g calcium chloride left; 3.96 g calcium hydroxide and 7.98 g potassium chloride

For Gorilla glass, Xensation, Sapphire glass, and Dragontrail glass, how they are made and processed, their hardness, strength, and cost. In metric please.

Mass of metal slug (measure once and use for both runs) 49.614 g 54.687 g Mass of water in calorimeter cup 80.113 g 80.087 g Initial temperature of water in the calorimeter 22.0 ºC 22.0ºC Initial temperature of the metal (assume 100.0 ºC) ____________ºC _____________ºC Equilibrium temperature of the metal + water 26.8 ºC 26.6ºC in the calorimeter ΔTwater ____________ºC ____________ºC ΔTmetal ____________ºC _____________ºC qwater * (S.H.C.water = 4.184 J/ g °C ) ____________J _____________J qmetal ** ____________J _____________J Calculated specific heat capacity of the metal ____________ J /g°C ____________ J /g°C B. Enthalpy of Reaction (Dissolution) CaCl2 NH4NO3 Mass of water in calorimeter cup 100.00 g 100.00g Mass of solid compound used 10.026 g 10.041g Mass of solution formed ____________g _____________g Initial temperature of water 22.0ºC 22.0ºC Max (if it rises) or min (if it falls) temperature of solution 38.2ºC 15.1ºC ΔTsoln (use initial temp. of water for initial temp. of soln.) ____________ºC _____________ºC qsoln (assume S.H.Cof soln. = S.H.C. of water) ____________J _____________J qreaction (amount of heat absorbed by the reaction)* ____________J _____________J “Heat of solution” ** ____________J/g _____________J/g ΔrH *** ____________kJ/mol_____________kJ/mol Is the dissolution reaction exothermic or endothermic? ____________ _____________ Enthalpy of Reaction (Neutralization) Initial temperature of HCl solution 22.0ºC Initial temperature of NaOH solution 23.2ºC Final temperature of neutralized mixture 29.4ºC ΔT (for the initial temperature, average the initial temperatures of the HCl and NaOH) ____________ºC qsoln (assume all the heat is absorbed by 104 g soln.) ____________J qrxn for the neutralization reaction ____________J Number of moles of H2O formed by the reaction ____________mol ΔHr (in kJ per mole of H2O formed by the reaction) ____________kJ/mol Is the neutralization reaction exothermic or endothermic? _____________

1) How many photons are emitted during a transition from a higher level orbit to a lower level orbit? a)1 b)2 c)3 d)4

2) True/False? An electron can transition from any allowed orbit to any other allowed orbit.

3) What is the wavelength of light emitted when an electron drops from the 3 to the 2 shell in a hydrogen atom?

1) Complete and balance the following half-reaction: H2SO3(aq)?SO2?4(aq) (acidic solution)

2)Complete and balance the following half-reaction:

NO?3(aq)?NO(g)(acidic solution)

3)Complete and balance the following half-reaction:

O2(g)?H2O(l)(acidic solution)

4)Complete and balance the following half-reaction:

O2(g)?H2O(l) (basic solution)

5)Complete and balance the following half-reaction: Mn2+(aq)?MnO2(s) (basic solution)

6)Complete and balance the following half-reaction: Cr(OH)3(s)?CrO2?4(aq) (basic solution)

When the following equation is balanced with the smallest integral coefficients, the coefficient of the HCl(g) is ______.
H₂O(l) + SO₂Cl₂(l) → HCl(g) + SO₃(g)

Given the reaction: 2 Al (s) + 6 HNO₃ (aq) ® 2 Al(NO₃)₃ (aq) + 3 H₂ (g) .. When 0.143 g of Al were added to 200 mL of 0.500 M HNO₃, 0.00842 g of H2 were produced. Find the percent yield of H₂.

(Please don’t forget to calculate the theoretical yield of hydrogen from both the aluminum and the nitric acid.)

A metal salt with the formula MCl2 crystallizes from water to form a solid with the composition MCl2⋅6H2O. The equilibrium vapor pressure of water above this solid at 298 K is 22.0 mbar .

What is the value of ΔrG for the reaction MCl2⋅6H2O(s)⇌MCl2(s)+6H2O(g) when the pressure of water vapour is 22.0 mbar ?

What is the value of ΔrG ∘ when the pressure of water vapour is 1 bar?

A buffer is prepared by mixing 25.0 mL of 0.500 M NH₃(aq) with 25.0 mL of 0.200 M HCl (aq). What is the pH of the buffer? [ K_b (NH₃) = 1.8 x 10^-5 ]