How much heat energy is required to convert 53.0 g of solid ethanol at -114.5 °C to gasesous ethanol at 141.8 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous ethanol is 1.43 J/g·°C.

The rate constant of the elementary reaction 2HI(g) H2(g) +I2(g) is k = 1.97 L mol-1 s-1 at 604°C, and the reaction has an activation energy of 206 kJ mol-1.

(a) Compute the rate constant of the reaction at a temperature of 767°C. L mol-1 s-1

(b) At a temperature of 604°C, 177 s is required for half of the HI originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 767°C?

Calculate the freezing point and boiling point of a solution containing 7.90 g g of ethylene glycol (C2H6O2) in 92.7 mL of ethanol. Ethanol has a density of 0.789 g/cm3

Calculate the freezing point of the solution.Express the answer using four significant figures.

Calculate the boiling point of the solution.Calculate your answer using three significant figures.

if 92.8 grams of sodium nitrite are dissolved in 2.3L of water, the resulting solution has a molarity of

1. The experimental empirical formula of a magnesium oxide compound was determined. To do this a magnesium ribbon weighing 0.252 g was heated in a crucible. From the data listed, determine the empirical formula for the magnesium oxide product. Please show all work! I'm trying to really understand

          Mass of empty crucible and cover: 20.74 g

          Mass of crucible, cover, and final product: 21.17 g

Hand draw the following transformations step by step, including all intermediates. Ideally, also show electron pushing

A. Conversion of asparagine to aspartic and isoaspartic acid in peptides.
B. Conversion of aspartic acid to isoaspartic acid in peptides.
C. Cleavage of the peptide backbone at the aspartic acid residue.
D. Discuss whether acid may catalyze each reaction (A, B or C); i.e., whether the reaction is faster at (pH lower than 7) than at pH 7.

E. Discuss whether base may catalyze each reaction (A, B or C); i.e., whether the reaction is faster at (pH higher than 7) than at pH 7.

1.) The cell reactions occurring in a battery are given by:

Cathode : 2MnO2 (s) + H2O (l) + 2e-→ Mn2O3 (s) + 2HO- (aq) E 0 red = +0.15 V

Anode : Zn (s) + 2HO- (aq) → Zn(OH)2 (s) + 2e- E 0 red = -1.25 V

a) What is the overall cell potential? What is the free energy change for this process?

b) During the discharge of the battery, 2.00 g of Mn2O3 is produced at the cathode. How many grams of Zn were consumed?

c) Consider this half reaction: Cd(OH)2 + 2e- → Cd(s) + 2HO- (aq) E°red = -0.76V What is the overall cell potential and free energy change of the battery described above if the Zn anode is replaced by Cd?

2.) Ca(s) can be obtained by electrolysis of molten CaCl2. What amperage is needed to produce 10.00 g of Ca(s) in a period of 1h assuming that the process is 100% efficient?

The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl₃) and chlorine:
1) Cl₂ ⇔ 2 Cl (fast, reversible)
2) Cl + CHCl₃ → HCl + CCl₃ (slow)
3) Cl + CCl₃ → CCl₄ (fast)
What rate law does this mechanism predict? Choose from the list below and enter the letters for all the terms needed in the rate law. (So for a rate law of k[Cl₂] enter AC, and for a rate law of k[Cl₂][CHCl₃] enter ACE.)

Calculate how many milligrams of the drug are contained in 2.0mL of a 3.0% (w/v) solution ofC₁₇H₁₉N₃O₃S

which one of the following molecules is polar?
a. CS2, b. SO2 c. XeF2 d.XeF4, e. SO3

Consider the titration of a 26.0?mL sample of 0.175M CH3NH2 with 0.155M HBr . Determine each of the following.

A. the initial pH

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

C.the pH at 5.0mL of added acid

D. the pH at 1/2 equivalence point

E. the pH at equivalence point

F.the pH after adding 4.0mL of acid beyond the equivalence point

Any help is appreciated!!! I'm just so lost with this one.

1. Moles

            a. Which has more mass, 1 g of C or 1 g of Pb?

            b. Which has more mass, I mole of C or 1 mole of Pb?

            c. How much mass does a mole of C have, and where do you find this information?

            d. How much mass does a mole of Pb have?

            e. How many atoms does a mole of C have?

            f. How many atoms does a mole of Pb have?

            g. Does a mole of any element have more atoms than a mole of another element?

            h. If a mole of C has the same number of atoms as a mole of Pb, why is a mole of Pb so much heavier than a mole of C?

i. How many molecules of CH₄ are in a mole of CH₄?

j. What is the mass of a mole of CH₄?

k. How many H atoms are in 1 molecule of CH₄?

l. How many moles of H atoms are in 1 mole of CH₄?

Given the data tables below for the concentrations of crystal violet dye in the crystal violet-hydroxide reaction CV⁺ + NaOH^- --> CVOH + Na, calculate the order of hydroxide if the order of crystal violet is first order (ln[A] shows a linear relationship for CV).

CV⁺ + OH^- --> CVOH

Data