Consider the reaction

C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l)

in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C. Calculate the change in internal energy, ΔE, for this reaction per mole of sucrose.

Express the change in internal energy in kilojoules per mole to three significant figures.

WORKSHEET 1- answers. i need explanation and wrok shown for each questions.

1) A 2) C 3) E 4) E 5) E 6) E 7) D 8) E 9) B 10) E 11) D 12) C 13) D 14) D 15) B 16) D

http://east.cherryhill.k12.nj.us/Summer_Assignments/pdfs/c01ws01.pdf

a) Magnesium metal reacts with HCl solution, liberating H₂ gas and generating Mg²⁺ cations in solution. A 2.780-g sample of Mg metal is added to 50.0 mL of a 4.00 M HCl solution, and the reaction goes to completion. What mass of H₂ is formed?

b) What is the concentration of Mg²⁺ ions in the resulting solution? (Assume the final volume of solution is still the same as the original volume of the acid.)

When Acetic acid (CH₃COOH) reacts with sodium bicarbonate a neutralization reaction occurs: [20 pts]

(a) Write the balanced chemical equation for this reaction.

(b) If you are given 1.26 x 10² g of acetic acid and 1.68 x 10² g of sodium bicarbonate, what reagent would be limiting?

(c) What would be the theoretical yield of the product(s)?

(d) How many grams of excess reagent would be left over?

(e) If the reaction yielded 68.46 g of the gas, 27.52 g of the liquid, and 159.6 g of the salt, what would their percent yields be?

On the basis of your research, respond to the following:

Why and how does atomic nuclear decay take place? Explain.

What is the significance of atomic nuclear decay?

What is your analysis on the societal implications of using this process?

What is the purpose of sodium hydrosulfite addition? What is the purpose of potassium ferricyanide in the conversion of luminol to an excited state?

Calculate ?H (298 K) per gram of fuel units of kJ*g^-1 (exclude oxygen)

a.) H2(g) + 1/2 O2(g) = H2O(g)

b.) CH4(g) + 2O2(g) = CO2(g) + 2H2O(g)

c.) CH3OH(l) + 3/2 O2(g) = CO2(g) + 2H2O(g)

d.) C6H14(g) + 9 1/2 O2(g) = 6CO2(g) + 7H2O(g)

A buffer contains 1.0 mol of CH3CO2H and 1.0 mol of CH3CO2- diluted with water to 1,0 L. How many moles of NaOH are required to increase the pH of the buffer to 5.10? pKa of CH2CO2H is 4.74

Can someone explain this step by step please!

Consider the distillation of ethanol (C2H5OH) and the combustion of ethanol . Use a bullet point list to compare and contrast the 2 processes. There should be at least 5 points of comparison

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.011 M in NH4Cl at 25 °C?

Calculate the pH of a 0.19 M CH₃COOLi solution. (K_a for acetic acid = 1.8 × 10⁻⁵.)

Rank the following compounds in order of increasing strength of intermolecular attractions: H2O2, CF4, KF, and CHCl3

You have a 5 mL sample of a protein in 0.5 M NaCl. You place the protein/salt sample inside dialysis tubing (see below) and place the bag in a large beaker of distilled water. If your goal is to remove as much NaCl from the sample as possible, which would be more effective: (1) placing the dialysis bag in 4 L of distilled water for 12 h, or (2) placing the bag in 1 L of distilled water for 6 h and then in another 1 L of fresh distilled water for another 6 h? EXPLAIN

For each of the following solutions, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

b. For 210.0mL of a buffer solution that is 0.210M in HCHO2 and 0.295M in KCHO2, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

c. For 210.0mL of a buffer solution that is 0.265M in CH3CH2NH2 and 0.240M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.