Hi

I have HW and I need help, need full answers

QUESTION 1

1. Explain why exothermic processes tend to be spontaneous.

QUESTION 2

1. The volume of an ideal gas is decreased from 5.0 L to 6.4 mL at a constant pressure of 1.8 atm. Calculate the work associate with this process in J. Submit your answer with a scientific notation format and correct significant figures. For example, if your answer is 23456, you must submit your answer as 2.34e+4 for 3 significant figures.

QUESTION 3

1. Does the system of the previous question do work on the surroundings? Briefly explain.

QUESTION 4

1. Calculate ∆E for a system when q = –54 kJ and w = +87 kJ

QUESTION 5

1. Calculate ∆E when q = +16 kJ and w = –47 kJ.

QUESTION 6

1. Calculate ∆E when q = +75 kJ and w = 0 kJ

QUESTION 7

1. In which questions (4, 5, and/or 6) that surroundings do work on the system?

   	1.	Question 4
   	2.	Question 5
   	3.	Question 6

QUESTION 8

1. A system undergoes a process consisting of the following two steps:Step 1: the system absorbs 39 J of heat while 13 J of work is done on it.Step 2: the system absorbs 20 J of heat while performing 37 J or work.Calculate ∆E of the overall process.

QUESTION 9

1. A balloon filled with helium gas has a volume of 826 L at 1.00 atm pressure. The balloon absorbs 30.9 kJ of heat as it expands to a volume of 1,019 L. Calculate the internal energy in kJ for the helium in the balloon.

QUESTION 10

1. Suppose you place 0.0603 g of magnesium chips in a coffee cup calorimeter and then add 100.00 mL of 1.00 M HCl. The reaction that occurs is:Mg (s) + 2HCl (aq) –> H₂ (g) + MgCl₂ (aq)

2. The temperature of the solution increases from 22.21 °C to 24.15 °C. Assume the specific heat capacity of the solution is 4.20 J/g·°C, and the density of the HCl solution is 1.00 g/mL
3. Calculate the enthalpy change for the reaction in J/mol.
4. You just submit your answer with the scientific notation format and with the correct number of significant figures. For example, if you answer is 12345, you must submit your answer as 1.24e+4 (for 3 significant figures)
   

QUESTION 11

1. McMurry and Fay question 8.52.

QUESTION 12

1. McMurry and Fay question 8.53.

QUESTION 13

Calculate the enthalpy change for the conversion of diamond to graphite:

C_diamond (s) –> C_graphite (s)

From the information provided below:

C_graphite (s) + O₂ (g) –> CO₂ (g) ∆H° = –394 kJ

C_diamond (s) + O₂ (g) –> CO₂ (g) ∆H° = –396 kJ

QUESTION 14

1. Is the conversion of diamond to graphite spontaneous? Explain

QUESTION 15

1. Use the standard heat of formation listed in Table 8.2 to calculate the standard enthalpy change for the following overall reaction:4NH₃ (g) + 7O₂ (g) –> 4NO₂ (g) + 6 H₂O (l)Where ∆H°_f of NO₂ is 34 kJ/mol

QUESTION 16

1. McMurry and Fay questions:

   –1.2. 8.103a) –1.2. 8.103b) –1.2. 8.103c)

   1. Non-spontaneous 2. Spontaneous

QUESTION 17

1. At what temperature is the following process spontaneous at 1 atm?

Br₂(l) –> Br₂ (g)

∆H° = 21 kJ/mol, and ∆S° = 93 kJ/mol

Submit your answer with the scientific notation format with correct number of significant figures and unit.