Thermochemistry: Quiz 3
Chapter 6

Dr. Robert Eugene Belford



Question 1
A 2.00 g sample of Iron (S=0.4513 J/g.0C) at 180.00C is dropped into 10.0 ml of water at 20.00C. What is the final temperature?
(A)  2.340C
(B)  23.40C
(C)  46.80C
(D)  1240C
 
Hint

Your response
Not answered yet

Question 2
A 2.00 g sample of Iron (S=0.4513 J/g.0C at 180.00C is dropped into 10.0 ml of water in a calorimeter at 20.00C. What is the final temperature if the calorimeter has a constant of 67J/0C?
(A)  45.80C
(B)  33.50C
(C)  21.30C
(D)  24.50C
 
Hint

Your response
Not answered yet

Question 3
What is the calorimeter constant of a calorimeter if 25.0 ml of water at 100.00C is added to 25.0 ml of water at 20.00C and the final temperature became 50.00C?
(A)  104J/0C
(B)  22.3J/0C
(C)  69.7J/0C
(D)  246J/0C
 
Hint

Your response
Not answered yet

Question 4
What mass of iron (S=0.4513 J/g.0C) at 500.0C would be required to raise 10.0 g of water from 20 0C to 700C
(A)  0.0355g
(B)  8.664g
(C)  1.09g
(D)  9.66g
 
Hint

Your response
Not answered yet

Question 5
What is the enthalpy of neutralization of hypochlorous acid with sodium hydroxide if mixing 100.0 ml of 1.000 M HClO with 100.0 ml of 1.000 M NaOH causes the temperature to increase from 25.000C to 30.010C?
(A)  -56.32KJ/mol
(B)  -41.92KJ/mol
(C)  -22.93KJ/mol
(D)  41.92kJ/mol
 
Hint

Your response
Not answered yet

Question 6
Calculate the enthalpy of reaction for the formation of phosphoric acid from the following unbalanced equation: P4O10 +H2O --> H3PO4 from the following enthalpies of formation:

ΔHof(P4O10(s)) = -2984 KJ/mol
ΔHof(H2O(l)) = -286 KJ/mol
ΔHof(H3PO4(aq)) = -1288 KJ/mol

(A)  -452 kJ/mol
(B)  -4520 kJ/mol
(C)  -8283 kJ/mol
(D)  8283 kj/mol
 
Hint

Your response
Not answered yet