13. 15.0g of water at 60.0°C is mixed with 45.0g of water at 40.0°C. What will b

Question

13. 15.0g of water at 60.0°C is mixed with 45.0g of water at 40.0°C. What will be the final temperature if no heat is lost to the surroundings? Use the reaction and the Al for the reaction provided to answer questions 14-16 AH-340 k 14. How much heat would be required to react 6 moles of Chlorine trifluoride (CIF3)? (A) 2040k (B) 340 (C) 1020kJ (D)-340k (E) 10,200k 15. If the reaction absorbed 170kJ of heat what mass of F:0 would be produced? (A) 8ig (B) 162g (C) 340g (D) 170g (E) 450g 16. If 340kJ of heat is absorbed what volume of products will format STP? a.224L b, 24.8L c, 89.6L d.646L e, 44.8L 17. Which of the following statements regarding heat and temperature is correct. a. Heat is an actual quantity of energy temperature is a measure of energy b. Temperature and heat are the same quantity c. A substance with a higher temperature is always has more heat than another substance with a lower temperature. d. Temperature is conserved but heat is not

Explanation / Answer

13. heat lost by hot water = heat gained by cold water

      m*s*DT = m*s*DT

   15*4.184*(60-x) = 45*4.184*(x-40)

x= final temperature of mixture= 45 C

answer: c

14. from equation, 2 mol ClF3 = 340 kj

                   6 mol ClF3 = 340*6/2 = 1020 kj

answer: C

15. no of mol of F2O formed = 170*3/340 = 1.5 mol

    mass of F2O formed = 1.5*54 = 81 G

Answer: A

16. volume of products = nRT/P

                       = (4*0.0821*273.15/1)

                       = 89.7 L

answer: C

17. answer: a,c

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