4H,O) the H fr the reaction. 12. Given the balanced reaction and the table of st

Question

4H,O) the H fr the reaction. 12. Given the balanced reaction and the table of standard enthalpies given below. Determine AH(cJ/mol) 238.7 393.5 -241.6 Substance CHOHg) H O(g) a. -1276kJ/mole b. -1150J/mole c. -1075kJ/mole d. 1250kJ/mole 13. 15.0g of water at 60.0C 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 c.45Cd. 25°C Use the reaction and the H for the reaction provided to answer questions i 4-16. -340 kJ 14. How much heat would be required to react 6 moles of Chlorine trifluoride (CIFs)? (A) 2040kJ (B) 340kJ (C) 1020kJ (D) -340kJ (E) 10,200k 15. If the reaction absorbed 170kJ of heat what mass of F20 would be produced? (A) 81g (B) 162g (C) 340g (D 170g (E)450g 16. If 340kJ of heat is absorbed what volume of products will format STP? a. 22.4L b. 24.8L c. 89.6L d. 64.6L 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

12)

we have:

Hof(CH3OH(g)) = -238.7 KJ/mol

Hof(O2(g)) = 0.0 KJ/mol

Hof(CO2(g)) = -393.5 KJ/mol

Hof(H2O(g)) = -241.6 KJ/mol

we have the Balanced chemical equation as:

2 CH3OH(g) + 3 O2(g) ---> 2 CO2(g) + 4 H2O(g)

deltaHo rxn = 2*Hof(CO2(g)) + 4*Hof(H2O(g)) - 2*Hof( CH3OH(g)) - 3*Hof(O2(g))

deltaHo rxn = 2*(-393.5) + 4*(-241.6) - 2*(-238.7) - 3*(0.0)

deltaHo rxn = -1276 KJ/mol

Answer: a

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