50 g of solid sodium hydroxide is dissolved in 175 mL of water. Using a coffee-cup calorimeter, the temperature change of the water is measured to be -2.1°C.  Which equation best describes this system? NaOH(s)→NaOH(aq)  +  kJ                   NaOH(s)+ kJ →NaOH(aq)                                    NaOH(s)→NaOH(l) + kJ                 NaOH(aq)→NaOH(s) + kJ                     NaOH(aq)+ kJ →NaOH(s)                                NaOH(l)+ kJ → NaOH(s)

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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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  1. 50 g of solid sodium hydroxide is dissolved in 175 mL of water. Using a coffee-cup calorimeter, the temperature change of the water is measured to be -2.1°C.  Which equation best describes this system?
  2. NaOH(s)→NaOH(aq)  +  kJ                  
  3. NaOH(s)+ kJ →NaOH(aq)                                   
  4. NaOH(s)→NaOH(l) + kJ                
  5. NaOH(aq)→NaOH(s) + kJ                    
  6. NaOH(aq)+ kJ →NaOH(s)                               
  7. NaOH(l)+ kJ → NaOH(s)  
  8. What is the definition of the temperature of a substance?
  9. the speed of the slowest particles in the substance, subtracted from the speed of the fastest particles.   
  10. the heat capacity of the substance times its mass   
  11. a measure of the average kinetic energy of a system
  12. the total heat content of a substance                    
  13. the speed of the fastest particles in the substance   
  14. Which statement describes an endothermic reaction?
  15. The surroundings warm up.     
  16. The system releases energy.  
  17. The potential energy of the products is less than the potential energy of the reactants.
  18. The potential energy of the reactants is less than the potential energy of the products.
  19. Which statement is true regarding the thermochemical equation    A +  B  + KJ àAB
  20. The reaction is endothermic and produces heat    C. The reaction is endothermic and requires heat   
  21. The reaction is exothermic and produces heat.      D. The reaction is exothermic and requires heat.
  22. 150.0 mL of water releases 7.84 kJ of energy. The specific heat capacity of water is 4.184 J/g·°C. What is the temperature change? (1mL of water = 1 g)
  23.  3.52oC            B.  -12.5 °C         C. - 0.0125oC         D.  0.0125°C        E.  12.5°C      

9.When a sample of potassium nitrate is dissolved in water, the temperature of the water changes from 18.5°C to 20.3°C. Which statement describes this process of the change of state of potassium nitrate?

  1.  This process is endothermic, so the water gets cooler.
  2.  This process is endothermic, so the water gets warmer.
  3.  This process is exothermic, so the water gets cooler.
  4.  This process is exothermic, so the water gets warmer.
  5.   None of the above options can be known for sure.

10.A ring with a mass of 14.8g is tossed into a fire and then removed. The ring’s temperature went from 23.2oC to 55.8oC.  During this process, the ring gained 214J of heat.  Of what pure metal is the ring composed?                                  A.   copper        B. iron       C. gold        D. aluminum

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