Cao(s) + h2o(l) → ca(oh)2(s): δh = −65.2 kj

which statement about the reaction between calcium oxide and water is correct?

65.2 kj of heat are released for every mole of cao that reacts.
130 kj of heat are released for every mole of h2o that reacts.
130 kj of heat are absorbed for every mole of cao that reacts.
65.2 kj of heat are absorbed for every mole of h2o that reacts.
question 2 (true/false worth 2 points)

(07.02 lc)

if the amount of energy required to break bonds in the reactants is more than the amount of energy released in forming bonds in the products, then the reaction will have a negative change in enthalpy (−δh).

true
false
question 3(multiple choice worth 4 points)

(07.02 mc)

a 52-gram sample of water that has an initial temperature of 10.0 °c absorbs 4,130 joules. if the specific heat of water is 4.184 j/(g °c), what is the final temperature of the water?

11 °c
19 °c
29 °c
51 °c
question 4(multiple choice worth 4 points)

(07.02 mc)

the specific heats of two natural substances are shown in the table.

specific heat
natural substance specific heat
wet mud 2.5 j/g °c
sandy clay 1.4 j/g °c

a pile of wet mud and a pile of sandy clay of equal masses were placed next to each other on a sunny day.

if the temperature of each pile was equal in the afternoon, which substance is likely to show a higher temperature after a few hours and why?
wet mud, because it released more heat while placed in the sun.
sandy clay, because it absorbed more heat while placed in the sun.
sandy clay, because it requires less energy to increase its temperature.
wet mud, because it requires more energy to increase its temperature.
question 5(multiple choice worth 3 points)

(07.02 lc)

the substances below are listed by increasing specific heat capacity value. starting at 30.0 °c, they each absorb 100 kj of thermal energy. which one do you expect to increase in temperature the most?

silver, 0.239 j/(g °c)
aluminum, 0.921 j/(g °c)
lithium, 3.56 j/(g °c)
water, 4.184 j/(g °c)
question 6(multiple choice worth 4 points)

(07.02 mc)

some thermodynamic properties of ethanol are listed in the table.

thermodynamic properties
property value
c (solid) 0.5 j/g °c
c (liquid) 1.0 j/g °c
c (gas) 2.0 j/g °c
melting point −114 °c
boiling point 78 °c

how much heat is released when 60.0 g of ethanol cools from 70 °c to 43 °c?
1,600 j
1500 j
810 j
750 j