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.

first let us lay out the formula for potential

and kinetic energy:

pe = mgh

ke = (mv^2)/2

where: m=mass, v=velocity, g=gravitational

acceleration, h=height

calculating for mass using the known values of

pe:

340j = m (9.81 m/s^2) (50ft) (1m/3.28ft)

m = 2.27 kg

the law of conservation of energy states that

energy is neither created nor destroyed. therefore, the change in kinetic

energy from 50 ft to 35 ft would be equal to the change in potential energy

from 50 ft to 35 ft. however it would be opposite in signs since one is losing

while other is gaining.

ke(35ft) – ke(50ft) = - [ pe(35ft) – pe(50ft]

ke(50ft) = 0 since the brick is initially at rest

ke(35ft) = 340j - 2.27kg (9.81 m/s^2) (35ft)

(1m/3.28 ft)

ke(35ft)

= 102.38 j

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this

he would use the colour black

what does the table look like