What is the volume of 1.5 moles of chlorine gas (cl2) at standard temperature and pressure ( answer . . . . 57.5 l. 71.0 l. 22.4 l. 33.6 l

The ideal gas equation is PV = nRT. if you are looking for the volume of the chlorine gas then the equation will turn out to be V = nRT/P. At STP, temperature is 273K and pressure is 1 atm.

V = nRT/P

V = (1.5 moles Cl2)(0.08206 L-atm/mol – K)(273K) / (1atm)

V = 33.6 liters

where's the diagram?

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