Answer: a. 17.7 KJ/Mol
b. T=210K
Explanation:
Arsine, ash3 is a highly toxic compound used in the electronics industry for the production of semiconductors. its vapor pressure is 35 torr at – 111.95°c and 253 torr at – 83.6°c. using these data calculate.
the question isnt completely originally, but we could look at the likely derivation from the questions
(a) the standard enthalpy of vaporization
using the clausius clapeyron equation
In (PT1vap / PT2vap) = delta H (vap) / R ( (1/T1) - (1/T2) )
In (35Torr/253Torr) = delta H (vap) / 8.3145 ( (1/189.55) - (1/161.2) )
Therefore, Delta H (vap) = 17.7 KJ/Mol
b. Also the boiling point
What is the normal boiling point of arsine?
At the boiling point Pvap = atmospheric pressure = 1 atm=760 torr
substitution into the equation as stated in question 1
ln(760/253)=17700/8.314(1/189.55-1/T)
T=210K
Do you have a diagram or anything?
Answer:
Right shoe
Explanation:
Let the mass and velocity of incoming puck be m and v respectively.
Momentum of the colliding puck will be mv
In case of first case , the momentum of puck becomes zero so change in momentum after collision with left shoe
= mv - 0 = mv
If time duration of collision be t
rate of change of momentum
= mv / t
This is the force exerted by puck on the left shoe .
Now let us consider collision with right shoe
momentum after collision with right shoe
- mv
change in momentum
= mv - ( - mv ) = 2mv
If time duration of collision be t
rate of change of momentum
= 2mv / t
This is the force exerted by puck on the right shoe .
Since the force on the right shoe is more , this shoe will have greater speed
after collision.
About <span>250,000 DWT(Dead Weight Tons)</span>
O3 has molar mass of 48 g/mol
Therfore I mole weighs 48 grams
9.11 moles of ozone has a mass of 9.11 x 48grams = 437grams = 0.437kg