decalescent energy-absorbing endothermal heat-absorbing endoergic.
Hope this helps!
Answer: P2 = 0.858 atm
Explanation:
Use the combined gas law: P1V1/T1 = P2V2/T2,
where the subscripts are the initial (1) and final (2) states. Temperature must be in Kelvin. We want P2, so rearrange the equation to solve for P2:
P2 = P1(V1/V2)(T2/T1)
Note how I've arranged the volume and temperature values: as ratios. Now it is easy to cancel units and see what is going to happen to the pressure if we lower the temperature. Since the pressure change is a function of (T2/T1), and we are lowering the temperature (T2), we'd expect this to decrease the pressure.
No information is given on volume, so we'll assume a convenient value of 1 liter. Now enter the data:
P2 = (0.917atm)*(1)*(322K/344K)
P2 = 0.858 atm
Answer:- 
.
Solution:- Mass of Iron added to water is 93.3 g. Initial temperature of iron metal is 65.58 degree C and final temperature of the system is 19.68 degree C.
temperature change, 
for iron metal = 65.58 - 19.68 = 45.9 degree C
specific heat for the metal is given as 0.444 J per g per degree C.
let's calculate the heat lost by iron metal using the equation:
where, q is the heat energy, m is mass, c is specific heat and delta T is change in temperature. let's plug in the values and calculate q for iron metal:
q = 1901.42 J
Using same equation we will calculate the heat gained by water.
mass of water is 75.0 g.
for water = 19.68 - 16.95 = 2.73 degree C
specific heat for water is 4.184 J pr g per degree C. Let's plug in the values:
q = 856.674 J
Total heat lost by iron metal is the sum of heat gained by water and calorimeter.
So, heat gained by calorimeter = heat lost by iron metal - geat gained by water
heat gained by calorimeter = 1901.42 J - 856.674 J = 1044.746 J
Change in temperature for calrimeter is same as for water that is 2.73 degree C
For calorimeter, 
So, the heat capacity of calorimeter is .
Answer:
Explanation:
Since we are not given the mole fraction of ethanol and water; we will solve this theoretically.
Using Raoult's Law:
For water:
where 
of water = 12.5 mmHg
Then, the vapor pressure of water:
For ethanol:
and the of ethanol = 32.1 mmHg
Then, the vapor pressure of ethanol:
The total vapor pressure 
The total vapor pressure = 
Answer:
0.342 m
Explanation:
From the question given above, the following data were obtained:
Mass of NaBr = 14.57 g
Mass of water = 415 g
Molar mass of NaBr = 102.89 g/mol
Molality of NaBr =?
Next, we shall determine the number of mole in 14.57 g of NaBr. This can be obtained as follow:
Mass of NaBr = 14.57 g
Molar mass of NaBr = 102.89 g/mol
Mole of NaBr =?
Mole = mass / molar mass
Mole of NaBr = 14.57 / 102.89
Mole of NaBr = 0.142 mole
Next, we shall convert 415 g of water to kg. This can be obtained as follow:
1000 g = 1 Kg
Therefore,
415 g = 415 g × 1 Kg / 1000 g
415 g = 0.415 Kg
Thus, 415 g is equivalent to 0.415 Kg.
Finally, we shall determine Molality of the solution as follow:
Mole of NaBr = 0.142 mole
Mass of water = 0.415 Kg
Molality of NaBr =?
Molality = mole / mass of water in Kg
Molality of NaBr = 0.142 / 0.415
Molality of NaBr = 0.342 m
Therefore, the molality of NaBr solution is 0.342 m.
