The air in a 4.00 L tank has a pressure of 1.20 atm . What is the final pressure, in atmospheres, when the air is placed in tank
1 answer:
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Answer:
The enthalpy change for the solution process = - 158.34 kJ/mol
Explanation:
Given that:
The mass of salt AX = 2.499 g
The mass of water = 135.3 g
The mass of the solution = ( 2.499 + 135.3 ) g = 137.799 g
The specific heat of salt solution s is known to be = 4.18 J/g° C
The change in temperature i.e. ΔT = 35.2 °C - 23.6 °C = 11.6 °C
Thus, the amount of heat raised is equal to the heat absorbed by the calorimeter.
∴
Recall that the mass of the salt = 2.499 g
The number of moles of the salt =
= 0.0422 mol of AX
Finally the enthalpy change,
= - 158.34 kJ/mol
The enthalpy change for the solution process = - 158.34 kJ/mol
Answer:The volume increases by 11%
Explanation:
When the pressure is decreased, the volume must definitely increase, to maintain the same pressure, the temperature must then also be increased as we see in the question. The volume was increased just as the pressure decreased and the temperature had to be increased to maintain a constant pressure. We have applied the general gas equation in solving the problem.
