Heat required to vaporize 1 mol of water from water at 100C to steam at 100C = 40.7 kJ
<span>1 mol of water weighs = 18.015g
</span>1.55 kg = <span>1550/18.015 mol = 86.03 mol
</span><span>Heat required to vaporize :
</span>= 86.03 mol x <span>40.7 kJ
</span>
= 3501.421 kJ
Well we need to see the fossil
The pressure of the nitrogen gas produced is determined as 44.77 atm.
<h3>
What is the pressure of the Nitrogen gas?</h3>
The pressure of the nitrogen gas is determined from ideal gas equation, as shown below;
PV = nRT
P = nRT/V
where;
- n is number of moles = 2 moles
- R is ideal gas constant = 0.08205 L.atm/mol.K
- T is temperature = 68⁰C = 68 + 273 = 341 K
- V is volume = 1.25 L
P = (2 x 0.08205 x 341)/(1.25)
P = 44.77 atm.
Learn more about pressure here: brainly.com/question/25736513
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A i believe is the answer
