Use the information in the table to describe the temperature-vs.-time diagrams.
1 answer:
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Answer:
77 L of water can be made.
Explanation:
Molar mass of = 32 g/mol
So, 55 g of =
mol of
= 1.72 mol of
As hydrogen is present in excess amount therefore is the limiting reagent.
According to balanced equation, 1 mol of produces 2 mol of
.
So, 1.72 mol of produce
mol of
or 3.44 mol of
.
Let's assume gas behaves ideally at STP.
Then, , where P, V, n, R and T represents pressure, volume, no. of moles, gas constant and temperature in kelvin scale respectively.
At STP, pressure is 1 atm and T is 273 K.
Here, = 3.44 mol and R = 0.0821 L.atm/(mol.K)
So,
Option (b) is correct.
Answer: The vapor pressure of water at 298 K is 3.565kPa.
Explanation:
The vapor pressure is determined by Clausius Clapeyron equation:
where,
= initial pressure at 298 K = ?
= final pressure at 373 K = 101.3 kPa
= enthalpy of vaporisation = 41.1 kJ/mol = 41100 J/mol
R = gas constant = 8.314 J/mole.K
= initial temperature = 298 K
= final temperature = 373 K
Now put all the given values in this formula, we get
Therefore, the vapor pressure of water at 298 K is 3.565kPa.