The boiling point of water can be calculated by the equation:
Where:
P = Pressure in mm Hg
Po = Atmospheric pressure in mm Hg
ΔH= heat of vaporization in kJ/mol
R = Ideal Gas Constant (J/mol-K)
To = normal boiling point in Kelvin
T = boiling point of water (K)
Our known values are:
P = 630 mm Hg
Po = 760 mm Hg
ΔH = 40.66 kJ/mol = 40.66×1000
=40660
R = 8.314 J mol⁻¹ K
⁻¹
To = 373 K
Putting these values in the equation,
Solving the equation will give:
T=370K
so, the boiling point of water is 370 K.
Answer:
Explanation:
Alkali metals ------ outermost orbit containing one electron
ns²np¹
Alkaline metals -------- outermost orbit containing two electron
ns²np²
halogens --------------- outermost orbit containing seven electron
ns²np⁵
noble gas --------------- outermost orbit containing eight electron
ns²np⁶.
Answer:
1.33 moles CO2
Explanation:
The number you are converting is 58.4 g CO2, so you start with this value. The conversion factor is 44.0 g/mol CO2. In order to cross out the grams, the grams must go on the bottom of the conversion factor.
1 mol CO2
58.4 g CO2 x -------------------------- = 1.33 moles CO2
44.0 grams
The answer has three sig figs.
Answer:
85.5 mmHg is the pressure of the gas sample when the valve is opened.
Explanation:
The combined gas equation is,
where,
= initial pressure of gas in container A = 165 mmHg
= final pressure of gas = ?
= initial volume of gas in container A= 
= final volume of gas = 135 mL + 117 mL = 252 mL
= initial temperature of gas in container A = 
= final temperature of gas = 
Now put all the given values in the above equation, we get:
85.5 mmHg is the pressure of the gas sample when the valve is opened.
I think the answer is A, ozone depletion
