A sample of gas has a volume of 5.79 L at 25C and 518. What will be the volume of this gas at STP
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Answer:
(a) The weight percent HNO3 is 63%.
(b) Density of HNO3 = 111.2 lb/ft3
(c) Molarity = 13792 mol HNO3/m3
Explanation:
(a) Weight percent HNO3
To calculate a weight percent of a component of a solution we can express:
(b) Density of HNO3, in lb/ft3
In this calculation, we use the specific gravity of the solution (1.382). We can start with the volume balance:
The density of HNO3 is 1.782 times the density of water (Sp Gr of 1.782). If the density of water is 62.4 lbs/ft3,
(c) HNO3 molarity (mol HNO3/m3)
If we use the molar mass of HNO3: 63.012 g/mol, we can say that in 1,704 kg (or 1704 g) of HNO3 there are 1704/63.012=27.04 mol HNO3.
When there are 1.704 kg of NHO3 in solution, the total mass of the solution is (1.704+1)=2.704 kg.
If the specific gravity of the solution is 1.382 and the density of water at 20 degC is 998 kg/m3, the volume of the solution is
We can now calculate the molarity as
We have that the minimum mass of ice , required to <em>bring</em> the <em>final </em>temperature to 15.0 ∘C is <em>mathematical </em>given as
- m=67.9g
From the question we are told
- The <em>optimum</em> drinking temperature for a Shiraz is 15.0 ∘C .
- A certain bottle of Shiraz having a heat capacity of 3.40 kJ∘C−1 is 23.1 ∘C at room <em>temperature</em>.
- The heat of fusion of ice is 6.02 kJmol−1 and the heat capacity of ice is 2.108 Jg−1∘C−1.
Generally the equation for the Heat released is mathematically given as
Q=cDT
Q=3.4*8.1*10^3
Q=27540J
Therefore
Heat absorded
H=m*4*2.108+m/18*6.02*10^3+m*15*4.18
H=405.58mJ
THerefore
m=67.9g
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