In the calorimetry experiment you performed in the lab, what will happen to the
ID: 695411 • Letter: I
Question
In the calorimetry experiment you performed in the lab, what will happen to the calculated value of heat of solution(Enthalpy) when: (I point) a) some salt gets spilled on the bench while transferring it to the calorimeter Answer here Lab-Ideal Gas Laws 3.) Determine the value of R from the following data obtained from the Ideal Gas Law experiments of production of Hydrogen gas: (3 points) a) Mass of Magnesium used b) M.W. of Mg 0.021g 24.31 c) Volume of Hydrogen gas produced d) Atmospheric pressure e) Vapor pressure of water ) Temperature 21.85 ml 752.562 tOrr 23.4 torr 24.8 °C g) Moles of Mg mol h) Pressure of Hydrogen gas produced atm. i) Value of R(Report up to 5 digit after decimal) (Also write the unit: 1 point) unit Space for calculation:Explanation / Answer
When Some salts get spilled on the bench while transforming it to calorimeter, then the value of R will be increase due to following relation
PV = n RT
R = PV/n T
As the number of mole decreases the value of R increases
Given:
Mass of Mg= 0.021 g
M.W. of Mg= 24.31 g / mole
Volume of H2 gas = 21.85 ml
Atmospheric pressure = 752.562 torr
Vapor pressure of water = 23.4 torr
Temperature = 24.8 C
Mole of Mg = amount in g / M.W
= 0.021 g/ 24.31
= 0.000864 moles
Pressure of H2 = total pressure - pressure of water vapor
= 752.562 torr - 23.4 torr
= 729.162 torr
760 torr = 1.0 atm, then
729.162 torr * 1 .0 atm /760 torr
= 0.9594 atm
T = 24.8 C , 24.8 +273.15 =297.95 K
Volume = 21.85 ml
= 0.02185 L
Now from ideal gas equation , PV = n RT
R = PV / n T
=0.9594 atm * 0.02185 L / 0.000864 moles *297.95 K
= 0.081432 atm –L/ mole –K
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