Mg(s)+2HCl(aq)=MgCl2(aq)+H2(g) (A) 0.0675g Mg AND 4mL of 6M HCl were used. Barometric pressure were 28.85 inches Hg....

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Chemistry

Mg(s)+2HCl(aq)=MgCl2(aq)+H2(g)
(A) 0.0675g Mg AND 4mL of 6M HCl were used. Barometric pressurewere 28.85 inches Hg. A volume of 73.6mL of hydrogen was collectedat a temperature of 26.0C. The vapor pressure of water is 25.2mm Hgat this temperature. Calculate R, the gas law constant, inL-atom\mol-K using the information above for the reaction of HCland Mg. 760 mmHg= 1.00atm. 1 inch=2.54 cm.
Show your calculation
(B) why is it necessary to substract the vapor pressure of thehydrogen gas formed to your experiment?
(C) If some gas was lost during the process and the measuredamount of gas was less than the amount that should have beenproduced, would this increase or decrease the calculated R ?Explain your answer.

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Solution a Lets calculate the moles of the hydrogen gas produced from each reactant 00675 g Mg 1 mol 24305 g 1 mol H21 mol Mg 0002777 mol H2 Moles of HCl molarity volume 60 mol per L 0004 L 0024 mol HCl 0024 mol HCl 1 mol H22 mol HCl 0012 mol H2 So the limiting reactant is Mg so the moles of H2 gas formed are See Answer

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Mg(s)+2HCl(aq)=MgCl2(aq)+H2(g) (A) 0.0675g Mg AND 4mL of 6M HCl were used. Barometric pressure were 28.85 inches Hg....

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Chemistry

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