When 0.044S g of magnesium metal was allowed to react with excess hydrochloric a

Question

When 0.044S g of magnesium metal was allowed to react with excess hydrochloric acid, 46.50 mL of hydrogen gas was collected over water. The barometric pressure at the time was reported to be at 30.07 inHg. The temperature of the water near the mouth of the eudiometer tube was 26.4 degree C. The water level inside the tube was measured to be 23.01 cm higher than the water level in the beaker. Calculate the molar volume of hydrogen at STP, and the percent error in this value Also calculate the experimental value for the universal gas constant R and the percent error in that value Be sure to consider significant figures and units. You can attach an extra sheet for your calculations.

Explanation / Answer

To do this calculation you have to use ideal gas equation PV = nRT

PH2 = Patm-Pwater = 763.7 mmHg- 17.04 mmHg = 746.66 mmHg = 1 atm *746.66 mmHg/760 mmHg = 0.982 atm

V = 46.50 mL = 0.0465 L

n = 0.00183

T = 26.4oC = 299.4 K

PV = nRT

or, R = PV/nT = 0.984 atm *0.0465 L/ 0.00183 mol *299.4 K = 0.083 L atm/K/mol

Actual value = 0.082 L atm/K/mol

% error = (0.083-0.082)/0.082 * 100 = 1.22 %

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