In the reaction between hydrochloric acid and magnesium 2 HCl(aq) + Mg(s) → MgCl 2 ( aq) + H 2 ( g ) 100.0 g of HCl(aq) is reacted. The volume of H 2 is produced if the temperature is 47.5 °C and the pressure is 1.02 atm is to be calculated. Assume the ideal gas law applied. Concept introduction: The ideal gas law or general gas equation is the equation of state of a hypothetical ideal gas. Thought it has some limitations, it is a good approximation of the behavior of several gases under several conditions. The term was first coined by Emile Clapeyron in the year of 1834 as combination of other laws. The ideal gas law can be written as PV = nRT.

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Chapter 1, Problem 1.25E

Interpretation Introduction

Interpretation:

In the reaction between hydrochloric acid and magnesium

2HCl(aq) + Mg(s)→MgCl2(aq) + H2(g)

100.0 g of HCl(aq) is reacted. The volume of H₂ is produced if the temperature is 47.5 °C and the pressure is 1.02 atm is to be calculated. Assume the ideal gas law applied.

Concept introduction:

The ideal gas law or general gas equation is the equation of state of a hypothetical ideal gas. Thought it has some limitations, it is a good approximation of the behavior of several gases under several conditions. The term was first coined by Emile Clapeyron in the year of 1834 as combination of other laws. The ideal gas law can be written as PV = nRT.

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A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based on experimentally collected data, the student calculates R to equal L'atm 0.0832 mol·K L'atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error =|1.389 (b) For the statements below, identify the possible source(s) of error for this student's trial. The student uses the barometric pressure for the lab to calculate R. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student does not clean the zinc metal with sand paper. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it.

References Use the References to access important values if needed for this question. Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 754 mm Hg. If the wet H2 gas formed occupies a volume of 6.46 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °C. Submit Answer