Please explain how to solve, thank you!! Background:Many metals react with hydrochloric acid to produce hydrogen gas and metal ions.In this Lab you will use Magnesium: Mg(s) + 2 H+(aq) → H2(g) + Mg2+(aq) The moles of hydrogen gas produced can be determined using the Ideal Gas equation,PV = nRT. Useful InformationPressure of water vapor at 18.8 °C = 16.3 torr P(gases in buret) = P(hydrogen gas) + P(water vapor) PV= nRT where P is in atm, V is in L, and T is in K TK = Tºc + 273 l.0 atm = 760 tor R = 0.082 L atm /K mol Data Volume of water added to the 50 mL buret that has uncalibrated bottom1.0 mL Buret reading after addition of 1.00 mL water 49.50 mLMass of metal sample 0.038 gTemperature of water (and thus temperature of gases). 18.8 °CBuret reading of gases 36.9 mLBarometric pressure 760 torrQUESTIONWhat is the total volume of hydrogen gas in milliliters? (2 decimal places) What is the total volume of hydrogen gas in liters? (4 sig figs) What is the temperature of hydrogen gas in Kelvins? (3 sig figs)

Given: mass of Mg = 0.038 g temperature = 18.8 °C = 291.8 K Barometric pressure = 760 torr Pressure of water vapor at 18.8 °C = 16.3 torr Calculation for pressure of hydrogen gas: P(hydrogen gas) = P(gases in buret) - P(water vapor) P(hydrogen gas) = 760 torr - 16.3 torr P(hydrogen gas) = 743.7 torr = 0.9785 atm Calculation for moles of Mg: moles=massmolar massmoles of Mg=0.038 g24.3 g/molmoles of Mg=0.00156 molCalculation for volume of H2 gas: 1 mole of Mg produces 1 mole of H2 gas. 0.00156 mole of Mg produces 0.00156 mole of H2 gas. PV=nRTV=nRTPV=0.00156 mol×0.0821×291.8 K0.9785 atmV=0.03819 L=38.19 mL Answer: 1) 38.19 mL 2) 0.03819 L 3) 292 K

Answered: Many metals react with hydrochloric…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

Please explain how to solve, thank you!!

Background:

Many metals react with hydrochloric acid to produce hydrogen gas and metal ions.

In this Lab you will use Magnesium:

Mg_(s) + 2 H⁺_(aq) → H_2(g) + Mg²⁺_(aq)

The moles of hydrogen gas produced can be determined using the Ideal Gas equation,

PV = nRT.

Useful Information

Pressure of water vapor at 18.8 °C = 16.3 torr

P(gases in buret) = P(hydrogen gas) + P(water vapor)

PV= nRT where P is in atm, V is in L, and T is in K

T_K =T^ºc + 273

l.0 atm = 760 tor

R = 0.082 L atm /K mol

Data
Volume of water added to the 50 mL buret that has uncalibrated bottom	1.0 mL
Buret reading after addition of 1.00 mL water	49.50 mL
Mass of metal sample	0.038 g
Temperature of water (and thus temperature of gases).	18.8 °C
Buret reading of gases	36.9 mL
Barometric pressure	760 torr

QUESTION

What is the total volume of hydrogen gas in milliliters? (2 decimal places)

What is the total volume of hydrogen gas in liters? (4 sig figs)

What is the temperature of hydrogen gas in Kelvins? (3 sig figs)

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