Loy Experiment 5: Generating Hydrogen Gas Part B: Molar mass of unknown metal Mass of unknown metal (X): Volume of H2 gas Temperature of H₂ gas Atmospheric pressure (see barometer) Vapor pressure of water Partial pressure of H₂ gas 746.5mmHg-16.5mmHg = 730 mmHg Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the experiment: (0.96a+m)(0.019L) V=19.0mL (0.0821latm) (292K) MOIK P=746.5mmHg T: 292K 273+19.0=292° 19.0m₂ x Unknown #: 0.1307 mL 19.0 °C 19.0 746.5 mmHg 16.5 mmHg 0.0217 730.0 mmHg 0.961 7 atm latm: 760mmHg 0.000769x g IL ¹2^1000ML 0.019L moles H₂: 0.00076 1000mL Convert moles of hydrogen gas to moles of the metal (X), using the balanced equation. X (s) + 2 HCl (aq) → XC12 (aq) + H₂ (g) 0.00076m₂l molx (XSPS) EPFO 0-1Pa 64 = 0.00076molX Tmg2₂0)( I Calculate the molar mass of the metal (g/mol) and identify the metal. 0.13079x171.97g/mol 0.019 292. 22R=0.0821 La -0.00076m0lX ma moles X: 0.00076 Molar mass: 171.97 Metal: L K 738
Loy Experiment 5: Generating Hydrogen Gas Part B: Molar mass of unknown metal Mass of unknown metal (X): Volume of H2 gas Temperature of H₂ gas Atmospheric pressure (see barometer) Vapor pressure of water Partial pressure of H₂ gas 746.5mmHg-16.5mmHg = 730 mmHg Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the experiment: (0.96a+m)(0.019L) V=19.0mL (0.0821latm) (292K) MOIK P=746.5mmHg T: 292K 273+19.0=292° 19.0m₂ x Unknown #: 0.1307 mL 19.0 °C 19.0 746.5 mmHg 16.5 mmHg 0.0217 730.0 mmHg 0.961 7 atm latm: 760mmHg 0.000769x g IL ¹2^1000ML 0.019L moles H₂: 0.00076 1000mL Convert moles of hydrogen gas to moles of the metal (X), using the balanced equation. X (s) + 2 HCl (aq) → XC12 (aq) + H₂ (g) 0.00076m₂l molx (XSPS) EPFO 0-1Pa 64 = 0.00076molX Tmg2₂0)( I Calculate the molar mass of the metal (g/mol) and identify the metal. 0.13079x171.97g/mol 0.019 292. 22R=0.0821 La -0.00076m0lX ma moles X: 0.00076 Molar mass: 171.97 Metal: L K 738
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Transcribed Image Text:Experiment 5: Generating Hydrogen Gas
Part B: Molar mass of unknown metal
Mass of unknown metal (X):
Volume of H₂ gas
Temperature of H₂ gas
Atmospheric pressure (see barometer)
Vapor pressure of water
Partial pressure of H₂ gas
746.5mmHg-/6.5mmHg = 730 mmHg
Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the
experiment:
(0.96atm) (0.019L)
(0.0821latm)(292k)
Molk
V: 19.0mL
P=746.5mmHg
T: 292K
273+19.0=292°
0.00076m₂l molx
Tmgha₂
(XSPS)
2
PassPro
Unknown #:
0.000769x
0.1307
19.0
°C
19.0
746.5 mmHg
16.5 mmHg 0.0217
730.0 mmHg 0.961
64
g
IL
19.0m₂ x
0.019L
moles H₂: 0.00076
JocomL
1000ML
Convert moles of hydrogen gas to moles of the metal (X), using the balanced equation.
CRED
X (s) + 2 HCl (aq) → XC12 (aq) + H₂ (g)
= 0.00076m0lX
Calculate the molar mass of the metal (g/mol) and identify the metal.
O.13079x171.97g/mol
mL
0.019
292,
220R=0.0821 La
-0.00076 mol X
mc
moles X: 0.00076
Metal:
L
atm
latm: 760mmHg
K
Molar mass: 171.97
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