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Quiz 4-26-12. Answers. 2.30 g Na are reacted with 100.0 mL of 0.10 M phosphoric acid. Calculate the number of liters of hydrogen gas formed at STP. 6 Na + 2H 3 PO 4 3 H 2 + 2 Na 3 PO 4. 2.30 g Na. 1 mole Na. 3 mole H 2. 22.4 L H 2. = 1.12 L H 2. 23.0 g Na. 6 mole Na. 1 mole H 2. - PowerPoint PPT Presentation
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Quiz 4-26-12
Answers
2.30 g Na are reacted with 100.0 mL of 0.10 M phosphoric acid. Calculate the number of liters of hydrogen gas formed at STP.
6 Na + 2H3PO4 3 H2 + 2 Na3PO4
2.30 g Na 1 mole Na
23.0 g Na
3 mole H2
6 mole Na
22.4 L H2
1 mole H2
= 1.12 L H2
2.30 g Na are reacted with 100.0 mL of 0.10 M phosphoric acid. Calculate the number of liters of hydrogen gas formed at STP.
6 Na + 2H3PO4 3 H2 + 2 Na3PO4
0.100 L H3PO4 0.1 mole H3PO4
1L H3PO4
3 mole H2
2 mole H3PO4
22.4 L H2
1 mole H2
= 0.336 L H2
When you actually perform the experiment, you get 0.30 L of H2. What is the percent yield.
• The two values for the volume of H2 were 0.336 L and 1.12 L of H2
• 0.336 L is the theoretical yield. 1.12 is just wishful thinking.
• 0.30 L is the actual yield.
Actual yield
theoretical yieldX 100 %
0.30 L H2
0.336 L H2
= 89%
A 0.336 L of sample of hydrogen gas at STP is heated to 23oC at 745 mm Hg.Calculate the volume of the gas at room temperature.
Identify the variablesV1 = 0.336 LT1 = 273 KP1 = 760 mm HgT2 = 23 + 273 = 296 KP2 = 745 mm HgV2 = ?
P1V1
=
P2V2
T1 T2
V2
P1 V1 T2
T1P2
(760 mm Hg)
=
(0.336 L) (296 K)
(273 K)(745 mm Hg)
0.372 L =