pter 5: Gases eral Chemsitry : Tro T, name: Emory Peacock - A 38.0 L tank at 35 C has nitrogen at a pressure of 4,65 atm. The contents of the tank are transferred without loss to an evacuațed 55.O L tank in a cold room where the temperature is 4 C. What is the pressure n the tankt 15-308.15k I5:277.14K )(38L -P?!SGL) 2.89 atm -P2 3018.15k 277.15K 2. A piece of dry ice (CO2) has a mass of 22.50 g. It is dropped into a evacuated 2.50L flask. What is the pressure in the flask at -4 C? PV=nRT mass- 22.509 Imol P(2.GOL)=(,611)608204l(264.1614) :てろ16946 209.15 각4-이14..511 mols 2.50L P=4.51atm 3. Calculate the density of ammonia at 75 C and 1.31 atm. d=PMIRT Ammouia : NHz (1.3)(17.041) 12.52 N: 14.01 H: 3.03 %3D d=.7819/11 31 atm 13.115-348.15りK 4. Cyclopropane mixed in a proper ration with oxygen can be used as an anesthetic. At 755mmHg and 25 C, it has a density of 1.71g/L. What is the molar mass? 7u0-.093 (.08206)(348.15k)=2%.67 d= PM/RT (1.7) 13.15=298.19 71g/L 5. Phosgene is a highly toxic gas made up of carbon, oxygen, and chlorine gas. Its density at 1.05 atm and 25 C is 4.24 g/L. What is the molar mass? 6. Nitric Acid can be prepared by bubbling dinitrogen pentoxide into water to the following equation: N2O5 () + H2O → 2H* + 2NO3 How many moles of H* are obtained when 1.50L of N2O5 at 25 C and 1.00 m pressure is bubbled into water? 7. Calcium reacts with water to produce gas and aqueous calcium hydroxide. Write the balanced equation. How many ml of water (d-1.00g/ml) are required to produce 7.00L of dry hydrogen gas at 1.05atm and 32 C?
pter 5: Gases eral Chemsitry : Tro T, name: Emory Peacock - A 38.0 L tank at 35 C has nitrogen at a pressure of 4,65 atm. The contents of the tank are transferred without loss to an evacuațed 55.O L tank in a cold room where the temperature is 4 C. What is the pressure n the tankt 15-308.15k I5:277.14K )(38L -P?!SGL) 2.89 atm -P2 3018.15k 277.15K 2. A piece of dry ice (CO2) has a mass of 22.50 g. It is dropped into a evacuated 2.50L flask. What is the pressure in the flask at -4 C? PV=nRT mass- 22.509 Imol P(2.GOL)=(,611)608204l(264.1614) :てろ16946 209.15 각4-이14..511 mols 2.50L P=4.51atm 3. Calculate the density of ammonia at 75 C and 1.31 atm. d=PMIRT Ammouia : NHz (1.3)(17.041) 12.52 N: 14.01 H: 3.03 %3D d=.7819/11 31 atm 13.115-348.15りK 4. Cyclopropane mixed in a proper ration with oxygen can be used as an anesthetic. At 755mmHg and 25 C, it has a density of 1.71g/L. What is the molar mass? 7u0-.093 (.08206)(348.15k)=2%.67 d= PM/RT (1.7) 13.15=298.19 71g/L 5. Phosgene is a highly toxic gas made up of carbon, oxygen, and chlorine gas. Its density at 1.05 atm and 25 C is 4.24 g/L. What is the molar mass? 6. Nitric Acid can be prepared by bubbling dinitrogen pentoxide into water to the following equation: N2O5 () + H2O → 2H* + 2NO3 How many moles of H* are obtained when 1.50L of N2O5 at 25 C and 1.00 m pressure is bubbled into water? 7. Calcium reacts with water to produce gas and aqueous calcium hydroxide. Write the balanced equation. How many ml of water (d-1.00g/ml) are required to produce 7.00L of dry hydrogen gas at 1.05atm and 32 C?
Chemistry
10th Edition
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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Calculate the density of ammonia at 75 C and 1.31 atm.
Transcribed Image Text:pter 5: Gases
eral Chemsitry : Tro
T,
name: Emory Peacock
- A 38.0 L tank at 35 C has nitrogen at a pressure of 4,65 atm. The contents of the tank are transferred without
loss to an evacuațed 55.O L tank in a cold room where the temperature is 4 C. What is the pressure n the tankt
15-308.15k
I5:277.14K
)(38L
-P?!SGL)
2.89 atm
-P2
3018.15k
277.15K
2. A piece of dry ice (CO2) has a mass of 22.50 g. It is dropped into a evacuated 2.50L flask. What is the pressure in
the flask at -4 C? PV=nRT
mass- 22.509 Imol
P(2.GOL)=(,611)608204l(264.1614)
:てろ16946
209.15
각4-이14..511
mols
2.50L
P=4.51atm
3. Calculate the density of ammonia at 75 C and 1.31 atm.
d=PMIRT Ammouia : NHz (1.3)(17.041) 12.52
N: 14.01
H: 3.03
%3D
d=.7819/11
31 atm
13.115-348.15りK
4. Cyclopropane mixed in a proper ration with oxygen can be used as an anesthetic. At 755mmHg and 25 C, it has
a density of 1.71g/L. What is the molar mass?
7u0-.093
(.08206)(348.15k)=2%.67
d= PM/RT (1.7)
13.15=298.19
71g/L
5. Phosgene is a highly toxic gas made up of carbon, oxygen, and chlorine gas. Its density at 1.05 atm and 25 C is
4.24 g/L. What is the molar mass?
6. Nitric Acid can be prepared by bubbling dinitrogen pentoxide into water to the following equation:
N2O5 () + H2O → 2H* + 2NO3 How many moles of H* are obtained when 1.50L of N2O5 at 25 C and 1.00
m pressure is bubbled into water?
7. Calcium reacts with water to produce gas and aqueous calcium hydroxide. Write the balanced equation. How
many ml of water (d-1.00g/ml) are required to produce 7.00L of dry hydrogen gas at 1.05atm and 32 C?
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