4. The density of an unknown gas in a 1.00 L container at 735 torr and 25°C is 1.11 g/L. What is the molecular weight of the gas? (a) not enough information (b) 0.036 (c) 28 (d) 2.33 (e) 44 The density of ammonia gas (NH3) in a 4.32 L container at 837 torr and 45°C is ___ g/L. (a) 4.22x10?² (b) 3.86 (c) 0.432 (d) 0.717 (e) 0.194
Added by Mariano T.
Close
Step 1
\[ 735 \, \text{torr} \times \frac{1 \, \text{atm}}{760 \, \text{torr}} = 0.967 \, \text{atm} \] Show more…
Show all steps
Your feedback will help us improve your experience
Ma Ednelyn Lim and 65 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
A 3.25 g sample of an unknown gas at 79 °C and 1.05 atm is stored in a 2.75 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol A gaseous mixture contains 437.0 Torr H2(g), 365.9 Torr N2(g), and 89.3 Torr Ar(g). Calculate the mole fraction, χ, of each of these gases. χH2= χN2= χAr=
Dj T.
(a) Calculate the density of NO2 gas at 0.970 atm and 35 degrees C. (b) Calculate the molar mass of a gas if 2.50 g occupies 0.875 L at 685 torr and 35 degrees C.
Adi S.
(a) Calculate the density of sulfur hexafluoride gas at 707 torr and $21^{\circ} \mathrm{C}$ . (b) Calculate the molar mass of a vapor that has a density of 7.135 $\mathrm{g} / \mathrm{L}$ at $12^{\circ} \mathrm{C}$ and 743 torr.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD