
please help due tonight 2. Calculate the quantity of a gas, in moles, if 45 L...
due tomorrow please help
At 298 K, a 5.0-L flask contains 0.15 mol of O, and 0.22 mol of N. Calculate the partial pressure of N2 inside the container. (note: the ideal gas constant is 0.0821 L atm/mol K) (4 points)
Please help with these two
1. A flask is filled with 1.08 moles of a gas at 20.7 K and
646.8 mm Hg. The flask is then opened and an additional 1.33 moles
are added. The temperature of the flask is then changed to 272.4 K.
What is the pressure (in atm) of the flask under these final
conditions?
2. The density of a gas is 4.22 g/L at a pressure of 1.77 atm
and a temperature of 14.66 °C. What...
Data provided
solve Q3 and Q4 please
Table 2. Experimental Data Trial 1 Trial 2 Trial 3 30.13 Atmospheric Pressure (inches Hg) Mass Mg used (8) 0.039 0.025 0.011 39.58 25.89 11.47 Volume Hz gas generated (mL) Water Temperature (°C) 19.0 19.0 19.0 16.48 16.48 16.48 Partial Pressure Water Vapor (mm Hg; from Table 1) Difference in Water Levels (mm) 14.31cm 35.72cm 46.13cm Table 3. Molar Gas Volume and Ideal Gas Constant Calculations Trial 1 Trial 3 Trial 2 Trial...
QUESTION 2 What amount (in moles) of a gas is contained in 40.4 L at-82.4 °C with a pressure of 527.4 mm Hg? QUESTION 3 A flask is filled with 1.03 moles of a gas at 13.4 K and 618.9 mm Hg. The flask is then opened and an additional 1.84 moles are added. The temperature of the flask is then changed to 172.9 K. What is the pressure (in atm) of the flask under these final conditions? QUESTION 4...
data provided
please solve Q5 & Q6
Q4 answer
Table 2. Experimental Data Trial 1 Trial 2 Trial 3 30.13 Atmospheric Pressure (inches Hg) Mass Mg used (6) 0.039 0.025 0.011 Volume Hz gas generated (mL) 39.58 25.89 11.47 Water Temperature (°C) 19.0 19.0 19.0 16.48 16.48 16.48 Partial Pressure Water Vapor (mm Hg: from Table 1) Difference in Water Levels (mm) 14.31cm 35.72cm 46.13cm Table 3. Molar Gas Volume and Ideal Gas Constant Calculations Trial 1 Trial 2 Trial...
Suppose you have a fixed container containing 0.255 moles of a gas (the identity of the gas doesn't matter). If the container volume is 0.748 L, and the temperature is 301.15 K, what is the pressure in atm? (R=0.0821 L'atm/mol-K) O A.0.784 atm OB. 0.00842 atm O C.7.84 x 104 atm D.8.42 atm
A sealed 89,98-m3 tank is filled with 5 265 moles of oxygen gas (O2) at an initial temperature of 293,38 K. The gas is heated to a final temperature of 397,1 K. The ATOMIC mass of oxygen is 16.0 g/mol, and the ideal gas constant is R = 8.314 J/mol · K = 0.0821 L · atm/mol · K. Calculate the initial pressure (MPa) of the gas. Answer in two decimal places.
Suppose you have a fixed container containing 2.48 moles of gas. If the container volume is 30.0L, and the pressure is 2.05 atm, what is the temperature (°C)? (R=0.0821 L'atm/mol-K) A.-84.0°C B. 302°C C. 29.0°C 0.189 °C
1a) Calculate the Volume in L of 1.2 moles of CH4 confined in a container at a pressure of 10 atm at 323 K. Use the ideal gas equation. C=12 g/mol H= 1 g /mol T(K)= T(°C)+273.15 R=0.0821 L-atm/mol-K PV=nRT answer a)0.318 b)90.2 c)3.18 d)31.8 1b) Is the number of particles or spheres in the cubic cell centered on the body? answer 1)3 2)4 3)1 4)2 3c) in the solid state does it form molecular crystals answer a)NaCL b)graphite c)CO2...
BG20.2 Determination of the Ideal Gas Law Constant Page 9 of 12 PRELAB QUESTIONS (Show all calculations.) I. Write a balanced chemical equation for the reaction of magnesium with hydrochloric acid. 2. A class ran this lab as described above. One student cut a piece of magnesium ribbon and found that it weighed 0.0347 g. The magnesium reacted with the 4.0 mL of concentrated hydrochloric acid. The concentration of concentrated hydrochloric acid is 12 mol/liter. Which reactant is the limiting...