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The mass of of an unknown gas sample is . It is collected by water displacement in a eudiometer tube at a temperature of and a barometric pressure of . It is carefully placed into a larger cylinder with water. The water level inside the tube is lower than the water level outside the tube. What is the partial pressure of the unknown gas? The number of moles of the unknown gas and the molecular mass of the gas?

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Related questions

ldeal Gas Law: Stoichiometry I. OBJECTIVES 1. To measure the mass of gas produced using temperature, pressure and volume 2. To calculate the theoretical yield of gas from starting quantities 3. To determine the percent yield of gas To understand partial pressure and mole fractions of gases II. PROCEDURES Wear Safety Glasses Weigh a short strip of magnesium ribbon on an analytical balance. If the mass of the ribbon is greater than 0.045 g, shorten the ribbon to reduce its mass to 0.045 g or less. Record the mass 2. Use a thistle tube to add 15 mL of 3 M hydrochloric acid (table top) to a cudiometer tube. 3. While holding the eudiometer tube at an angle to minimize mixing of the acid at the bottom, add deionized water to fill it within a centimeter of the end 4. Use forceps to push one of the magnesium strips into the open end of the eudiometer tube (like a small spring) so that it will not fall out when the tube is inverted 5. Finish filling the eudiometer tube completely with water so no air bubble will be formed when it is inverted. Also add at least 350 mL. (but not more than 400 mL) of tap water to a 400-mL beaker With a finger solidly over the open end of the filled eudiometer tube, invert it into the beaker nearly filled with tap water so that no water runs out of the eudiometer tube when the open end is released. If the magnesium ribbon falls out of the tube, trap it under the tube completely before bubbles start to form. 6. 7. Hold the eudiometer tube upright (either by hand or with a ring stand) until the magnesium ribbon completely reacts. If the magnesium stays at the bottom, the reaction will run faster if the tube is tilted away from vertical by about 30 degrees. If the magnesium floats to the surface, it is probably better to hold the tube straight up. Wiggle the tube as necessary to keep the n from sticking to the side above the water line 8. When the reaction is complete, transfer the eudiometer tube (with finger over the end) to a tall cylinder of water. Read and record the volume of gas in the eudiometer tube when the water levels are the same inside and outside the tube. Notice the scale increases going down the tube. 9. Repeat proedures 1 through 8 for the second trial 10. Obtain the barometric pressure in the room and record the valu 11. Measure the temperature of the water in the tall cylinder and look up the vapor pressure of water for that temperature. Assume this is the temperature of the gas at the volume and pressure measured.

As a result of the reaction between a nitrite compound and sulfamic acid, a 43.7 mL sample of nitrogen was collected over water at 24.0 degrees Celsius. The height of the water column inside the eudiometer tube was 126.9 mm higher than the surface of the water in the surrounding beaker. Barometric pressure was 739.2 torr.

1. Show your work in finding the partial pressure of the nitrogen gas, P_N2â¢

2. Show your work in finding the mass of the nitrogen collected.

3. The original sample, which decomposed to produce the nitrogen gas, weighed 0.1198 g. find the percent nitrogen in the sample.

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