Mass of Mg ribbon(g): trial 1__0.035__ Volume of H2 collected(mL)__35.3__ Temperature of H2(g) (ºC)__23.0 Atmospheric pressure(torr)__756.0__ Vapor pressure of water(torr)__3.02__ Volume of H2 gas in liters(L)__0.0353 Temperature of H2 gas in Kelvin(K)__296ºK What is the Moles of H2gas(mol),pressure of H2 gas in atmosphere(atm) and the experimental value of R

How many moles (n2) remain in the cylinder?

QUESTION 9 Complete the following table for data collected at 80°C. Temperature   80°C     Temperature T    K   Report your answer to 2 decimal places Volume of Gas Bubble   7.8 mL     Volume V    L   Report your answer to 2 significant figures Height of the Water Column, h   88 mm     Mercury Equivalent of Water (MEW)     mm   Report your answer to 2 significant figures Barometric Pressure, Pbarometric   764.6 torr     Total Pressure of the Enclosed Gas Sample Ptotal    torr   Report your answer to 1 decimal place Partial Pressure of Air in the Gas Sample, Pair    torr   Report your answer to 1 decimal place Vapor Pressure of Water in the Gas Sample, Pwater    torr   Report your answer to 1 decimal place Natural log of the Vapor Pressure of Water in the Gas Sample, ln (Pwater)    torr   Report your answer to 2 decimal places Reciprocal of Temperature 1/T    K−1   Report your answer to 3 significant figures

At a temperature of __________°C, 0.444 mol of CO gas occupies 11.8L at 839 torr.

15. A fuel-air mixture contains 0.5 mol CH4(g), 1.5 mol 02(g), and 6.0 mol N2(g), under a total pressure Ptot = 25 atm. Find the partial pressure of 02(g) in it: A) 25 atm B) 0.063 atm C) 1.6 atm D) 19 atm E) 4.7 atm

Use Boyle's law to complete the following table (assume temperature and number of moles of gas to be constant).  P1P1 V1V1 P2P2 V2V2 _____ 2.00 LL 4.30 atmatm 1.05 LL 757 mmHgmmHg 119 mLmL 708 mmHgmmHg _____ 2.70 atmatm 5.06 mLmL _____ 49.8 mLmL 345 torrtorr _____ 689 torrtorr 7.79 LL   Complete the fourth column of the table.

At what temperature (in K) would 1.88 moles of H2 gas have a pressure of 0.94 atm and take up a space of 15.3 L?  (Do NOT put units in the answer box).R= 0.08206 L atm/mol K R= 8.3145 L kPa/mol K

A sample of gas contains 0.1800 mol of and 0.09000 mol of and occupies a volume of 11.9 L. The following reaction takes place:2HCI(g) +Br_2(g) --->2HBr(g) +Cl_2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = ___ L

A 22.1 mL sample of H2 gas was collected from an experiment at 1.059 atm and 23.5 °C. How many moles of gas are in this sample?

Use Charles's law to complete the table. (Assume pressure and number of moles of gas to be constant.)   Part V1V1 T1T1 V2V2 T2T2 A 117 LL 10.5 ∘C∘C __ 122.0 ∘C∘C B __ 133 KK 174 LL 319 KK C 2.08 LL 14.5 ∘C∘C 2.33 LL __ D 16.2 cm3cm3 __ 18.9 cm3cm3 11.1 ∘C∘C   Complete the first row of the table. Express the volume in liters to three significant figures.