Suppose you want to calculate the number of moles of a gas released from a chemical reaction based on the ideal gas law equation. In the lab, you observe that 17.4 mL of gas are released at a temperature of 25.4°C and a pressure of 991 Torr. You begin calculations using the value for R as 0.08206 L'atm mol-K Next, convert the remaining values to units suitable for use in this equation.

Suppose you want to calculate the number of moles of a gas released from a chemical reaction based on the ideal gas law equation. In the lab, you observe that 17.4 mL of gas are released at a temperature of 25.4°C and a pressure of 991 Torr. You begin calculations using the value for R as 0.08206 L'atm mol-K Next, convert the remaining values to units suitable for use in this equation.

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...

See similar textbooks

Similar questions

The balanced equation for the chemical equation is Mg+2HCl->MgCl2+H2 If the student used an excess of hcl to dissolve 0.045 grams of pure Mg ribbon, and collected the gas in a test tube over water how much H2 gas could she produce, calculate the answer in moles.
If pressure is expressed in atmospheres and volume is expressed in liters, PAV has units of L atm (liters x atmospheres). Remember that 1 atm = 101,325 Pa, and that 1 L = 1 dm. Use this information to determine the number of joules corresponding to 5 L atm. i J
A 8.00 L tank at 17.5 °C is filled with 12.8 g of chlorine pentafluoride gas and 4.02 g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. olo mole fraction: chlorine pentafluoride partial pressure: atm Ar mole fraction: carbon dioxide partial pressure: atm Total pressure in tank: atm
Consider the complete combustion of glucose (C6H12O6) with O2 and calculate the moles of CO2produced when 1.02 g of glucose is reacted with 25 mL of O2 at body temperature (37 ºC) and 0.970 atm. C6H12O6 + 6 O2 (g) → 6 CO2 (g) + 6 H2O a. 0.95 b. 0.0022 c. 9.53 x 10-4 d. 6.33 x 10-2 e. 5.67 x 10-3
For many purposes we can treat propane (C,Hg) as an ideal gas at temperatures above its boiling point of -42. °C. Suppose the temperature of a sample of propane gas is raised from -20.0 °C to 21.0 °C, and at the same time the pressure is changed. If the initial pressure was 1.5 atm and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits. atm x10
Suppose you want to calculate the number of moles of a gas released from a chemical reaction based on the ideal gas law equation. In the lab, you observe that 11.3 mL of gas are released at a temperature of 25.6°C and a pressure of 922 Torr. You begin calculations using the value for R as 0.08206 Latm mol-K Next, convert the remaining values to units suitable for use in this equation. T= atm 關
X 12 13 Por many purposes we can treat nitrogen (N,) as an ideal gas at temperatures above its boiing point of -196. "C. Suppose the temperature of a sample of nitrogen gas is raised from -25.0 "C to 13.0 "C, and at the same time the pressure is changed. ir the intial pressure was 3.2 atm and the volume decreased by 30.0%, what is the final pressure? Round your answer to 2 significant digits atn D.P
Consider the following samples of gas: sample composition pressure temperature A 2.0mol Xe (g) 1.7atm 228.°C B 2.0mol Xe (g) 1.4atm 258.°C C 2.0mol Xe (g) 1.6atm 280.°C sample composition pressure temperature D 1.5mol He (g) 1.5atm 41.°C E 1.5mol Ar (g) 2.4atm 41.°C F 1.5mol Ne (g) 1.2atm 41.°C Draw the set of graphs below that show the distributions of the speed of the atoms in each sample.
7. When detern ing the mass of a liquid, ras in a hurry and did not allow enough time for the temperature of the flask to reach the temperature of the boiling water bath. The student recorded the temperature of the gas as 100.0°C when it was only 80.0°C, Is the molar mass calculated by the student higher or lower than the accepted molar mass, or does this error have no effect on the calculated result? Briefly explain your answer # 2/HB Office DEPOTS b) If the student assumed the volume of the flask was 125 mL (as marked by the side of the flask) rather than measuring the volume experimentally, would the unknown's calculated molar mass be too high, too low, or unaffected? Explain. # 2/HB 4
The ideal gas law, R, can be experimentally determined. Use the data provided below from the reaction of potassium chlorate decomposing to form oxygen gas and potassium chloride to experimentally determine the value of R in units of L•atm/mol•K. 2KClO3 (s) → 2KCl (s) + 3O2 (g) The evolved oxygen is collected over water. The relevant data from the experiment is summarized below. Mass of KClO3 used 0.0665 g Initial volume reading 46.0 mL Final volume reading 64.2 mL Temperature 22.0°C Total pressure 772.0 mm Hg A table of vapor pressures of water is also available: Temperature (°C) Vapor Pressure of Water (mm Hg) 21 18.7 22 19.8 23 21.1 24 22.4 25 23.8 What is the volume (in L) of O2 gas formed in the experiment? What is the dry pressure (in mm Hg) of O2 gas in the experiment? What is the dry pressure (in atm) of O2 gas in the experiment? What is the temperature (in K) for the experiment? How many moles of KClO3 were used in this…
Use the ideal gas equation to calculate the number of moles of hydrogen gas produced from a reaction between hydrochloric acid, HCl, and magnesium metal in which 12.0 liters of gas was collected at 22.0 C with a barometric pressure of 761.09 torr. The gas was collected over water with a vapor pressure pf 19.83 torr. R= 82.1 atm mL/mol K or R= 0.0821 atm mL/mol K
BIOL 1603: Org & Evol - Google x A ALEKS - Katie Matthews - Grac x Content app.101edu.co → C esc 1 F1 A glass container was initially charged with 1.50 moles of a gas sample at 5.00 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 33.1 °C, so the final pressure in the container was reduced to 1.50 atm. How many moles of the gas sample are present at the end? Q 2 F2 W # 3 80 E $ 4 F4 R % 675 뽀 F5 T 6 X Question 38 of 66 F6 Y Aktiv Chemistry & 7 F7 U * 00 8 DII F8 ( 1 9 X a Amazon.com: wireles F9 0 1 2 4 7 +/- 0 7 F10 5 8 P