Calculate the total partial pressures of H2 and N2 in a reaction vessel of volume 24.4 dm3 containing 1.0 mol H2 and 2.5 mol N2 at292.15 K.O A. PN = 1.5 atm, PH = 4.0 atmO B. PN = 3.5 atm; PH = 2.5 atmOCPN= 1.5 atm, PH = 2.5 atmOD. PN = 4.0 atm; PH = 1.5 atmO E. PN = 2.5 atm, PH = 1.5 atm

Answered: Image /qna-images/answer/7b67dbfb-81b9-4b73-a58c-28b281310310.jpg

Answered: Calculate the total partial pressures…

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 equilibrium constant Kc for the reaction N2(g) + O2(g)⇋ 2NO(g) at 1200 degrees Celsius is 1.00 x 10-5. Calculate the equilibrium molar concentrations of NO, N2, O2 in a reaction vessel of volume 10.00 L that initially held 0.312 mol N2 and 0.407 mol O2.
Calculate mole fraction of each component in a reaction vessel of volume 24.4 dm containing 1.0 mol H2 and 2.5 mol N2 at 298.15 K. OA.XN = 0.63; XH=0.37 %D O B. XN = 0.25; XH= 3.5 %3D OUYND0.15; XH=0.37 OD.XN = 0.25; XH=0.63 OE. XN = 0.72; XH= 0.37
(1) (2) ] A certain species of trout requires dissolved oxygen of 7.5 mg/L. Would it be wise to release the trout in a mountain stream at an altitude with a Po2 = 0.17 atm. (KH (02) = 1.3x10-³ mol/Latm). Calculate the mole fraction for the following: 14.5 g of HNO3 in 150 g of H₂O. (b) moles of Solute kg Solvent X (a) H=1.01 N = 14.00- 50 mm= 63.01 g/mol 03=16.0x3 Imol 14.6g HNO3 63.01g 149 150 g 1000g = 0.15 kg 6.00 M HCI. (notice, concentration is an extensive property. You can assume any volume!) 0.23 mol HNO3 0.16 kg H2O 1.53 = 0.23 mol HNO3
In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. K for the reaction SbCls(g) z SÜC];(g) + Cl2(g) is 2.50 x 10 2 at 248 °C. 2.00 mol of S6CI3 and 1.00 mol of Cl, is introduced into a 4.00 L bulb at 248 °C. What are the concentrations of all three species once equilibrium is established? Enter your value for [SBCI5] in the first box and an appropriate unit of measure in the second box. Enter your value for [SBCI3] in the first box and an appropriate unit of measure in the second box. Enter your value for [Cl,] in the first box and an appropriate unit of measure in the second box. A/
For the reaction 4HCl(g) +O2(g) == 2Cl2(g) + H2O (g), Keq =889 at 480 o If 0.03 mole HCl , 0,02 mole O2 , 0.08 mole Cl2 and 0.07 mole H2O were mixed in 1 liter container, in what direction will the reaction proceed. Support your answer.
a sealed one liter reaction vessel was loaded with 0.245mol n2o and 0.574 mol o2. the system (represented by the balanced chemical equation) was allowed to reach equilibrium. where the concentration of no2 was measured to be 0.194M. 2N2O(g)+3O2(g)=4NO2. Determine the equilibrium constant (Kc) for the reaction under these conditions.
Calculate the partial pressure of O2 produced from 1.80 L of 0.576 M N2O5 solution at 45 ∘C over a period of 20.8 h if the gas is collected in a 10.3-Lcontainer. (Assume that the products do not dissolve in chloroform.)
For the following reactions, predict whether the mole fraction of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. a. SO (9) + 1/2 0,(9) = SO3 (g) O mole fraction of reactants increases O mole fraction of products increases O mole fraction remains the same b. 2HI(9) = H2 (g) + I2 (9) O mole fraction of reactants incr Omole fraction of products increases Omole fraction remains the same c. 2 H2O2(1) = 02(9) + 2 H2O(1) Omole fraction of reactants increases O mole fraction of products increases Omole fraction remains the same
- Exhaust gas from an automobile contains air and 10‐5 mole fractions of COin air at 25 degC and 1.2 atm. Express this concentration as a mass concentration (kg/m3). - If the atmosphere is 25 degC and 1.2 atm and contains 0.79 mole fractions of N2, 10‐5 mole fractions of a chemical, and a remainder of O2, what is its density (in kg/m3)?
What pressure is required to achieve a CO2 concentration of 0.0690 mol L-l at 20°C?
Consider the reaction: N2(g) + 3H2(g) 2NH3(g) where Kc = 0.500 at 400 °C. If 50.0 L reaction vessel contains 1.000 mole N₂; 3.000 mole H₂ and 0.050 mole NH3, which of the following is TRUE? The reaction based on the following parameters is in equilibrium. More ammonia will be produced as the reaction approaches equilibrium. Data provided is not enough to warrant a conclusion regarding equilibrium. More ammonia will dissociate as the reaction approaches equilibrium.
What is the mole fraction of O2 in a mixture that is 79.0 mole N2 and 21.0 mole O2? Carry only 1 decimal point on all atomic weights.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

Calculate the total partial pressures of H2 and N2 in a reaction vessel of volume 24.4 dm containing 1.0 mol H2 and 2.5 mol N2 at 292.15 K. OA PN= 1.5 atm, PH = 4.0 atm OB. PN = 3.5 atm, PH = 2.5 atm OCPN= 1.5 atm, PH = 2.5 atm OD. PN = 4.0 atm, PH = 1.5 atm OE. PN=2.5 atm, PH = 1.5 atm