The vapor pressure of liquid methanol, CH3OH, is 100. mm Hg at 294 K. A 0.116 g sample of liquid CH3OH is placed in aclosed, evacuated 490. mL container at a temperature of 294 K.Assuming that the temperature remains constant, will all of the liquid evaporate?What will the pressure in the container be when equilibrium is reached?mm HgSubmit AnswerRetry Entire Group9 more group attempts remainingThe vapor pressure of liquid octane, CgH18, is 100. mm Hg at 339 K.A sample of C8H18 is placed in a closed, evacuated 516 mL container at a temperature of 339 K. It is found that all of theCSH18 is in the vapor phase and that the pressure is 53.0 mm Hg. If the volume of the container is reduced to 351 mL atconstant temperature, which of the following statements are correct?Choose all that applyO Some of the vapor initially present will condense.O The pressure in the container will be 100. mm Hg.O No condensation will occur.OLiquid octane will be present.OOnly octane vapor will be present.The vapor pressure of liquid carbon disulfide, CS2, is 40.0 mm Hg at 251 K.A sample of CS2 is placed in a closed, evacuated container of constant volume at a temperature of 376 K. It is found that all ofthe CS2 is in the vapor phase and that the pressure is 73.0 mm Hg. If the temperature in the container is reduced to 251 K,which of the following statements are correct?Choose all that apply.OSome of the vapor initially present will condense.O Only carbon disulfide vapor will be present.O No condensation will occur.O The pressure in the container will be 48.7 mm Hg.O Liquid carbon disulfide will be present.

Since you have posted multiple questions, I am going to answer the first one only as per the…

The vapor pressure of liquid methanol, CH3OH, is 100. mm Hg at 294 K. A 0.116 g sample of liquid CH3OH is pla closed, evacuated 490. mL container at a temperature of 294 K. Assuming that the temperature remains constant, will all of the liquid evaporate? What will the pressure in the container be when equilibrium is reached? mm Hg Submit Answer Retry Entire Group 9 more group attempts remaining

The vapor pressure of liquid methanol, CH3OH, is 100. mm Hg at 294 K. A 0.116 g sample of liquid CH3OH is pla closed, evacuated 490. mL container at a temperature of 294 K. Assuming that the temperature remains constant, will all of the liquid evaporate? What will the pressure in the container be when equilibrium is reached? mm Hg Submit Answer Retry Entire Group 9 more group attempts remaining

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

As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
3sa
The equilibrium constant, K,, for the following reaction is 2.74 at 1.15x1o3K. 2503(g) 2s02(g) + 02(g) If an equilibrium mixture of the three gases in a 16.5 L container at 1.15×103K contains soz at a pressure of 1.62 atm and So, at a pressure of 1.04 atm, the equilibrium partial pressure of O, is atm.
At a certain temperature, 0.389 mol CH4 and 0.606 mol H₂S are placed in a 3.00 L container. CH₂(g) + 2 H₂S(g) = CS₂(g) + 4H₂(g) At equilibrium, 12.3 g CS₂ is present. Calculate Kc. 2 Вс =
How increasing the total pressure by compressing the gases would change the shift of the equilibrium?
Question 8 of 21 > At a certain temperature, 0.301 mol CH, and 0.688 mol H₂O is placed in a 2.50 L container. CH₂(g) + 2 H₂O(g) = CO₂(g) + 4H₂(g) At equilibrium, 8.71 g CO, is present. Calculate K. K₂ = Check Answer 53
P
Review Topics] A researcher put 0.320 mol PCI3 and 0.192 mol Cl2 into a 2.10 L vessel at a given temperature to produce phosphorus pentachloride, PC1 : References] PC13 (g) + Cl2 (9) PC15 (g) What will be the composition of this gaseous mixture at equilibrium? K. = 25.6 at the temperature of this experiment. [PCl3] = M [Cl2] =| [PCI5] = Retry Entire Group 7 more group attempts remaining Submit Answer Previo
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S₂(g) + C(s) CS₂(g) Kc = 9.40 at 900 K How many grams of CS₂(g) can be prepared by heating 13.4 mol S₂(g) with excess carbon in a 5.65 L reaction vessel held at 900 K until equilibrium is attained? mass of CS₂(g): 6.0 g
Predict the effect if the partial pressure of PCl5(g) is increased using the following equation. PCl3(g) +Cl2(g)⟶ PCl5(g) Group of answer choices A decrease in partial pressure of phosphorous trichloride and phosphorous pentachloride. Shift left. Shift right. No effect. An increase in partial pressure of phosphorous trichloride and phosphorous pentachloride.
Part A An equilibrium mixture contains N2O4, (P = 0.27 atm ) and NO2 (P = 1.0 atm ) at 350 K. The Calculate the equilibrium pressure of N204 when the system reaches a new equilibrium. volume of the container is doubled at constant Express your answer using two significant figures. temperature. 响 AX中画] ? P = atm Submit Request Answer Part B Calculate the equilibrium pressure of NO2 when the system reaches a new equilibrium. Express your answer using two significant figures. ΑΣφ. 画] ? P = atm
Same question