A 36.8 g sample of N204 was heated in a closed flask of volume 16.0 L. An equilibrium was established at a constant temperature according to the following equation. N204(g) 2NO2@) The equilibrium mixture was found to contain 0.180 mol of Ng04 a. Write an expression for Kç and calculate its value under these conditions. b. Another 36.8 g sample of N:O4 was heated to the same temperature as in the original experiment, but in a larger flask. State the effect, if any, of this change on the position of equilibrium and on the value of Kc compared with the original experiment.

A 36.8 g sample of N204 was heated in a closed flask of volume 16.0 L. An equilibrium was established at a constant temperature according to the following equation. N204(g) 2NO2@) The equilibrium mixture was found to contain 0.180 mol of Ng04 a. Write an expression for Kç and calculate its value under these conditions. b. Another 36.8 g sample of N:O4 was heated to the same temperature as in the original experiment, but in a larger flask. State the effect, if any, of this change on the position of equilibrium and on the value of Kc compared with the original experiment.

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

Subm leating N2O4(g) at some constant temperature causes some of this compound to decompose, forming NO2(g). Eventually, the amounts of the species do not change furthe ne system has reached equilibrium. (At this point, only part of the N204 has decomposed.) What is happening in this system at the molecular level? O NO2 (g) molecules collide with N2O4(g) making the reaction stop. O NO2(g) reacts to produce N204(g) at the same rate as it decomposes. O Only part of the N2O4(g) molecules has enough energy to decompose at this temperature. 7:29 PM als-asp.cengage.info/als-asp/take 82°F 9/15/2021 e Type here to search insert 144
- Bromine monochloride is synthesized using the reaction Br2(g) + Cl2(g) 2 BrCl(g) Kp = 1.1 x 104 at 150 K A 209.0 L flask initially contains 1.100 kg of Br2 and 1.053 kg of Cl₂. Calculate the mass of BrCl, in in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? percent yield: grams, that is present g %
At a certain temperature, 0.347 mol CH, and 0.619 mol H,S are placed in a 2.50 L container. CH,(g) + 2 H, S(g)= CS, (g) + 4 H,(g) At equilibrium, 11.8 g CS, is present. Calculate K.. K. =
The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M
Phosphorus pentachloride decomposes according to the chemical equation PC15(g) PC13(g) + Cl₂(g) Kc = 1.80 at 250 °C A 0.1584 mol sample of PC1, (g) is injected into an empty 2.00 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PC13 (g) at equilibrium.
A student adds 0.600 mol of methane gas, CH4(g) into a 2.00 L container and the methane forms ethyne, C2H2(g) and hydrogen gas, H2(g). At equilibrium, the container was found to contain 0.045 mol/L C2H2.a) Calculate the initial concentration of CH4. Then complete an ICE Table to organize the initial, change and equilibrium concentrations for this equilibrium system. Show any calculations needed. 2CH4(g) ⇄ C2H2(g) + 3H2(g)b) Calculate the equilibrium constant, Keq, for this equilibrium. Show all work.c) What is the equilibrium concentration of H2(g) ?
Please don't provide handwritten solution ....
At a certain temperature, 0.760 mol SO, is placed in a 2.50 L container. 2 SO,(g) = 2 SO2(g) + O,(g) At equilibrium, 0.120 mol O, is present. Calculate K.. Ke
LRererencesj Isoidan 1 Use the References to access important values if needed for this question. Consider the following equilibrium system at 844 K. 2HI(8) 2 H2 (g) + L (g) If an equilibrium mixture of the three gases at 844 K contains 0.196M HI, 3.37 × 10-2 M H2, and 2.80 × 10- M I2, what is the value of the equilibrium constant K?
An equilibrium mixture of SO2,O2,and SO3 at high temperature contains the gases at the following concentrations: SO2 =3.17*10-3 mol/L,O2=4.83*10-3 mol/L and SO3=4.50*10-3 mol/L.Calcualte the equilibrium constant,Kc,for the reaction. 2SO2(g) + O2(g)=2SO3(g) Kc= please solve