Nitrogen dioxide is a component in smog. Nitrogen dioxide is yellow/brown. Its dimer, dinitrogen tetroxide is colorless. 2 NO₂ (g) N₂O4 (9) Brown → colorless 1. Does placing the tube into a hot water bath cause the brown color to increase or decrease? 2. Does adding heat shift the reaction to the right or to the left? 3. Does placing the tube into an ice water bath cause the brown color to increase or decrease?

Nitrogen dioxide is a component in smog. Nitrogen dioxide is yellow/brown. Its dimer, dinitrogen tetroxide is colorless. 2 NO₂ (g) N₂O4 (9) Brown → colorless 1. Does placing the tube into a hot water bath cause the brown color to increase or decrease? 2. Does adding heat shift the reaction to the right or to the left? 3. Does placing the tube into an ice water bath cause the brown color to increase or decrease?

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 following amounts of HI, H2, and I2 are introduced into a 10.00 L flask and are heated to 745 K. mol of HI mol of H2 mol of I2 Case A 1.0 0.10 0.10 Case B 15.0 1.0 1.0 Case C 10.0 10.0 1.0 Case D 5.5 0.38 1.75 The equilibrium constant for the reaction 2HI (g) ↔ H2 (g) + I2 (g) is 0.0200 at 745 K. In which cases will the concentration of HI increase as equilibrium is attained and in which cases will the concentration of HI decrease?
Question 24 Which statement is true for a reaction with Kc equal to 8.90 x 10 122 O The reaction proceeds nearly all the way to completion. O The reaction proceeds hardly at all towards completion. O There are appreciable concentrations of both reactants and products. Increasing the temperature will not change the value of K.
1. If a reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.179 M at 1000 K. What is the equilibrium concentration of CO at 1000 K? 2. What is the equilibrium concentration of Cl2 at 1000 K? 3. What is the equilibrium concentration of COCl2 at 1000 K? Thank you so much! These three questions bothered me for so long.
Question #8. Le Chaterliers Principle Experiments Consider the following fully reversible reaction: A(g) + B(g) ↔ C(g). How many moles of gas are on the left-hand side of the reaction?
Explain why please?
I need help with this questions and show the work step by step?
What effect does each of the following changes have on the equilibrium of the reaction: (left or right) C(s) + H₂O(g) + heat ⇒ CO (g) + H₂ (g) a. add H₂ b. lower temperature c. add H₂O d. remove CO
A Moving to another question will save this response. Question 11 The equilibrium constant for the reaction N204 (g) 2 2 NO2 (g) is 0.200 at 65 °C. Calculate AG° for this reaction. O +4.52 kJ/mol O +0.479 kJ/mol -0.479 kJ/mol -4.52 kJ/mol O 0.00 kJ/mol A Moving to another question will save this response. MacBook Air 吕口 F3 esc F4 F5 F1 F2 #3 $. & 3. 6. Q W E R.
The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. N2O4(g) = 2NO2 (g) Kc = 1.46 5N2O4(g) = 10NO2 (g) K. = ? %3D 0.322 O 5.40 O 1.46 O 1.13 O 6.63
If 50 kJ of energy are absorbed when 25 g of Ca(OH) 2 are dissolved in water. How much energy would be absorbed with 1.5 mol of Ca(OH)2 is dissolved in water? 3 kJ 222.3 kJ 75 kJ 3000 kJ 111.15 kJ
Assuming the system is already at equilibrium, predict whether each of the following changes will cause the amount of CO2(g) to increase, decrease, or stay the same. 2 NaHCO3(s) <-> Na2CO3(s) + H2O(g) + CO2(g) H°= + 91.6 kJ/mol a. Increase the amount of NaHCO3(s)b. Increase the amount of Na2CO3(s)c. Increase the amount of H2O(g)d. Decrease the temperaturee. Addition of HCl (which catalyzes this reaction)f. Increase the volume of the reaction container
For each pair, write a balanced chemical equation with states of matter describing the reaction that takes place.