Consider the following reaction initially at equilibrium in a fixed container at 25 °C: P4(s) + 5 O2(g) P4010 (8) If Ne(g) is introduced into the vessel, keeping the volume constant, such that the total pressure of the vessel increases, the rate of the forward reaction will and the system will 11 = If the volume of the container is cut in half, the rate of the forward reaction will and the system will -= -- -- -- When the temperature is increased, the moles of O₂(g) increase. Is the forward reaction endothern 1 Save Submit an

A chemical engineer is studying the following reaction: N2(9)+3H,(g) → 2NH,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.00029. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound pressure expected change in pressure vessel N2 52.94 atm f increase OI decrease (no change) H2 23.44 atm O t increase OI decrease O (no change) A NH3 14.08 atm O t increase I decrease (no change) N2 47.16 atm O f increase I decrease (no change) В H2 20.07 atm O f increase O I decrease (no change) NH3 11.95 atm O f increase OI decrease (no change) N2 47.80 atm O f increase OI decrease (no change) H2 21.97 atm O f increase OI decrease (no…

For the reaction of NO2 to form NO and O2, which reaction vessel (all at different temperatures) would yield the smallest equilibrium constant? 2 NO2(g) +2 NO(g) + O2(g) → is supposed to be an equilibrium arrow

For the reaction 2 CO2(g) <-->2 CO(g) + O2(g) , K = 4.3 x 10-21 at a particular temperature. If initial [CO2] = 0.01 M and all other initial concentrations are zero, what is [CO2] at equilibrium?   Please provide answer to two decimal places.

A student ran the following reaction in the laboratory at 1080 K: 2SO3(g) 2S02(g) + O₂(g) When he introduced SO3(g) at a pressure of 0.886 atm Into a 1.00 L evacuated container, he found the equilibrium partial pressure of SO3(g) to be 0.340 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer 44 $ T R F V/ % 5 Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support F5 G ^ 6 MacBook Air Y H & 7 RN U * 0 J ► 11 F8 M ( 9 ►► K F9 O 1 F11 + { Save and Exit = F12 11

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Consider the reaction: 2S (s) + 30₂ (9)2SO3(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: 3 80 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K = E D S(s) + O2(g) → SO₂(g) K₁ SO₂(g) + 1/2O₂(g) SO3(9) K₂ 13 с Submit Answer $ 888 FA F4 R F Show Hint V Retry Entire Group 9 more group attempts remaining % 5 T Cengage Learning Cengage Technical Support F G 6 B MacBook Air FO Y H & 7 N F7 U J * 00 8 ➤11 FO I M ( 9 V K O < H дв ) O L F10 question. P command F11 A ; Previous { + alt #2 “ . ? option Save and Exit I 1 delete 1 ente re

14.  The following reaction is allowed to come to equilibrium and then the volume is increased.  Predict the effect of the indicated volume change once equilibrium is restored.                         H2O(g)            +          CO2(g)               double arrow              H2CO3(g)     The reaction will shift right.     The reaction will shift left.     There will be no effect.     Effect can not be determined from information provided.

An evacuated reaction vessel is filled with 0.800 atm of N₂ and 1.681 atm of Br2. When equilibrium is established according to the reaction below, there are 1.425 atm of Br2 remaining in the vessel. What is the equilibrium partial pressure of NBr3? 2 NBr3 (g) = N₂ (g) + 3 Br2 (g)

A chem ngineer is studying the following reaction: + HCN(aq) + NH3(aq) → CN¯(aq)+NH (aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.1. C The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B C compound HCN NH3 CN NH4 HCN NH3 CN NH₁ HCN NH₂ CN NHA 4 concentration 0.28 M 0.12 M 1.05 M 0.94 M 0.67 M 0.51 M 0.66 M 0.55 M 0.31 M 0.15 M 1.02 M 0.91 M expected change in concentration ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease 888888 ↓decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease…