For the following systems at equilibrium A:2NOCl(g)⇌2NO(g)+Cl2(g) B: H2(g)+I2(g)⇌2HI(g) classify these changes by their effect. Drag...

For the following systems at equilibrium A:2NOCl(g)⇌2NO(g)+Cl2(g) B: H2(g)+I2(g)⇌2HI(g) classify these changes by their effect.

Drag the appropriate items to their respective bins.

Bins: leftward shift, no shift, rightward shift

Items: system A Decrease container size, system A Increase container size, system b Increase container size, system B Decrease container size

Expert Solution

queen_honey_blossom answered 1 year ago

For the reaction H2(g) + I2(g) ↔ 2HI the value of the equilibrium constant is 25....

For the reaction H2(g) + I2(g) ↔ 2HI the value of the equilibrium constant is 25. Starting with 1.00mol of each reactant in a 10.L vessel, how many moles of HI will be present at equilibrium?

Consider the following equilibrium: 2NOCl(g) 2NO(g) + Cl2(g)with K = 1.6 × 10–5. 1.00 mole of pure...

Consider the following equilibrium: 2NOCl(g) 2NO(g) + Cl2(g)with K = 1.6 × 10–5. 1.00 mole of pure NOCl and 1.50 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of NO(g).

Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this...

Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature Kp 150 K 1.4×10?6 175 K 4.6×10?6 200 K 3.6×10?2 225 K 1.1 250 K 15.5 Use the data to find ?H?rxn and ?S?rxn for the reaction.

For the reaction 2NO(g) + Cl2(g) --->2NOCl(g) if the concentration of NO is tripled, the rate...

For the reaction 2NO(g) + Cl2(g) --->2NOCl(g) if the concentration of NO is tripled, the rate of the reaction increases by a factor of nine. if the concentration of Cl2 is cut in half, the rate of the reaction is decreased to half the original rate. Find the order of reaction for each reactant and write the rate expression for the reaction.

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2:...

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2: 0.050M, and HI:0 Assume this reaction is not at equilibrium. When it does reach equilibrium, what will the concentrations be?

At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g)....

At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g). Calculate the equilibrium constant for the reaction 2H2(g) + 2I2(g) ↔ 4HI(g), 1/2H2(g) + 1/2I2(g) ↔ HI(g), and 2HI(g) ↔ H2(g) + I2(g).

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature,...

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature, 0.7 mol of H2 and 0.7 mol of I2 were placed in a 1 L container. What is the concentration of HI present at equilibrium?

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on (a) total pressure (b) catalyst used (c) amount of H2 and I2 (d) temperature

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on___________.(a) total pressure(b) catalyst used(c) amount of H2 and I2(d) temperature

If delta H rxn is -75.2 kJ, 2NO(g) + Cl2 (g) <---> 2NOCl(g)

If delta H rxn is -75.2 kJ, 2NO(g) + Cl2 (g) <---> 2NOCl(g) A scientist places four moles of nitrogen monoxide and two moles of chlorine gas into flask A and the same amounts into Flask B, then allows the systems to reach equilibrium. Flask A is at 25 degrees Celsius and Flask B is at 200 degrees Celsius A) In which flask will the reaction occur faster? Explain. B) In which flask will the reaction occur to a greater...

The reaction 2NO(g) + Cl2(g) --> 2NOCl(g) obeys the rate law rate = k [NO]2 [Cl2]....

The reaction 2NO(g) + Cl2(g) --> 2NOCl(g) obeys the rate law rate = k [NO]2 [Cl2]. The following mechanism is proposed: NO (g) + Cl2 (g) --> NOCl2(g) NOCl2(g) + NO (g) -->2NOCl (g) a) What would the rate law be if the first step was rate determining? b) Based on the observed rate law, what can be concluded about the relative rates of the 2 reactions?

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