A system at equilibrium contains I2(g) at a pressure of 0.13 atm and I(g) at a...

A system at equilibrium contains I2(g) at a pressure of 0.13 atm and I(g) at a pressure of 0.18 atm . The system is then compressed to half its volume.

Part A

Find the pressure of I2 when the system returns to equilibrium.

Part B

Find the pressure of I when the system returns to equilibrium.

Expert Solution

queen_honey_blossom answered 2 years ago

A system at equilibrium contains I2(g) at a pressure of 0.18 atm and I(g) at a pressure...

A system at equilibrium contains I2(g) at a pressure of 0.18 atm and I(g) at a pressure of 0.21 atm . The system is then compressed to half its volume. Part A Find the pressure of I2 when the system returns to equilibrium. Part B Find the pressure of I when the system returns to equilibrium.

A system at equilibrium contains I2(g) at a pressure of 0.25 atm and I(g) at a...

A system at equilibrium contains I2(g) at a pressure of 0.25 atm and I(g) at a pressure of 0.25 atm . The system is then compressed to half its volume. Part A Find the pressure of I2 when the system returns to equilibrium. Express your answer to two significant figures and include the appropriate units. Part B Find the pressure of I when the system returns to equilibrium. Express your answer to two significant figures and include the appropriate units.

A system at equilibrium contains I 2 (g) at a pressure of 0.19 atm and I(g)...

A system at equilibrium contains I 2 (g) at a pressure of 0.19 atm and I(g) at a pressure of 0.22 atm . The system is then compressed to half its volume. Part A Find the pressure of I 2 when the system returns to equilibrium. Part B Find the pressure of I when the system returns to equilibrium.

A-Calculate the equilibrium concentration of IBr and I2 for the reaction 2 IBr(g) ⇄ I2 (g)...

A-Calculate the equilibrium concentration of IBr and I2 for the reaction 2 IBr(g) ⇄ I2 (g) + Br2 (g) when the initial [IBr] = 1.00 M and the concentrations of the products is initially zero. (KC = 2.50x10-3) [IBr]equilibrium = _______________ [I2]equilibrium =_______________ B- KC = 1.88x10-14 for the reaction CH3NC(g) ⇄ CH3CN(g). If the initial concentrations are [CH3NC] = 0.122 M and [CH3CN] = 0.244 M, what is the equilibrium concentration of CH3CN? [CH3CN] = _______________ M

For the equilibrium 2IBr(g)?I2(g)+Br2(g) Kp=8.5×10?3 at 150 ?C. A) If 2.1×10?2 atm of IBr is placed...

For the equilibrium 2IBr(g)?I2(g)+Br2(g) Kp=8.5×10?3 at 150 ?C. A) If 2.1×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? Express your answer to two significant figures and include the appropriate units. B) If 2.1×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? Express your answer to two significant figures and include the appropriate units. C) If...

Consider the reaction of I2 (g) described by I2 (g) = 2 I (g). The total...

Consider the reaction of I2 (g) described by I2 (g) = 2 I (g). The total pressure and partial pressure of I2 (g) at 14000C have been measured to be 36.0 torr and 28.1 torr, respectively. Use these data to calculate KP0, K0c, and Kx at 14000C. Calculate xI under these conditions? What would X1 be if we decreased the total pressure to 36.0×10-6 torr? What would X1 be if we increased the total pressure to 36.0 atm?

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

Calculate the partial pressure (in atm) of NO at equilibrium when 1.05 atm of NO2 dissociates...

Calculate the partial pressure (in atm) of NO at equilibrium when 1.05 atm of NO2 dissociates at 250 K according to the following chemical equilbrium: 2NO2(g) ⇌ 2NO(g) + O2(g) Kp = 2.96×10-12 If the 5% approximation is valid, use the assumption to compute the partial pressure. Report your answer to three significant figures in scientific notation.

Calculate the partial pressure (in atm) of CH3Br at equilibrium when 2.01 atm of CH3OH and...

Calculate the partial pressure (in atm) of CH3Br at equilibrium when 2.01 atm of CH3OH and 2.01 atm of HBr react at 1000 K according to the following chemical equation: CH3OH (g) + HBr (g) ?CH3Br (g) + H2O (g) Kp = 2.78

Consider an open system that is in equilibrium with 10^-2 atm CO2 (g). You have no...

Consider an open system that is in equilibrium with 10^-2 atm CO2 (g). You have no other information about the system. Henry's Law telss us that KhCI2=H2CO3/pCO2= 10^-1.5 M-atm^-1 pKa1 is 6.3 (for H2CO3* dissassociation) and pKa2 is 10.3 (for HCO3- dissassociation). What is the [HCO3*], and [CO3^2-] if the pH of the solution is 5, 7,9?

Question