For a particular reaction at equilibrium, the pressure of the bromine is 2.0 atm at 25°C.

For a particular reaction at equilibrium, the pressure of the bromine is 2.0 atm at 25°C. The total pressure in the vessel at equilibrium is 10.0 atm. The balanced chemical equation is:

2NOBr (g) <-- --> 2NO (g) + Br₂ (g)

What is the value of Kp for the reaction?

Solutions

Expert Solution

2 NOBr (g) <-------------> 2 NO (g) + Br2 (g)

y 0 0

y - 2x 2x x

At equilibrium :

pressure of Br2 = x = 2.0 atm

total pressure = 10.0 atm

y - 2x + 2x + x = 10

y + x = 10

y + 2 = 10

y = 8

pressure of NOBr = y - 2x = 8 - 4 = 4 atm

pressure of NO = 2x = 4 atm

Kp = P²NO x Pbr2 / P²NOBr

= 4^2 x 2 / 4^2

= 2

Kp = 2.0

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

For the reaction below, determine the equilibrium partial pressure (in atm) of HBr at 252.70 K...

For the reaction below, determine the equilibrium partial pressure (in atm) of HBr at 252.70 K if the initial pressure of H2 is 2.83 atm. Assume that ΔH and ΔS do not vary with temperature. Report your answer to three significant figures. LiBr (s) + H2 (g) ⇌ LiH (s) + HBr (g) ΔHf° (kJ/mol) S° (J mol-1 K-1) LiBr -351.20 74.30 H2 0.00 130.68 LiH -90.50 20.00 HBr -36.29 198.70

44.At 25 ° C, the equilibrium partial pressures of NO2 and N2O4 are 0.150 atm and...

44.At 25 ° C, the equilibrium partial pressures of NO2 and N2O4 are 0.150 atm and 0.200 atm, respectively. If the volume is increased by 2.20 fold at constant temperature, calculate the partial pressures of the gases when a new equilibrium is established. PNO2 = atm PN2O4 = atm 45. At 25 ° C, the equilibrium partial pressures of NO2 and N2O4 are 0.150 atm and 0.200 atm, respectively. If the volume is increased by 2.20 fold at constant temperature, calculate the...

Part A) A sample of a gas at 25°C and 1.0 atm pressure has a volume...

Part A) A sample of a gas at 25°C and 1.0 atm pressure has a volume of 2.5 L. The container is allowed to expand until the pressure is 0.85 atm and the temperature is 15°C. The final volume of the gas is __________ L. Part B) A reaction is carried out that produces hydrogen gas. The gas is collected in an inverted beaker over water at 25 oC. The vapor pressure of water at 25 oC is 23.78 mmHg....

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

The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K is...

The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K is 54.7 and the reaction is: Br2(g) + F2(g) ⇔ 2 BrF(g) What is the equilibrium concentration of fluorine if the initial concentrations of bromine and fluorine were 0.121 moles/liter in a sealed container and no product was present initially?

At 1 atm and 25 ˚C the molar entropy change for the reaction CO(g) + 1...

At 1 atm and 25 ˚C the molar entropy change for the reaction CO(g) + 1 2 O2(g)  CO2(g) (1) is ΔSo = - 86.46 J K-1. The molar heat capacities at constant pressure at 1 atm and 25 ˚C for CO, O2, and CO2 are, respectively, 29.123, 29.362, and 37.12 J K-1 mol-1. Assume that the heat capacities are independent of temperature and calculate the entropy change for reaction (1) at 100 ˚C and 1 atm.

1-Calculate the partial pressure (in atm) of CH3OH at equilibrium when 4.84 atm of CH3I and...

1-Calculate the partial pressure (in atm) of CH3OH at equilibrium when 4.84 atm of CH3I and 4.84 atm of H2O react at 3000 K according to the following chemical equation: CH3I (g) + H2O (g) ⇌ CH3OH (g) + HI (g) Kp = 7.47×101 Report your answer to three significant figures in scientific notation. 2-Calculate the partial pressure (in atm) of H2O at equilibrium when 59.6 g of CdO and 3.21 atm of H2 react at 800 K according to...

a) At 25 °C the first-order rate constant for a reaction is 2.0 x 103 s-1....

a) At 25 °C the first-order rate constant for a reaction is 2.0 x 103 s-1. The activation energy is 15.0 kJ/mol. What is the value of the rate constant at 75 °C? (5 pts). b)A first-order reaction has rate constants of 4.6 x 10-2 s-1 and 8.1 x 10-2 s-1 at 0 °C and 20 °C, respectively. What is the value of the activation energy? (5 pts)

A fire extinguisher has a pressure of 12 atm at 25∘C.What is the final pressure, in...

A fire extinguisher has a pressure of 12 atm at 25∘C.What is the final pressure, in atmospheres, when the fire extinguisher is used at a temperature of 63 ∘C, if Vand n are constant? P=

Subjects