n-butane and isobutane are in equilibrium at 25 degrees
centigrade:
n-butane
(g) isobutane
(g)
A one liter flask with the two species at equilibrium contains
0.170 mole isobutane and 0.0680 mole n-butane. Then the
concentration of n-butane is increase by 0.200 moles. (0.200 mole
n-butane is added.) What is the new equilibrium concentration for
isobutane? Assume value for K c remains constant
throughout process. Hint--this is a hard problem. At equilibrium
(which you are given) you can find K C. Now, the
equilibrium changes. You must use ICE to find new values.
9.22 x 10-2M |
||
1.57 x 10-1M |
||
9.25 x 10-3M |
||
3.50 x 10-2M |
||
0.312 M |
||
7.67 x 10-5M |
||
0.190 M |
||
3.12 x 10-2 M |
n-butane and isobutane are in equilibrium at 25 degrees centigrade: n-butane (g)
butane exists as two isomers n butane and isobutane kp = 2.5 at 25 degrees celsius what is the pressure of isobutane in a container of the two isomers at equilibrium with a total pressure of 1.22 atm
Show that the equilibrium mole fraction of n-butane and isobutane are given AGO RT 0 1SO iSO 1SO 0 iSo
1.18 The equilibrium constant K, for the reaction N.(g)+0g) 2 NO(g) at 1200 °C is 1.00 x 10. Cakculate the equilibrium molar concentrations of NO, N, and O, in a reaction vessel ef volume 10.00 L that initially held 0.312 mol N, and 0.407 mol O
The equilibrium constant for the following reaction is 0.190 at 346K. COBr2(8) PCO(g) + Brz(8) If an equilibrium mixture of the three gases at 346K contains 2.14x10-2 M COBr2(g) and 2.66x10-2 MCO, what is the equilibrium concentration of Brz? M Consider the following equilibrium system at 831 K. COC12(g) = CO(g) + Cl2(g) If an equilibrium mixture of the three gases at 831 K contains 2.89 x 10-4 M COCI2, 2.03 x 10-2 MCO, and 5.54 x 10-² M Cl2,...
The value of AG° is +4,730 J/mole for the reaction N,O.(g) 2NO. (g) at 25°C K= a) Use the value of AG° to calculate the value of K for this reaction at 25°C? b) Calculate the value of Q and of AG if you begin with a concentration of 0.300M N2O4 and a concentration of 1.40 M NO, c) In which direction will the reaction proceed to reach equilibrium under these conditions?
Calculate the value of the equilibrium constant, ?c , for the reaction Q(g)+X(g)↽−−⇀2M(g)+N(g) Q ( g ) + X ( g ) ↽ − − ⇀ 2 M ( g ) + N ( g ) given that M(g)↽−−⇀Z(g)6R(g)↽−−⇀2N(g)+4Z(g)3X(g)+3Q(g)↽−−⇀9R(g)?c1=3.21?c2=0.495?c3=13.4 M ( g ) ↽ − − ⇀ Z ( g ) K c 1 =3.21 6R ( g ) ↽ − − ⇀ 2N ( g ) +4Z ( g ) K c 2 =0.495 3X ( g ) +3Q...
The equilibrium constant () of the reaction below is K-6.0 x 10 with initial concentrations as follows: [H2] = 1.0 x 102 M. [Na] - 4.0 M, and (NH) - 1.0 x 10* M. N (8) + 3H,() 2NH3(e) 3. Consider the chemical reaction: N2 + 3H2 yields 2NH3. If the concentration of the reactant Hy was increased from 1.0 x 10-2M to 2.5 x 10-M, calculate the reaction quotient (C) and determine which way the chemical system would shift...
2. For the reaction: A(g) +B(g) = 2C(g) K = 1.0 x 10-5 at 25°C When equilibrium was reached at 25°C, the equilibrium concentrations of the reactant gases were: [A] = 2.5 x10-2M [B] = 2.0 x 10- M Calculate the equilibrium concentration of the product gas C? 3. At a certain temperature the reaction has an equilibrium constant of 0.400. CO(g) + H2O(g) = CO2(g) + H2(g) When 1.50 mol of carbon dioxide gas and 1.50 mol of hydrogen...
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) + H20 (I) b) CuO (s) + H2(g) Cu(l)+H20 (g) 2. At room temperature, a 1.5 L flask contains 3.0 moles of Cl, 0.5 mole of NOCI, and 4.0x10 mole of NO. Calculate Ke at this temperature for the following reaction: 2NO (g) + Cl2(g) 2NOCİ (g) 0.00245 M, does this represent a system at M, [No] 0.2 M and [Ch] If [NOCI] 2.0x 10...
The equilibrium constant, K, for the reaction N204(g) = 2N02 (8) is 4.8 x 10-3 If the equilibrium mixture contains NO2 = 0.051 M , what is the molar concentration of N, 04? Express the concentration to two significant figures and include the appropriate units. TH A Roa? N, 04] = Value