Question

MULTIPLE CHOICE. Choose the na t ive that best completes the statement or answer the questi 1) Write the equilibri e the equilibrium constanter ia for the following reaction in the forward direction 2CH )302)2006) 4H2O) 2100) + 4H20 A) KICHg2.0P B) Ke- CH-302 CO2+ [H2014 2 CH431021 COP 2014 Dj Ke-2100 H30 KICHAPOP 2) Ar elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide H2(g) + Brz (g) 211Br (g) A mixture of 0.682 mol of H2 and 0.410 mol of Bey is combined in a reaction vessel with a volume of 2.00 L At equilibrium at 700 K, there are 0.566 mol of H2 present. At equilibrium, there are mol of Bez present in the reaction vessel A) 0.440 B) 0.324 0.000 D) 0.566 D) 0.232 3) The equilibrium constant is equal to 5.00 at 1.300 K for the reaction 2 502) OR) - 2 SO3). If initial concentrations are SO2] - 1.20 M. 1O2-0.45 M. and S03] 1.80 M the system is A) notat equilibrium and will remain in an unequilitated state B) mot at equilibrium and will shift to the right to achieve an equilibrium state C) at equilibrium D) notat equilibrium and will shift to the left to achieve an equilibrium 4) What is true about the relationship of Ko and for the reaction: 2 CH4). 3 026) -2 COX) 4H2O() A) Kp <ke BỊ E, K . C) Kp-ke D) Kp and are not related 5) The equilibrium constant (Kp) for the interconversion of PCs and PC is 0.0121 PCI (8) PC (8) C12 (8) A vessel is charged with PCs, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PC atm. A) 0.078 B) 0.123 90.090 D) 0.033 E) 0.045 6) The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is Keq – A) ktkr B) kg + kr C) kaks D) kq-ks E) kelkę
Just give me the answers

Answer 1

1.) 2CH₄ (g) + 3O₂ (g) ----->2 CO(g) + 4H₂O(g)

equilibrium constant = K_c = [CO]²[H₂O]⁴/[CH₄]²[O₂]³

option C is correct

2) H₂(g) + Br₂ (g) -----> 2HBr(g)

inital = 0.682 mol 0.440 mol 0 mol

at equilibrium = (0.682 - a) (0.440- a) 2a

where a = degree of dissociation

now at equilibrium, concentration of H₂ = 0.566 mol

but at equilibrium,concentration of H₂ = (0.682 - a) mol

therefore, 0.682 - a = 0.566

a = 0.116 mol

concentration of Br₂ at equilibrium = 0.440 - 0.116 = 0.324 mol

Option B is correct

3.)Given,

concentration of SO₂ = 1.20 mol

concentration of O₂ = 0.45 mol

concentration of SO₃ = 1.8 mol

equilibrium constant = 5

according to question,theoretical value of K_c is

equilibrium constant = K_c = [SO₃]²/[SO₂]²[O₂]

putting concentration values = 1.8²/(1.2² x 0.45)

K_c = 5

both given and theoretical values are same,therefore system is in equilibrium

Option C is correct

4) relation between K_c and K_p is given as

K_p = K_c (RT)^{$\bigtriangleup$n}

where $\bigtriangleup$ n = (sum of molar concentration co-efficient of product side) - (sum of molar concentration coefficient of reactant side)

here $\bigtriangleup$ n = (2+4) -(3+2) = 1

therefore K_p = K_c(RT)

therefore K_p > K_c (

option B is correct