Write the expressions for K_c for the following reactions CH_4(g) + 2 H_2S (g) r
ID: 487095 • Letter: W
Question
Write the expressions for K_c for the following reactions CH_4(g) + 2 H_2S (g) reversiblearrow CS_2 (g) + 4 H_2 (g) 3 NO (g) reversiblearrow 2 N_2O(g) + NO_2 (g) C(s) + 2H_2 (g) reversiblearrow CH_4 (g) Which of the following reactions lies to the right, favoring the formation of products, and which lies to the left favoring the formation of reactants? 2 NO (g) + O_2 (g) reversiblearrow 2 NO_2 (g) K_p = 5.0 times 10^12 2 HBr(g) reversiblearrow H_2(g) + Br_2 (g) K_c = 5.8 times 10^-18 Calculate K_c at 303 K for SO_2(g) + Cl_2 (g) reversiblearrow SOCl_2 (g) if K_p = 34.5 at this temperature. Consider the following equilibrium for which K_p = 0.0752 at 480 degree C: 2 Cl_2(g) + 2 H_2O (g) reversiblearrow 4 HCl (g) + O_2 (g) What is the value of K_p for the reaction 4 HCl (g) + O_2 (g) reversiblearrow 2 Cl_2 (g) + 2 H_2 O (g)? What is t5he value of of K_p for the reaction Cl_2 (g) + H_2 O(g) reversiblearrow 2 HCl (g) + 1/2 O_2 (g)?Explanation / Answer
Answer of (1)
In a reaction in which aA + bB <---> cC + dD, the equilibrium constant Kc is defined as:
Kc = [C]^c [D]^d / [A]^a [B]^b
(a)
Kc = [CS2] [H2]^4 / [CH4] [H2S]^2
(b)
Kc = [NO2]*[N20] / [NO]^3
(c)
Kc = [CH4] / [C]*[H2]^2
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