C) CaCO3(s) → CaO(s)+CO2(g)   Calculate the value of the equilibrium constant. Express the equilibrium constant to three significant figures. K=_____ I) 2NO(g)+O2(g) ⇌ 2NO2(g)      Calculate the value of the equilibrium constant. Express the equilibrium constant to three significant figures. K=___ Using data from the table below, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions

Nitrogen dioxide decomposes according to the reaction 2 NO2 (g) ⇌ 2 NO (g) + O2 (g)  Where Kp = 4.48 x 10 ^ -13 at a certain temperature. If 0.40 atm of NO is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO (g) and O2 (g)?  P NO =   atm NO P O2 =   atm O2 Use correct significant figures.

Consider the reaction, PCl5(g) ⇌ PCl3(g)+ Cl2(g) where the value for Kc is 4.1 x 10-5. The initial concentration of PCl5 is 1.11 M. What is the concentration (molarity) of PCl3 at equilibrium? Report your answer to two decimal places using scientific notation.

Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.

Hydrogen and chlorine react to form hydrogen chloride, like this: H₂(g) + Cl₂(g) - 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound concentration at equilibrium H₂ 0.26M Cl₂ HCI Kc Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. = 1.4M 0 0.97 M 0 x10 X

A student ran the following reaction in the laboratory at 672 K: 2NH3(g)     N2(g) + 3H2(g) When she introduced 6.42×10-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 9.09×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HF (aq) + OH- (aq)F- (aq) + H2O (l)   K =

1.

N2(g) +3H2(g) 2NH3 (g) what is the value of K. at 500 °C if the equilibrium concentrations are as follows: H2 = 0.50 M , N2] = 0.60 M , and [NH3] = 2.2 M ? Express the equilibrium constant to two significant figures. ? Ke =

Write the equilibrium constant expression, Kc, for the equation:                         2NO2(g)  +  7H2(g)   -----> 2NH3(g)  +  4H2O(g) Write the equilibrium constant expression, Kc, for the reverse of the previous reaction.