(please type answer only) I am having problems answering these questions on this page.A student ran the following reaction in the laboratory at 341 K:CH₂(g) + CCL (9) 2CH₂Cl₂ (9)When she introduced 0.0405 moles of CH₂(g) and 0.0650 moles of CCL, (g) into a 1.00 liter container, she found the equilibrium concentration of CCL, (g)to be 0.0587 M.Calculate the equilibrium constant, Ke, she obtained for this reaction.Ke-Show Transcribed TextCarbon tetrachloride can be produced by the following reaction:CS₂(g) + 3 Cl₂(g) = 5₂Cl₂(g) + CCl4(8)In an experiment, 0.120 mol of CS₂ and 0.360 mol of Cl₂ were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, themixture contains 0.070 mol CCl4. Calculate the value of K under the experimental conditions.K=Show Transcribed TextThe reactionJatm2 NO(g) + Br₂(g) → 2 NOBr(g)has K₂ = 109 at 25°C. If the equilibrium partial pressure of Bry is 0.0262 atm and the equilibrium partial pressure of NOBr is 0.0822 atm, calculate the partialpressure of NO at equilibrium.Partial pressure.Show Transcribed Text3

The equilibrium constant is defined as the ratio of the concentration of product to the…

A student ran the following reaction in the laboratory at 341 K: CH₂(g) + CCL (9) 2CH₂Cl₂ (9) When she introduced 0.0405 moles of CH₂(g) and 0.0650 moles of CC1, (g) into a 1.00 liter container, she found the equilibrium concentration of CC1, (g) to be 0.0587 M. Calculate the equilibrium constant, K., she obtained for this reaction. Ke-