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A student ran the following reaction in the laboratory at 431 K: PC15 (9) PC13 (g) + Cl₂ (g) When she introduced 2.98 moles of PC15 (g) into a 1.00 liter container, she found the equilibrium concentration of PC15 (9) to be 2.94 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. Show Hint Retry Entire Group 9 more group attempts remaining 2 Previous Next or n er et

Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)

Hydrogen and chlorine react to form hydrogen chloride, like this: H,(g) + Cl,(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 0.86 M Cl, 0.30 M HC1 1.9 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0

Consider the equilibrium 3Al + 2Baq 2Cg. Which of these is the correct expression for Q? Q =  PC2 + [1]3 + [B]2 Q= (PC2) / ([1]3 + [B]2) Q = (2PC) / (3[1] + 2[B]) Q = (PC2) / ([1]3 x [B]2) Q = (2PC) / (3[1] x 2[B])

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

056575718snapshotld=13245488&id-5636490008takeld=4bfba59b09f0e5b& Q Search this course X References Use the References to access important values if needed for this question. Consider the following reaction where K, = 4.55x10 at 723 K: H N2(g) +3H2(g)2NH3(g) 1008 If the three gases are mixed in a rigid container at 723 K so that the partial pressure of each gas is initially one atm, what will happen? A-Z Indicate True (T) or False (F) for each of the following 1. A reaction will occur in which NH (g) is consumed. 2. Kn will increase. 3. A reaction will occur in which N, is consumed 4. Q is less than K. 5. The reaction is at equilibrium. No further reaction will occur 4. Q versus K: This is group attempt 1 of 5 Autosaved at 1:06 PM Back Next 1:06 PM PRA x 11 9/24/2019 Lhp delete 12 prt sc f11 insert KA

For the following reaction :   H2 (g)   +   I2 (g)     2HI (g) it was found that a 13.0L vessel at equilibrium contained 0.852 mol H2, 0.361 mol I2, and 2.99 mol of HI.  A)   Write an expression for Kc. B).  Determine the value of Kc for this reaction.

Give correct answer please..don't use Ai for answering this