Predict the equilibrium partial pressure of HBr in the reaction described below by constructing an equilibrium expression for Qp, constructing an ICE table, writing the equilibrium constant expression, writing an equilibrium expression for Kp expressed in partial pressures, and solving for the equilibrium partial pressure of HBr. Complete Parts 1-4 before submitting your answer. 2 HBr(g) H₂(g) + Br2(g) 2 3 4 NEXT > An initial mixture of 0.20 atm HBr, 0.010 atm H2, and 0.010 atm Br2 reacts. Set up the expression for Qp to determine the direction of the reaction. Each reaction participant must be represented by one tile. not combine terms. Once the expression is constructed, solve for Qp. (0.20) 5.0 x 10-4 1 (0.010) 0.050 Qp = 2(0.20) 0.0025 2(0.010) 2.0 x 10³ (0.20)² 4.0 x 10² (0.010)² 2(0.20)² RESET 2(0.010)²

1-A mixture of 0.100 mol of NO, 0.0500 mol of H2, and 0.100 mol of H₂O is placed in a 1.00L vessel. The following equilibrium is established: 2NO(g) + 2H2(g) -- N₂(g) + 2H2O(g) At equilibrium [NO] = 0.0620 M. Calculate the equilibrium concentration of H2, N2, H₂O.

Given the following reaction, the equilibrium constant, and the initial concentrations; answer the four bullet questions. 2 NO2 (g) - 2 NO (g) + O2 (g) Kc = 1.56 x 10-10 Initial Species Concentration (M) NO2 5.62 x 10-10 NO 3.99 x 10-16 O2 9.35 x 10-3 • Set up the equilibrium expression, and calculate the reaction quotient (Q). Note: ^ means "to the" Q = [ Select ] • How does Q compare to K? Q is [ Select]

The following reaction has an equilibrium constant of 2.65 x10-3 at 300K. Br2 (g) + Cl2 (g) 2 BrCl (g) Which of the following statements is true?   Question 5 options:   The system has a higher concentration of reactant molecules than product molecules at equilibrium, but there are significant quantities of both.   The system consists almost entirely of reactant molecules at equilibrium.   The system consists almost entirely of product molecules at equilibrium.   The system has approximately equal concentrations of product and reactant molecules at equilibrium.   The system has higher concentrations of product molecules than reactant molecules at equilibrium, but there are significant quantities of both.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH4 (g) 3H₂(g) + C₂H₂ (g) K₂=9. × 10-10 He fills a reaction vessel at this temperature with 5.0 atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. yes no atm X S ?

Rank the molecules in decreasing (strongest to weakest) acidity. Include ALL resonance structures with arrows and explain reasoning for rank.

Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(9)→3 NO2(g)+H,0(1) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 5.2 g NO 19.8 g NO, 7.9 g H,O 134.3 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. °C K_ = 0 x10 C