H2(g) + Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas? ○ The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right whi would result in more CO2 being produced until equilibrium is achieve ○ The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved

H2(g) + Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas? ○ The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right whi would result in more CO2 being produced until equilibrium is achieve ○ The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given K, and all but one of the equilibrium concentrations, find the concentration of the one that was not given. Example: Z2 D 2 Z An equilibrium mixture of Z2 and Z has [Z] = 0.93 M. Find [Z2], given that the value of K is 5.00. Given K and the initial concentrations of all reactants and products, find the final (equilibrium) concentrations. Example: Z2 D 2 Z initial concs: 0.400M 0.000M Given K and the concentrations of all reactants and products, determine if the reaction is at equilibrium. If it is not, determine which way the reaction will go. In the hardest version of this problem type, determine the equilibrium concentrations. Example: Is the system below at equilibrium? (K is equal to 5.00.) If not, which way will the reaction go? Find the equilibrium concentrations. Z2 D 2 Z concs: 2.00 M…
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 10 at a certain temperature. If a solid sample of NH SH decomposes, what will the equilibrium concentration of NH, be? NH,SH(s) = NH,(g) + H,S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH,SH(s) NH,(g) H¸S(9) + Initial (M) Change (M) Equilibrium (M) 2 RESET 1.2 x 101 x+ -X +2x -2x 1.2 x 10*+x 1.2 x 10 - x 1.2 x 10* + 2x 1.2 x 10* - 2x
Consider the following reaction: 2 H2O(g) + 2 SO2(g) 2 H2S(g) + 302(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6. 3.1 × 10-3 M 0.058 M 0.028 M 0.12 M 0.045 M
The decomposition of NH,HS is endothermic: NH,HS (s) NH3 (g) + H,S (g) Which change to an equilibrium mixture of this reaction results in the formation of more H,S? O a decrease in pressure an increase in temperature an increase in the amount of NH4HS O a decrease in the volume of the reaction vessel (at constant temperature)
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
Consider the reversible reaction. PCI, = PCI, + Cl, What substances are present at equilibrium? PCI, PCI, O Cl, Are the concentrations of phosphorus pentachloride, PCI,, and phosphosphorus trichloride, PCl, , constant or changing at equilibrium? The concentrations of both PCl, and PCl, are changing at equilibrium. The concentration of PCl, is constant, and the concentration of PCl, is changing at equilibrium. The concentration of PCl, is changing, and the concentration of PCl, is constant at equilibrium. The concentrations of both PCl, and PCl, are constant at equilibrium.
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]
Consider the following equilibrium: CO(g) + NO2(g) ↔ CO2(g) + NO(g) At a specific temperature the equilibrium concentrations where determined to be: [CO] = 0.0033M [NO2] = 0.021M [CO2] = 0.59M [NO] = 0.59M a- Calculate the value of the equilibrium constant b- Describe the position of the equilibrium
Consider the following equilibrium system at 817 K. SO2 Cl2 (g) 2 SO2(g) + Cl2 (g) If an equilibrium mixture of the three gases at 817 K contains 1.60 x 10-3 M SO2 Cl2, 3.57 x 10-2 SO2, and 2.12 x 10-2 M Cl2, what is the value of the equilibrium constant К? M K =
Phosphorus pentachloride decomposes at higher temperatures. PC15 (8) PCl3(g) + Cl₂(g) An equilibrium mixture at some temperature consists of 5.81 g PCI, 208.23 g/mol 4.86 g PC3, 137.33 g/mol 3.59 g Cl₂, 70.91 g/mol in a 1.00-L flask. If you add 1.31 g of Cl₂, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished? O shift left O shift right Ono shift will occur [PCI5] = mol/L