In each of the reactions, how does the equilibrium respond to an increase in pressure?
(a)
(b)
(c)
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Chemistry for Engineering Students
- Heating a metal carbonate leads to decomposition. BaCO3(s) BaO(s) + CO2(g) Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left or (iii) shifts right. (a) add BaCO3 (b) add CO2 (c) add BaO (d) raise the temperature (e) increase the volume of the flask containing the reactionarrow_forwardNitrosyl bromide, NOBr, dissociates readily at room temperature. NOBr(g) NO(g) + Br2(g) Some NOBr is placed in a flask at 25 C and allowed to dissociate. The total pressure at equilibrium is 190 mm Hg and the compound is found to be 34% dissociated. What is the value of Kp?arrow_forwardGiven the following descriptions of reversible reactions, write a balanced net ionic equation (simplest whole-number coefficients) and the equilibrium constant expression (K) for each. (a) Liquid acetone (C3H6O) is in equilibrium with its vapor. (b) Hydrogen gas reduces nitrogen dioxide gas to form ammonia and steam. (c) Hydrogen sulfide gas (H2S) bubbled into an aqueous solution of lead(ll) ions produces lead sulfide precipitate and hydrogen ions.arrow_forward
- The formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2 NH3(g) 1. Does the reaction shift to the right or to the left, or does it remain unchanged, when extra H2 is added? (a) shift left (b) shift right (c)unchangedarrow_forwardA necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?arrow_forwardAt a particular temperature, iodine vapor, I2, is added to a bulb containing H2(g). Describe what is happening to the concentrations of reactants on the molecular level: (a) at the moment I2 enters the reaction bulb (b) as reaction proceeds (c) at equilibriumarrow_forward
- Write the mathematical expression for the reaction quotient, QC, for each of the following reactions: (a) CH4(g)+CI2CH3CI(g)+HCI(g) (b) N2(g)+O2(g)2NO(g) (c) 2SO2(g)+O2(g)2SO3(g) (d) BaSO3(s)BaO(s)+SO2(g) (e) P4(g)+5O2(g)P4O10(s) (f) Br2(g)2Br(g) (g) CH4(g)+2O2(g)CO2(g)+2H2O(l) (h) CuSO45H2O(s)CuSO4(s)+5H2O(g)arrow_forwardIn a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317 torr; NH3, 1.00103 torr. N2(g)+3H2(g)2NH3(g) (a) How will the partial pressures of H2, N2, and NH3 change if H2 is removed from the system? Will they increase, decrease, or remain the same? (b) Hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressures of the other substances under the new conditions.arrow_forwardA mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 5.0 103 mol/L, [O2] = 1.9 103 mol/L, and [SO3] = 6.9 103 mol/L. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 SO2(g) + O2(g) 2 SO3(g) Kc = 279arrow_forward
- For the following endothermic reaction at equilibrium: 2SO3(g)2SO2(g)+O2(g) which of the following changes will increase the value of K? a. increasing the temperature b. decreasing the temperature c. removing SO3(g) (constant T) d. decreasing the volume (constant T) e. adding Ne(g) (constant T) f. adding SO2(g) (constant T) g. adding a catalyst (constant T)arrow_forwardWrite expressions for Kp for the following reactions. a. 2Fe(S)+32O2(g)Fe2O3(S) b. CO2(g)+MgO(s)MgCO3(s) c. C(s)+H2O(g)CO(g)+H2(g) d. 4KO2(s)+2H2O(g)4KOH(s)+3O2(g)arrow_forwardYou place 4.00 mol of dinitrogen trioxide, N2O3, into a flask, when: it decomposes at 25.0C and 1.00 atm: N2O3(g)NO2(g)+NO(g) What is the composition of the reaction mixture at equilibrium if it contains 1.20 mol of nitrogen dioxide, NO2?arrow_forward
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