Practice ProblemATTEMPT
For each change indicated, determine whether the equilibrium:
will shift to the right, shift to the left, or neither: (a) addition of
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- issue 6Choose the equilibrium in which the products are favored by a drop in pressure and the reactants favored by a drop in temperature.a) N2(g) + 3 H2(g) ⇔ 2 NH3(g) + 92.3 kJb) H2(g) + I2(g) + 51.8 kJ ⇔ 2 HI(g)c) PCl3(g) + Cl2(g) ⇔ PCl5(g) ΔH = -84.2 kJd) 2 NO2(g) ⇔ 2 NO(g) + O2(g) ΔH = +54 kJarrow_forwardThe reaction of bromine gas with chlorine gas, Br2(g) + Cl2(g) ⇄ 2 BrCl(g), has a Kp value of 7.20. If 0.400 atm of both Br2 and Cl2 are placed in a closed vessel and allowed to come to equilibrium, what is the equilibrium partial pressure of BrCl(g)? (answer in atm and no scientific notation)arrow_forwardConsider the following equilibrium: N2O4(g) ⇄2NO2(g). If Kp = 0.144 at 950.0 K, calculate Kc. (no scientific notation)arrow_forward
- Hydrogen iodide gas is formed from its elements with a value for Kp = 25.5 at a certain temperature: H2 (g) + I2 (g) <---> 2 HI (g) What will the equilibrium pressure (in atm) of hydrogen iodide gas be if the initial partial pressure of both reactant gases is 0.150 atm? (answer in 3 significant figures)arrow_forwardAt 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is 2.25 × 10−4. If [H2S] = 4.80 × 10−3 M and [H2] = 1.40 × 10−3 M, calculate [S2]. Please write to text formet answerarrow_forwardReaction of nitrogen and hydrogen in the presence of a catalyst produces ammonia: N2 + 3H2 2NH3 , rHo = -92 kJ mol-1 . What would increase equilibrium concentration of the product in the mixture? A) Increase pressure, keep temperature constant B)Increase temperature, keep pressure constant C) Decrease pressure, keep temperature constant D) Information is insufficient for answerarrow_forward
- Which of the following is NOT necessarily true of a reaction at equilibrium? a. the forward and reverse reaction rates are equal b. the concentration of reactants is the same as the concentration of products c. the concentration of reactants and products doesn't change with time d. no correct response is givenarrow_forwardThe equilibrium constant for the reaction 2 HF (g) ⇌ H₂ (g) + F₂ (g) is 0.360 at a particular temperature. What is the equilibrium constant for the equation ½ H₂ (g) + ½ F₂ (g) ⇌ HF (g)? ANswer _____arrow_forwardCalculate T (in K) given ΔG^0= -19.4 kJ/mol and ΔH^0= 69.9 kJ/mol and ΔS^0= 253 J/mol KΔG^0=ΔH^0−TΔS^0 A) 706 B) 1,760 C) 353 D) 0.353 E) 118arrow_forward
- Given that K c of the reaction below is 2.2 × 10-3 at a certain temperature, which of the following statements is correct? 2ICl (g) ⇄ I2 (g) + Cl2 (g) View Available Hint(s) Given that K c of the reaction below is 2.2 × 10-3 at a certain temperature, which of the following statements is correct? 2ICl (g) ⇄ I2 (g) + Cl2 (g) A. At this temperature, the products are favored and equilibrium lies to the left. B. At this temperature, the reactants are favored and the equilibrium lies to the right. C. At this temperature, the products are favored and the equilibrium lies to the right. D. At this temperature, the reactants are favored and the equilibrium lies to the left.arrow_forwardPlease HELP!!! Need correct solution. The equilibrium constant for the chemical equation N₂(g) + 3H₂(g) = 2NH₂(g) is Kp = 0.0328 at 201 C. Calculate the value of K, for the reaction at 201 ˚C.arrow_forwardCarbon monoxide and hydrogen react according to the following equation: CO (g) + H2 (g) CH4 (g) + H2O (g) When 1.00 mol of CO and 3.00 moles of H2 are placed in a 10.0 L container at 927 ° C (1200 K) and allowed to reach equilibrium, the mixture is found to have 0.363 moles of H2O What is the molar composition (that is, how many moles) of H2 are present in the equilibrium mixture? Answer:arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning