Practice ProblemATTEMPT
In an analysis of the following reaction at
the equilibrium concentrations were found to be
at
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Chemistry
- Solve all part please. Consider the equilibrium reaction N2O4 (g) ⇌ 2 NO2 (g)a. Using appendix C, find H and S for this reaction (you will need this for b,c). delta s= 176.6J delta H=5802kJb. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PNO2 = PN2O4 = 1.0 atm.c. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PT = 10.0 atm and PNO2 = 2 PN2O4.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_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
- Consider the hypothetical reaction, which has an equilibrium constant (Kp) of 16.1 when the reaction occurs at 167°C. 2 W (g) + X (g) <---> 3 Y (g) If the equilibrium partial pressure of W is 0.787 atm and that of Y is 1.65 atm, what will the equilibrium partial pressure (in atm) of X be? (answer in 3 significant figures)arrow_forwardFor the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g) At 298 K in a 10.0 L vessel, the equilibrium values are as follows: 0.721 atm of A, 4.18 mol of B, 6.25 mol of C, and 2.91 atm of D. What is the value of the equilibrium constant? Answer _____arrow_forwardSuppose you are given the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas B, the value of K: Select one: a. increases, because by adding A more products are made, increasing the product to reactant ratio b. does not change, as long as the temperature is constant c. depends on whether the reaction is endothermic or exothermic d. does not change, because A does not figure into the product to reactant ratio e. decreases, because A is a reactant so the product to reactant ratio decreasesarrow_forward
- The reaction shown below has an equilibrium constant value of Kp=5.50 at a certain temperature.CO (g) + Cl₂ (g) ⇄ COCl₂ (g) Kp = 5.50A container is pressurized with CO and Cl₂ until the pressure of CO is 0.450 atm and the pressure of Cl₂ is 0.200 atm. Calculate the pressure of COCl₂ in the container when the system reaches equilibrium.Answer: atm COCl₂arrow_forwardChemistry Find ΔHfus for water Mass of cup and warm water: 45.67 gFinal mass of cup, water, and melted ice: 69.76 gMass of empty cup: 2.21 gTemperature of warm water: 63 °CTemperature of ice: 0 °CTemperature at equilibrium: 45.2 °Carrow_forwardConsider the following reaction: CO (g) + H2O (g) <===> CO2 (g) + H2 (g) a. Write the expression for the equilibrium constant (K) of the reaction b. Calculate the value for K using the following concentrations of each substance at equilibrium: [CO) = 0.55 M [H2O) = 0.44 M [CO2) = 0.25 M [H2) = 0.10 M c. Based on the value you obtained for K, are the products or reactants lower in energy? d. Is the value for ΔH negative or positive? please show workarrow_forward
- Consider the following equilibrium: 2HF(g)⇌H2(g)+F2(g) At equilibrium, the concentration of hydrogen fluoride gas, hydrogen gas, and fluorine gas are 2.04 mol/L, 2.47 mol/L, and 1.89 mol/L. What is the value of the equilibrium constant? Answer to 3 decimal places.arrow_forwardA chemical equilibrium A ⇄ 2B has a forward rate constant, kf = 12 M –1 s–1, and a reverse rate constant, kr = 18 s–1. If the system has a concentration of [A] = 0.15 M at equilibrium, what is the concentration of B at equilibrium? (no scientific notation)arrow_forwardGiven 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_forward
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