Be sure to answer all parts. The water-gas shift reaction plays a central role in the...

Be sure to answer all parts. The water-gas shift reaction plays a central role in the chemical methods for obtaining cleaner fuels from coal: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) A study was made in which equilibrium was reached with [CO] = [H2O] = [H2] = 0.100 M and [CO2] = 0.400 M. After 1.40 mol of H2 is added to the 2.00−L container and equilibrium is reestablished, what are the new concentrations of all the components?

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queen_honey_blossom answered 2 years ago

The water-gas shift reaction plays a central role in the chemical methods of obtaining clean fuels...

The water-gas shift reaction plays a central role in the chemical methods of obtaining clean fuels from coal. CO (g) + H2O (g)= CO2 (g) + H2 (g) A study was made in which equilibrium was reached with [CO]=[H2O]=[H2]=0.100M and [CO2]=0.400M. After 0.800 mol of H2 is added to the 2.00L container and equilibrium is reestablished, what are the new concentrations of all the components?

Be sure to answer all parts. Chlorine oxide (ClO), which plays an important role in the...

Be sure to answer all parts. Chlorine oxide (ClO), which plays an important role in the depletion of ozone, decays rapidly according to the equation 2ClO(g) → Cl2(g) + O2(g) From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) [ClO] (M) 3.59 × 10−3 8.44 × 10−6 4.21 × 10−3 7.22 × 10−6 4.83 × 10−3 6.31 × 10−6 5.45 × 10−3 5.60 × 10−6 6.07 × 10−3 5.04 × 10−6

Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen...

Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) 1. Calculate the mass of ammonia produced when 30.0 g of nitrogen react with 11.3 g of hydrogen. 2. Which is the excess reactant and how much of it will be left over when the reaction is complete?

The water gas shift reaction involves the reaction of carbon monoxide with water vapor to form...

The water gas shift reaction involves the reaction of carbon monoxide with water vapor to form carbon dioxide and hydrogen gas: CO(g) + H2O(g) → CO2(g) + H2(g) 28.01 g CO and 9.01 g water vapor are combined in a reaction vessel. At the end of the reaction, a total pressure of 945.3 torr is found. A.) Which gases are left at the end of the reaction? B.) What are mole fractions of the gases left in the reaction vessel...

19. Be sure to answer all parts. At 1000 K, a sample of pure NO2 gas...

19. Be sure to answer all parts. At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) ⇌ 2NO(g) + O2(g) The equilibrium constant, KP, is 158. Analysis shows that the partial pressure of O2 is 0.35 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture. Pressure of NO: atm Pressure of NO2: atm

Be sure to answer all parts. Consider the following reaction at equilibrium: A(g) ⇆ 2B(g) From...

Be sure to answer all parts. Consider the following reaction at equilibrium: A(g) ⇆ 2B(g) From the data shown here, calculate the equilibrium constant (both KP and Kc) at each temperature. Is the reaction endothermic or exothermic? Temperature (°C) [A] (M) [B] (M) 200 0.0180 0.870 300 0.150 0.790 400 0.240 0.695 Kc(200°C) = KP(200°C) = Kc(300°C) = KP(300°C) = Kc(400°C) = KP(400°C) = Cannot be determined. The reaction is exothermic. The reaction is endothermic

Be sure to answer all parts. At 1280°C the equilibrium constant Kc for the reaction Br2(g)...

Be sure to answer all parts. At 1280°C the equilibrium constant Kc for the reaction Br2(g) ⇌ 2Br(g) is 1.1 ×10−3. If the initial concentrations are [Br2] = 0.0320 M and [Br] = 0.0290 M, calculate the concentrations of these two species at equilibrium. [Br2]eq = [Br]eq =

Be sure to answer all parts. The equilibrium constant Kc for the Reaction: H2(g) + CO2(g)...

Be sure to answer all parts. The equilibrium constant Kc for the Reaction: H2(g) + CO2(g) <--> H2O(g) + CO(g) is 4.2 at 1650 C. Initially 0.87 mol H2 and 0.87 mol CO2 are injected into a 4.9 L flask. Calculate the concentraion of each species at equilibrium Equilibrium concentration of H2: ____ M Equilibrium concentraion of CO2: ___ M Equilibrium concentraion of H2O: _____M Equilibrium concentration of CO: ______M

Consider the water-shift gas reaction: H2O + CO --> H2 + CO2 A closed reaction vessel...

Consider the water-shift gas reaction: H2O + CO --> H2 + CO2 A closed reaction vessel maintained at 3000 degrees Celcius is filled with 0.475 M H2 and 0.490 M CO2. At equilibrium, their respective concentrations are 0.410 and 0.425 M. PART A: The following ratio represents [H2][CO2] / [H2O][CO] CHOOSE ONE OR MORE: the law of mass action, the mass action expression, the equilibrium constant expression, the equilibrium constant. none of these PART B: which way must the system...

The most important commercial process for generating hydrogen gas is the water-gas shift reaction: CH4(g) +...

The most important commercial process for generating hydrogen gas is the water-gas shift reaction: CH4(g) + H2O(g) → CO(g) + 3H2(g) a) Use tabulated thermodynamic data to find ΔG° for this reaction at the standard temperature of 25°C. b) Now calculate ΔG°1100 for this process when it occurs at 1100 K.

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