The reaction\[ \text{CO(g) + H}_2\text{O(g) } \rightleftharpoons \text{ CO}_2\text{(g) + H}_2\text{(g)} \]has an equilibrium constant \( K_c \) of 0.58 at 1000 °C. If a 90.0-L mixture of CO and H\(_2\)O has a concentration of each of \( 7.00 \times 10^{-2} \) mol/L, what amount (in moles) of each species will be present when the mixture reaches equilibrium?- \(\_\_\_\_\_\_\_\_\_\_\_\) mol CO- \(\_\_\_\_\_\_\_\_\_\_\_\) mol H\(_2\)O- \(\_\_\_\_\_\_\_\_\_\_\_\) mol CO\(_2\)- \(\_\_\_\_\_\_\_\_\_\_\_\) mol H\(_2\)

GIVEN: Concentration of CO= 7.00 x 10-2 mol/L Concentration of H2O= 7.00 x 10-2 mol/L Volume = 90.0 L Kc = 0.58 To calculate: Moles of CO,H2O,CO2 and H2 present at equilibrium ICE TABLE for the given reaction is: CO (g) + H2O (g) <--------------> CO2 (g) + H2 (g) INITIAL 0.07M 0.07 M CHANGE -x -x +x +x EQUILIBRIUM 0.07-x 0.07-x x x Expression for equilibrium constant can be expressed as: KC=CO2H2COH2O0.58=xx0.07-x0.07-x0.58 (0.07-x)2 =x2 0.58 (0.0049+x2-0.14x) =x2 0.002842 + 0.58 x2 -0.58014 x =x20.42 x2 +0.58014 x -0.002842 =0On solving the quadratic equation, we getx=0.00488156 MSo, equilibrium concentration of CO2 =0.004882 MH2= 0.004882 MCO= 0.07-0.004882 =0.0651 MH2O = 0.07 -0.004822 = 0.0651 MMoles = concentration x VolumeAt equilibriumMoles of CO2=0.004882 M ×90.0 L= 0.4394 molMoles of H2=0.004882 M ×90.0 L= 0.4394 molMoles of H2O= 0.0651 M ×90.0 L= 5.589 molMoles of CO= 0.0651 M ×90.0 L= 5.589 molAt equilibriumMoles of CO2= 0.4394 molMoles of H2= 0.4394 molMoles of H2O= 5.589 molMoles of CO= 5.589 mol

Science

Chemistry

The reaction CO(g) + H2O(g) 2 CO2(g)+ H2(g) has an equilibrium constant K̟ of 0.58 at 1000 °C. If a 90.0-L mixture of CO and H0 has a concentration of each of 7.00×10² mol/L, what amount (in moles) of each species will be present when the mixture reaches equilibrium? mol CO mol H20 mol CO2 mol H2

The reaction CO(g) + H2O(g) 2 CO2(g)+ H2(g) has an equilibrium constant K̟ of 0.58 at 1000 °C. If a 90.0-L mixture of CO and H0 has a concentration of each of 7.00×10² mol/L, what amount (in moles) of each species will be present when the mixture reaches equilibrium? mol CO mol H20 mol CO2 mol H2

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

The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K.NH4Cl(s) NH3(g) + HCl(g)If an equilibrium mixture of the three compounds in a 4.47 L container at 548 K contains 4.00 mol of NH4Cl(s) and 0.214 mol of NH3, the number of moles of HCl present is moles.
The equilibrium constant, K, for the following reaction is 6.59×10-2 at 546 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 6.59 L container at 546 K contains 0.254 M PCl5, 0.129 M PCl3 and 0.129 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.7 L? [PCl5] = M [PCl3] = M [Cl2] = M
The equilibrium constant, Kc, for the following reaction is 1.80 × 10-4 at 298 K. NH4HS(s) NH3(g) + H₂S(g) If an equilibrium mixture of the three compounds in a 4.30 L container at 298 K contains 3.12 mol of NH4HS(s) and 0.310 mol of NH3, the number of moles of H₂S present is | mol.
The equilibrium constant for the following reaction is 0.18 at a set temperature. Find the equilibrium concentrations if the initial concentration of PCl3 is 0.225 mol/L and the initial concentration of Cl2 is 0.150 mol/L. PCI3(g)+CI2(g)=PCI5(g)
The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g)If an equilibrium mixture of the three compounds in a 6.01 L container at 298 K contains 4.00 mol of NH4HS(s) and 0.432 mol of NH3, the number of moles of H2S present is moles.
The equilibrium constant, Kp, for the following reaction is 1.04×10-² at 548 K. NH4CI(S)2NH3(g) + HCI(g) If an equilibrium mixture of the three compounds in a 6.72 L container at 548 K contains 1.63 mol of NH4Cl(s) and 0.190 mol of NH3(g), the partial pressure of HCI(g) is I atm.
Consider the following reaction at a certain temperature: 4 Fe(s) + 3 O2(g)→ 2 Fe203(s) An equilibrium mixture contains 1.2 mol Fe, 0.00090 mol O2, and 2.0 mol Fez03 all in a 2.0-L container. Calculate the value of K for this reaction. K =
Some NOBR is placed in a sealed flask and heated to 385 K. When equilibrium is reached, the flask is found to contain NOBR (9.30×103 M), NO (1.27x102 M), and Br2 (1.18×102 M). What is the value of the equilibrium constant for this reaction at 385 K? 2NOBR(g)=2NO(g) + Br2(g) K=
The equilibrium constant, K. , for the following reaction is 5.10×10-6 at 548 K. NHẠC(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 7.80 L container at 548 K contains 2.74 mol of NH,Cl(s) and 0.323 mol of NH3, the number of moles of HCl present is moles.
At a certain temperature, the equilibrium constant K for the following reaction is 3.1 × 10 : H,(g) + I,(g) = 2 HI(g) Use this information to complete the following table. Suppose a 36. L reaction vessel is filled with 1.7 mol of HI. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little H2 and I2. There will be very little HI. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = 1 2 HI(g) H2(9)+I,(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = I 2 H,(9)+21½(9) 4 HI(g)
The equilibrium constant, Kc , for the following reaction is 7.00×10-5 at 673 K.NH4I(s) NH3(g) + HI(g)If an equilibrium mixture of the three compounds in a 4.05 L container at 673 K contains 2.71 mol of NH4I(s) and 0.262 mol of NH3, the number of moles of HI present is moles. --- The equilibrium constant, Kc, for the following reaction is 6.30 at 723K.2NH3(g) N2(g) + 3H2(g)If an equilibrium mixture of the three gases in a 12.1 L container at 723K contains 0.250 mol of NH3(g) and 0.208 mol of N2, the equilibrium concentration of H2 is M.