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Please write clearly and show all work, with correct units, for full credit. This completed quiz...
im having trouble solving both of these please help, thank you Tutored Practice Problem 16.3.1 Close...
im having trouble solving both of these please help, thank
you
Tutored Practice Problem 16.3.1 Close Probl Use equilibrium concentrations to calculate K Some SO3 is placed in a flask and heated to 1350 K. When equilibrium is reached, the flask is found to contain SO, (6.58s 103 M), So, (3.ss-102 M), and O (1.53x102 M). What is the value of the equilibrium constant for the following at reaction at 1350 K? (0-(a)ost(afost K Check &Submit Answer Show Approach Tutored...
JUS Date Section 01 02 For full credit, please show all work clearly and give answers...
JUS Date Section 01 02 For full credit, please show all work clearly and give answers to the correct number of significant figures. This quiz will be chie at the start of class on Friday November 8, 2019 1. per total) a. What are the hydronium ion concentration and the hydroxide ion concentration in pure water? (OH) - b. Write the equilibrium constant expression for pure water, including its value. K, c. What are the pH and pOH values for...
Use an ICE table to calculate K A mixture of H, and I, is allowed to react at 661 K H2(g) + 12(g) +2HI(g) The initi...
Use an ICE table to calculate K A mixture of H, and I, is allowed to react at 661 K H2(g) + 12(g) +2HI(g) The initial concentration of the reactants are (Hy] -0.1960 M and [1,1 -0.2130 M. After the system reaches equilibrium, it is found that the l, concentration has decreased to 0.0506 M. Based on these data, determine the value of the equilibrium constant, K, for this reaction.
Show all work for full credit. You would like to determine the equilibrium constant for the bindi...
please help me with filling the table and show me how
you did it. thanks
Show all work for full credit. You would like to determine the equilibrium constant for the binding of a ligand to a metal ion: Mt" + L-<-> ML2+, where K-[([M1.*.1)/(M1")(し11. The ML-complex has aunique absorbance in the visible region, so its concentration at equilibrium can be determined by measuring the absorbance of the solution at an appropriate wavelength. An ICE table can used to determine...
CHM1046L, Quiz 4 Practice, Exp. 9 --- Show all work with units. Equations: pH = -log[1],...
CHM1046L, Quiz 4 Practice, Exp. 9 --- Show all work with units. Equations: pH = -log[1], pH + pOH = 14, pH = pka + log HA 1. The concentration of HNO, is 1 M, calculate its pH and pOH. 2. The concentration of NaOH is 10 M, calculate its pOH and pH. Suppose a buffer (PK, - 4) contained 5 moles of HA and 5 moles of A, calculate the pH when: A. 1 mole of HCl is added....
ice box quadraric formula please show work and write neat to understand. What is the concentration...
ice box
quadraric formula
please show work and write neat to understand.
What is the concentration of all species at equilibrium if the initial concentrations were 0.10 M for CO2 and 0.30 M for HZ? K=25. CO(g) + H2O(g) CO2(g) + H2(g) Initial Change Equilibrium
Please show all work. Provide equations used for full credit. Please use correct significant figures and...
Please show all work. Provide equations used for full credit. Please use correct significant figures and correct units in answers. The reaction, 2NOBr(g) + 2NO(g) + Br2(8) has an equilibrium constant, K = 0.42 at 373 K. a. Calculate Agºrxn at 373 K. b. Using the value of AHºrxn = 45.38 k) and the AGºrxn calculated in part a, calculate the ASºrxn at 373 K. Consider the reaction: 2NO(g) + C12(8) + 2NOCI(g) Given the following table of thermodynamic data,...
Consider the chemical reaction below at a given temperature and at equilibrium: H2(g) +12(g) = 2HI(g)...
Consider the chemical reaction below at a given temperature and at equilibrium: H2(g) +12(g) = 2HI(g) Kc = 53.3 If 0.800 mol of H2 and 0.800 mol of 12 are placed in a 1.00L container and allowed to react, what is the [HI] when the reaction reaches equilibrium? [HIN In the expression for K N- (H2] [12]' The equilibrium concentrations can be expressed as follows: NOTE: This is NOT asking for the concentrations you solve for this is literally asking...
Help please with work Show your work when there are calculations, write units where appropriate, and...
Help please with work
Show your work when there are calculations, write units where appropriate, and use the correct significant figures. Do the work on a separate sheet of paper and once you have done it correctly, transcribe youir work clearly onto this sheet. 1. The value of Ke for the equilibrium: is 794 at 25°C a) At this temperature, what is the value of Ke for the following equilibrium? H2(g) + 12(g)% 2H1(g) HI(g)与½ H2(g) + ½ 12(g) b)...
Please show work! Calculate equilibrium concentrations A closed system initially containin 1.000 x 10-3 M H2(g)...
Please show work!
Calculate equilibrium concentrations A closed system initially containin 1.000 x 10-3 M H2(g) and 2.000 x 10-3 M 12(9) at 448 °C is allowed to form HI and reach equilibrium. Analysis of the equilibrium mixture shows that the concentration of HI is 1.87 x Calculate K, at 448 °C for the reaction. a) 935 b) 27000 c) 4.00 d) 50.5
im having trouble solving both of these please help, thank
you
Tutored Practice Problem 16.3.1 Close Probl Use equilibrium concentrations to calculate K Some SO3 is placed in a flask and heated to 1350 K. When equilibrium is reached, the flask is found to contain SO, (6.58s 103 M), So, (3.ss-102 M), and O (1.53x102 M). What is the value of the equilibrium constant for the following at reaction at 1350 K? (0-(a)ost(afost K Check &Submit Answer Show Approach Tutored...
JUS Date Section 01 02 For full credit, please show all work clearly and give answers to the correct number of significant figures. This quiz will be chie at the start of class on Friday November 8, 2019 1. per total) a. What are the hydronium ion concentration and the hydroxide ion concentration in pure water? (OH) - b. Write the equilibrium constant expression for pure water, including its value. K, c. What are the pH and pOH values for...
Use an ICE table to calculate K A mixture of H, and I, is allowed to react at 661 K H2(g) + 12(g) +2HI(g) The initial concentration of the reactants are (Hy] -0.1960 M and [1,1 -0.2130 M. After the system reaches equilibrium, it is found that the l, concentration has decreased to 0.0506 M. Based on these data, determine the value of the equilibrium constant, K, for this reaction.
please help me with filling the table and show me how
you did it. thanks
Show all work for full credit. You would like to determine the equilibrium constant for the binding of a ligand to a metal ion: Mt" + L-<-> ML2+, where K-[([M1.*.1)/(M1")(し11. The ML-complex has aunique absorbance in the visible region, so its concentration at equilibrium can be determined by measuring the absorbance of the solution at an appropriate wavelength. An ICE table can used to determine...
CHM1046L, Quiz 4 Practice, Exp. 9 --- Show all work with units. Equations: pH = -log[1], pH + pOH = 14, pH = pka + log HA 1. The concentration of HNO, is 1 M, calculate its pH and pOH. 2. The concentration of NaOH is 10 M, calculate its pOH and pH. Suppose a buffer (PK, - 4) contained 5 moles of HA and 5 moles of A, calculate the pH when: A. 1 mole of HCl is added....
ice box
quadraric formula
please show work and write neat to understand.
What is the concentration of all species at equilibrium if the initial concentrations were 0.10 M for CO2 and 0.30 M for HZ? K=25. CO(g) + H2O(g) CO2(g) + H2(g) Initial Change Equilibrium
Please show all work. Provide equations used for full credit. Please use correct significant figures and correct units in answers. The reaction, 2NOBr(g) + 2NO(g) + Br2(8) has an equilibrium constant, K = 0.42 at 373 K. a. Calculate Agºrxn at 373 K. b. Using the value of AHºrxn = 45.38 k) and the AGºrxn calculated in part a, calculate the ASºrxn at 373 K. Consider the reaction: 2NO(g) + C12(8) + 2NOCI(g) Given the following table of thermodynamic data,...
Consider the chemical reaction below at a given temperature and at equilibrium: H2(g) +12(g) = 2HI(g) Kc = 53.3 If 0.800 mol of H2 and 0.800 mol of 12 are placed in a 1.00L container and allowed to react, what is the [HI] when the reaction reaches equilibrium? [HIN In the expression for K N- (H2] [12]' The equilibrium concentrations can be expressed as follows: NOTE: This is NOT asking for the concentrations you solve for this is literally asking...
Help please with work
Show your work when there are calculations, write units where appropriate, and use the correct significant figures. Do the work on a separate sheet of paper and once you have done it correctly, transcribe youir work clearly onto this sheet. 1. The value of Ke for the equilibrium: is 794 at 25°C a) At this temperature, what is the value of Ke for the following equilibrium? H2(g) + 12(g)% 2H1(g) HI(g)与½ H2(g) + ½ 12(g) b)...
Please show work!
Calculate equilibrium concentrations A closed system initially containin 1.000 x 10-3 M H2(g) and 2.000 x 10-3 M 12(9) at 448 °C is allowed to form HI and reach equilibrium. Analysis of the equilibrium mixture shows that the concentration of HI is 1.87 x Calculate K, at 448 °C for the reaction. a) 935 b) 27000 c) 4.00 d) 50.5
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