Question

A) Calculate the vapour pressure of a 5% by mass benzoic acid [C7H6O2(aq)] in ethanol solution...

A) Calculate the vapour pressure of a 5% by mass benzoic acid [C7H6O2(aq)] in ethanol solution at 35oC. The vapour pressure of pure ethanol at this temperature is 13.40 kPa. Present your answer in kPa.

B) The half-life of the zero order reaction A → B is 0.56 minutes. If the initial concentration of A is 3.4 M, what is the rate constant?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
a solution is 0.936 moles of benzoic acid (C7H6O2) dissolved in 4.832 moles acetone (C3H6O). Calculate...
a solution is 0.936 moles of benzoic acid (C7H6O2) dissolved in 4.832 moles acetone (C3H6O). Calculate the vapor pressue of the solution in a bttle that is in a room at 21.3 C. The vapor pressure of pure acetone at this temperature is 19450 torr.
Question 5: The reaction A(aq) → B(aq) is a first order reaction with respect to A(aq)....
Question 5: The reaction A(aq) → B(aq) is a first order reaction with respect to A(aq). The concentration of A(aq) is reduced from 0.822 M to 0.576 M in 3.16 minutes. What is the half-life, in seconds, of this reaction? Question 6: The reaction A(aq) → B(aq) + C(aq) is a first order reaction with respect to A(aq). The half-life of A(aq) is 93.2 s at 25.0oC and its half-life is 60.9 s at 75.0oC. What is its half-life at...
The equilibrium constant for the esterification of ethanol and aceticacid in an aqueous solution CH3COOH(aq) +...
The equilibrium constant for the esterification of ethanol and aceticacid in an aqueous solution CH3COOH(aq) + C2H5OH(aq) -----> CH3COOC2H5(aq) + H2O(l) amounts to 0.566 at 298 K. The reaction mixture initially contains 0.040 mol dm^−3 of acetic acid and 0.025 mol dm^−3 of ethanol. Find themolar concentration of ethyl acetate at the equilibrium. Assume that the pH is low enough that CH3COOH is not dissociated at all and thatthe activity of water equals 1 just like for pure liquid water...
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of...
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of H3O+ in the solution if the initial concentration of C6H5COOH is 6.3×10−2 M . Express your answer using two significant figures. Part B Calculate the equilibrium concentration of C6H5COO− in the solution if the initial concentration of C6H5COOH is 6.3×10−2 M . Part C Calculate the equilibrium concentration of C6H5COOH in the solution if the initial concentration of C6H5COOH is 6.3×10−2 M . Express...
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of...
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of H3O+ in the solution if the initial concentration of C6H5COOH is 6.3×10−2 M . Express your answer using two significant figures. Part B Calculate the equilibrium concentration of C6H5COO− in the solution if the initial concentration of C6H5COOH is 6.3×10−2 M . Part C Calculate the equilibrium concentration of C6H5COOH in the solution if the initial concentration of C6H5COOH is 6.3×10−2 M . Express...
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of...
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of H3O+ in the solution if the initial concentration of C6H5COOH is 6.6×10−2 M . Express your answer using two significant figures. [H3O+] =   M   SubmitRequest Answer Part B Calculate the equilibrium concentration of C6H5COO− in the solution if the initial concentration of C6H5COOH is 6.6×10−2 M . Express your answer using two significant figures. [C6H5COO−] =   M   SubmitRequest Answer Part C Calculate the equilibrium...
1. A 0.0450 M solution of benzoic acid has a pH of 2.71. Calculate pKa for...
1. A 0.0450 M solution of benzoic acid has a pH of 2.71. Calculate pKa for this acid. 2. A 0.0460 M solution of HA is 0.80% dissociated. Calculate pKa for this acid. 3. Consider a reaction mixture containing 100.0 mL of 0.112 M borate buffer at pH = pKa = 9.24. At pH = pKa, we know that [H3BO3] = [H2BO3−] = 0.0560 M. Suppose that a chemical reaction whose pH we wish to control will be generating acid....
The Standard Hydrogen Electrode (S.H.E.) consists of H2 gas bubbled through a solution of H+ ions;...
The Standard Hydrogen Electrode (S.H.E.) consists of H2 gas bubbled through a solution of H+ ions; which of the following conditions must be met to give E0 = 0.00V, as part of the S.H.E.? I. Temperature of cell is 298 K II. Pressure of the Hydrogen gas is 1 atm III. Concentration of H+ is 1.0 moldm-3 Select one: a. I and II only b. I and III only c. I only d. I, II and III Use the data...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare the NaOH Solution Take a 250 mL volumetric flask from the Containers shelf and a balance from the Instruments shelf and place them on the workbench. Zero the mass of the volumetric flask on the balance. Take sodium hydroxide from the Materials shelf and add 1 g to the flask. Record the mass from the balance display. Place the volumetric flask on the workbench....
A solution of a theoretical triprotic acid was prepared by dissolving 4.037 g of solid in...
A solution of a theoretical triprotic acid was prepared by dissolving 4.037 g of solid in enough DI water to make 500.0 mL of solution.   10.11 mL of a 0.592 M solution was required to titrate 20.00 mL of this acid's solution. Part A What is the concentration of the acid solution? Part B What is the molar mass of the acid? Hint: You need to calculate the total moles in the 500.0 mL solution (the full 500.0 mL was...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT