Question

Part A Calculate the number of moles of B at 10 min , assuming that there...

Part A

Calculate the number of moles of B at 10 min , assuming that there are no molecules of B at time zero.

Express your answer using two significant figures.

SubmitMy AnswersGive Up

Part B

Calculate the number of moles of B at 20 min , assuming that there are no molecules of B at time zero.

Express your answer using two significant figures.

Part C

Calculate the number of moles of B at 30 min , assuming that there are no molecules of B at time zero.

Express your answer using two significant figures.

Part D

Calculate the number of moles of B at 40 min , assuming that there are no molecules of B at time zero.

Express your answer using two significant figures.

Consider the following hypothetical aqueous reaction: A(aq)→B(aq) . A flask is charged with 0.065 mol of A in a total volume of 100.0 mL . The following data are collected:
Time (min) 0 10 20 30 40
Moles of A 0.065 0.051 0.042 0.036 0.031
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
Consider the following hypothetical aqueous reaction: A(aq)→B(aq). A flask is charged with 0.065 mol of A...
Consider the following hypothetical aqueous reaction: A(aq)→B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 Part A Calculate the average rate of disappearance of A between t= 30 min and t= 40 min, in units of M/s. Express your answer using two significant figures. Part B Between t= 10 min and t=...
1) Time(min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 -...
1) Time(min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 - Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time B at time zero, and that A cleanly converts to B with no intermediates. - Calculate the average rate of disapperance of A for each 10-min interval in units of M/s. - Between t=10 min and t=30 min, what is the...
How many moles of NaCl are contained in each solution? Part A 1.8 L of a...
How many moles of NaCl are contained in each solution? Part A 1.8 L of a 1.2 M NaCl solution Express your answer using two significant figures. mol SubmitMy AnswersGive Up Part B 0.408 L of a 0.95 M NaCl solution Express your answer using two significant figures. mol SubmitMy AnswersGive Up Part C 159 mL of a 1.85 M NaCl solution Express your answer using three significant figures. mol SubmitMy AnswersGive Up
Calculate the equilibrium constant at 25 ∘C for each of the following reactions: Part A Cd(s)+Sn2+(aq)→Cd2+(aq)+Sn(s)...
Calculate the equilibrium constant at 25 ∘C for each of the following reactions: Part A Cd(s)+Sn2+(aq)→Cd2+(aq)+Sn(s) Express your answer using one significant figures. K = 6×108 SubmitMy AnswersGive Up Correct Part B 2Al(s)+3Cd2+(aq)→2Al3+(aq)+3Cd(s) Express your answer using one significant figures. K = 5×10127 SubmitMy AnswersGive Up Correct Part C Cr2O2−7(aq)+6Fe2+(aq)+14H+(aq)→2Cr3+(aq)+6Fe3+(aq)+7H2O(l) Express your answer using one significant figures. K = 2•1057 SubmitMy AnswersGive Up Just need Part C
The acid-dissociation constant for hypochlorous acid (HClO) is 3.0×10−8. Part A Calculate the concentration of H3O+...
The acid-dissociation constant for hypochlorous acid (HClO) is 3.0×10−8. Part A Calculate the concentration of H3O+ at equilibrium if the initial concentration of HClO is 8.6×10−3 M . Express your answer using two significant figures. [H3O+] =   M   SubmitMy AnswersGive Up Part B Calculate the concentration of ClO− at equilibrium if the initial concentration of HClO is 8.6×10−3 M . Express your answer using two significant figures. [ClO−] =   M   SubmitMy AnswersGive Up Part C Calculate the concentration of HClO...
Problem 16.45 Part A Calculate [OH−] for 1.0×10−3 M Sr(OH)2. Express your answer using two significant...
Problem 16.45 Part A Calculate [OH−] for 1.0×10−3 M Sr(OH)2. Express your answer using two significant figures. [OH−] = 2.0×10−3   M   SubmitMy AnswersGive Up Correct Part B Calculate pH for 1.0×10−3 M Sr(OH)2. Express your answer using two decimal places. pH = 11.30 SubmitMy AnswersGive Up Correct Part C Calculate [OH−] for 2.500 g of LiOH in 220.0 mL of solution. Express your answer using four significant figures. [OH−] = 0.4745   M   SubmitMy AnswersGive Up Correct Significant Figures Feedback: Your...
Oxycodone (C18H21NO4), a narcotic analgesic, is a weak base with pKb=5.47. Part A Calculate the pH...
Oxycodone (C18H21NO4), a narcotic analgesic, is a weak base with pKb=5.47. Part A Calculate the pH in a 0.00270 M oxycodone solution. Express your answer using three significant figures. pH = 9.97 SubmitMy AnswersGive Up Correct Part B Calculate the concentrations of C18H21NO4 in a 0.00270 M oxycodone solution. Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part C Calculate the concentrations of HC18H21NO+4 in a 0.00270 M oxycodone solution. Express your answer...
Problem 16.63 Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the...
Problem 16.63 Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook). Part A 0.388 M . Express your answer using two significant figures.   %   SubmitMy AnswersGive Up Part B 0.117 M . Express your answer using two significant figures.   %   SubmitMy AnswersGive Up Part C 3.61×10−2 M . Express your answer using two significant figures.   %  
Part A Calculate the pH of 0.100 L of a buffer solution that is 0.23 M...
Part A Calculate the pH of 0.100 L of a buffer solution that is 0.23 M in HF (Ka = 3.5 x 10-4 ) and 0.45 M in NaF. Express your answer using three significant figures. pH = SubmitMy AnswersGive Up Part B What is the pH after adding 0.001 mol of HNO3 to the buffer described in Part A? Express your answer using three significant figures. pH = SubmitMy AnswersGive Up Part C What is the pH after adding...
A 100.0 mL flask is filled with 0.065 moles of A and allowed to react to...
A 100.0 mL flask is filled with 0.065 moles of A and allowed to react to form B according to the reaction below. The following experimental data are obtained for the amount of A as the reaction proceeds. What is the average rate of appearance of B in units of M/s between t = 10 min. and t = 30 min.? Assume that the volume of the flask is constant. A(g) → B(g) Time 0.0 10.0 20.0 30.0 40.0 Moles...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT