Solve a, b & c In a precipitation reaction, 0.679 g of BaSO4 were produce from a mixture of BaCl2 (aq)and NazSO4 (aq). Calculate the followings:BaCl2 (aq) + NazSO4 (aq)BaSO4 (s) +2NACI (aq)a. Moles of BaSO4 formedb. Moles of Bacl2 reactedc. Moles of Na2SO4 reactedd. Moles of NaCl formede. Mass of Na2SO4 reacted

A chemical reaction is a process in which one or more substances known as reactants are converted to…

In a precipitation reaction, 0.679 g of BaSO4 were produce from a mixture of BaCl2 (aq) and NazSO4 (aq). Calculate the followings: BaCl2 (aq) + Na2SO4 (aq) BaSO4 (s) +2NACI (aq) a. Moles of BaSO4 formed b. Moles of Bacl2 reacted c. Moles of Na2SO4 reacted d. Moles of NaCl formed e. Mass of Na2SO4 reacted

In a precipitation reaction, 0.679 g of BaSO4 were produce from a mixture of BaCl2 (aq) and NazSO4 (aq). Calculate the followings: BaCl2 (aq) + Na2SO4 (aq) BaSO4 (s) +2NACI (aq) a. Moles of BaSO4 formed b. Moles of Bacl2 reacted c. Moles of Na2SO4 reacted d. Moles of NaCl formed e. Mass of Na2SO4 reacted

Human Physiology: From Cells to Systems (MindTap Course List)

9th Edition

ISBN:9781285866932

Author:Lauralee Sherwood

Publisher:Lauralee Sherwood

Chapter3: The Plasma Membrane And Membrane Potential

Section: Chapter Questions

Problem 1SQE: Using the Nernst equation, calculate the equilibrium potential for Ca2 and for C1 from the following...

See similar textbooks

Similar questions

The Ksp values of silver chromate Ag2CrO4 and silver iodate Ag(IO3) are given below. Ag2CrO4 Ag(IO3) Ksp 1.12 x 10-12 3.17 x 10-8 Based on these Ksp values, which of the following is true? Choose one option only. Options: a. In the solution consisting of 1.00 x10-4 M Ag+ and 5.00 x10-5 M CrO42-, Ag2CrO4 precipitate will form. b. In the solution consisting of 1.0 x10-4 M Ag+ and 1.0 x10-4 M IO3-, Ag(IO3) precipitate will form. c. In pure water, the solubility of Ag2CrO4 is lower than the solubility of Ag(IO3). d. In the solution consisting of 0.200 M CrO42- and 0.200 M IO3-, Ag2(CrO4) will precipitate first if we add Ag+ ions gradually into the above mixture.
For the following reaction 3 experiments have been run and the data collected is in the following table @ 35 degrees Celsius 2 NO2F(g) ---> 2 NO2(g) + F2(g) Experiment [NO2F], M Rates, M/s 1 0.263 0.168 2 0.349 0.223 3 0.421 0.269 a) How long will it take for a 65% NO2F solution to become a 31% NO2F solution @35 degrees Celsius?(Hint: Use mass ratios and assume ~1g/ml for density of solutions to get you started) b) It has been determined that at 75 degrees Celsius the rate constant is 1.046 s-1. Calculate the activation energy for the decomposition of NO2F. [Hint: ]ln?1?2=?a?(1?2―1?1) c) What is the half-life of a 35% solution of NO2F @ 35 degrees Celsius?
You have an initial solution in which you added quantities of “A” and “B” such that there is 4.5 M “A” and 2.5 M “B” and no complex (“AB”) at time 0. After equilibrium, you are able to isolate and quantitate the “AB” complex, and find its concentration is 1.5 M. Given that RT is 0.59 kcal/mol, what is the delta Go’ for the association reaction?
if the absorbance of pure chlorophyll a in a 1 cm cell is 0.876 at 530 nm and the concentration is 8.66 x 10^-6 M, what is the molar extinction coefficient of chlorophyll a?
At 39.9ºC, a solution of ethanol (XetOH = 0.9006, P * etOH = 130.4 Torr) and isooctane (P * iso = 43.9 Torr) forms a vapor phase with YetOH = 0.6667. The total pressure is 185.9 a. Calculate the activity and the activity coefficient of each component.b. Calculate the total pressure the solution would have if it were ideal.c. Comparing the ideal pressure to the actual pressure, what does this indicate about the molecular interactions?
Why is it difficult to determine an exact number for P/O ratios?
The formation constants at 25°C for Fe(CN)4-6 and Fe(EDTA)2– are 1.00 x 1037 and 2.10 x 1014, respectively. Answer the questions below. 1) Calculate K under standard conditions for the reaction Fe(EDTA)2−(aq) + 6CN−(aq) ----> Fe(CN)4−6(aq) + EDTA4−(aq) 2) Calculate ΔG° for the reaction. (kJ/mol)
For the following reaction, 4.91 grams of water are mixed with excess chlorine gas. The reaction yields 12.5 grams of hydrochloric acid.chlorine (g) + water (l) hydrochloric acid (aq) + chloric acid (HClO3) (aq) What is the theoretical yield of hydrochloric acid ? grams What is the percent yield of hydrochloric acid ? %
Using the Nernst equation, calculate the equilibrium potential for Ca2 and for C1 from the following sets of data: a. Given [ Ca2+ ]0=1mM,[ Ca2+ ]i=100nM, find Eca2+ b. Given [ Cl- ]0=110mM,[ Cl- ]i=100mM, find Ecl
How many moles of Na2S2O3 would be required to react completely with 0.450 g of AgBr?
For the following reaction X + YA + B at 300 K, it is found equilibrium constant equal to 10. Therefore, AG & AGⓇ of the reaction at 300 K respectively are - Answer b
Consider a reaction with ΔH = 15 kJ and ΔS = 50 J · K−1. Is the reaction spontaneous (a) at 10°C, (b) at 80°C?