Question

[4] Please calculate the volume for H2 gas at 25°C and 1.00 atm that will college...

[4] Please calculate the volume for H2 gas at 25°C and 1.00 atm that will college at the cathode when an (aq) solution of Na2SO4 is electrolyzed for 2.00 hours with a 10.0-amp current.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

2 hours means

Thus , total charge -

According to Faraday's law , if 96486 C charge is passed , then 1 equivalent is deposited.

Thus, total production of H2 is-

For , H2 , 2 equivalent means 1 mol.

Thus , total H2 produced is -

From Ideal gas equation ,

Thus,

[ANSWER]

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
1. Calculate the equilibrium constant Keq for the following reaction at 25°C: 3Fe2+(aq) + 2Cr(s) ↔...
1. Calculate the equilibrium constant Keq for the following reaction at 25°C: 3Fe2+(aq) + 2Cr(s) ↔ 3Fe(s) + 2Cr3+(aq) 3.8 x 10–31 7.2 x 10–11 1.4 x 1010 2.6 x 1030 1.6 x 1015 2. A 1M aqueous solution of copper(II) nitrate is electrolyzed. What are the predicted products at the anode and cathode? N2 gas at the anode; copper metal at the cathode O2 gas at the anode; copper metal at the cathode NO2 gas at the anode; copper...
Could someone please explain how to do this in detail please? If an aqueous solution of...
Could someone please explain how to do this in detail please? If an aqueous solution of HNO3 is electrolyzed for 24.00 min at a steady current of 1.09 A, what volume of H2 (g) at 25.0oC and 0.99 atm will be collected at the cathode?
What volume of air contains 10.0 g of oxygen gas at 273 K and 1.00 atm?
What volume of air contains 10.0 g of oxygen gas at 273 K and 1.00 atm?
4. Three moles of a monatomic ideal gas are initially at a pressure of 1.00 atm...
4. Three moles of a monatomic ideal gas are initially at a pressure of 1.00 atm and a temperature of 20.0OC. The gas is compressed adiabatically to a final pressure of 5.00 atm. Find: (a) the initial volume of the gas; (b) the final volume of the gas; (c) the final temperature of the gas; (d) the work done by the gas during the compression. Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8 atm-L Please show...
Calculate the volume of CO2 produced at 37°C and 1.00 atm when 4.78 g of glucose...
Calculate the volume of CO2 produced at 37°C and 1.00 atm when 4.78 g of glucose is used up in the reaction.
Calculate ∆E and the work done in joules when 50.0 g of tin (MM = 118.7...
Calculate ∆E and the work done in joules when 50.0 g of tin (MM = 118.7 g/mol) dissolves in excess acid producing 10.3 L of H2 (MM = 2.016 g/mol) gas at 1.00 atm and 25°C. The initial volume of gas is 0 L. Sn (s) + 2H+ (aq) → Sn2+ (aq) + H2 (g) ∆Hrxn = -137 kJ
The production of hydrogen chloride gas (HCl) at 1.0 atm and 25°C is represented by the...
The production of hydrogen chloride gas (HCl) at 1.0 atm and 25°C is represented by the following thermochemical equation. H2(g) + Cl2(g) → 2 HCl(g);     ΔH = −184.6 kJ Suppose exactly 4 mol H2(g) reacts with exactly 4 mol Cl2(g) to form HCl(g) under the same conditions of temperature and pressure. (a) Calculate the amount of pressure-volume work that is done. kJ (b) Calculate the change in internal energy (ΔE) of the system, assuming the reaction proceeds to completion. kJ
Mg metal reacts with HCl to produce hydrogen gas. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) What volume of hydrogen at 0...
Mg metal reacts with HCl to produce hydrogen gas. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) What volume of hydrogen at 0 ∘C and 1.00 atm (STP) is released when 8.80 g of Mg reacts? Express your answer with the appropriate units. How many grams of magnesium are needed to prepare 5.75 L of H2 at 745 mmHg and 16 ∘C? Express your answer with the appropriate units.
A gas sample has a volume at 2.0 L at 0.75 atm and 25 •C. What...
A gas sample has a volume at 2.0 L at 0.75 atm and 25 •C. What is the volume of the pressure is increased to 1.75 atm at constant temperature ?
Calculate the volume (in mL) of CO2 at 25 oC and 1.0 atm dissolved in a...
Calculate the volume (in mL) of CO2 at 25 oC and 1.0 atm dissolved in a 10.0 L bucket of rainwater that has pH of 4.5. The answer is supposed to be 580 but I keep getting 568. Please Help!
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT