5B r â (aq)+Br O â 3 (aq)+6 H + (aq)â3B r 2 (aq)+3 H 2 O(l)
Consider the reaction 5B r â (aq)+Br O â 3 (aq)+6 H + (aq)â3B r 2 (aq)+3 H 2 O(l) The average rate of consumption of B r â is 1.55Ã10â4 M/s over the first two minutes. What is the average rate of formation of B r 2 during the same time interval? Express your answer numerically in molar per second to three significant figures.
5B r â (aq)+Br O â 3 (aq)+6 H + (aq)â3B r 2 (aq)+3 H 2 O(l)
Consider the reaction 5B r â (aq)+Br O â 3 (aq)+6 H + (aq)â3B r 2 (aq)+3 H 2 O(l) The average rate of consumption of B r â is 1.55Ã10â4 M/s over the first two minutes. What is the average rate of formation of B r 2 during the same time interval? Express your answer numerically in molar per second to three significant figures.
For unlimited access to Homework Help, a Homework+ subscription is required.
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
Chemistry: The Central Science
Related questions
Consider the reaction
2H3PO4âP2O5+3H2O
Determine the average rate of decomposition of H3PO4 between 10.0 and 40.0s.
Time (s) | 0 | 10.0 | 20.0 | 30.0 | 40.0 | 50.0 |
[P2O5] (M) | 0 | 1.90Ã10â3 | 4.90Ã10â3 | 6.70Ã10â3 | 7.90Ã10â3 | 8.50Ã10â3 |
Part B
Consider the reaction
5Brâ(aq)+BrOâ3(aq)+6H+(aq)â3Br2(aq)+3H2O(l)
The average rate of consumption of Brâ is 2.06Ã10â4M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval?
Pls Pls only answer if you are going to answer all of them and not just one or two thanks i got alot in my hands cuz of finals, and don't have time to do them, Appreciate it, trust that they'll be right , I posted this once but they only did one instead of all six so yeah thanks
1) The electrochemical cell described by the balanced chemical equation has a standard emf of 0.35 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures.
2MnO42-(aq) + 2Hg2+(aq) â 2MnO4-(aq) + Hg22+(aq)
St. Red. Pot. (V) | ||||
| ||||
Faraday's Constant | ||||
|
2) The voltaic cell described by the balanced chemical reaction has a standard emf of 4.05 V. Calculate the equilibrium constant (Kc) for the reaction at 25 oC. Round your answer to 3 significant figures. F2(g) + Mn(s) â 2F-(aq) + Mn2+(aq)
St. Red. Pot. (V) | ||||
| ||||
Constants | ||||
| ||||
Faraday's Constant | ||||
|
3) The voltaic cell described by the cell notation has an Eo of 0.68 V. Calculate the Wmax (kJ) the cell has done if 6.4700 mol of MnO4-(aq) (Molar Mass - 118.94 g/mol) reacts. Round your answer to 3 significant figures.
Pt(s) l VO2+(aq), VO2+(aq), H+(aq) ll H+(aq), MnO4-(aq) l MnO2(s) l Pt(s)
St. Red. Pot. (V) | ||||
| ||||
Faraday's Constant | ||||
|
4) The galvanic cell described by the cell notation has an Eo of 1.23 V. Calculate the value (kJ) for the ÎGË of the cell. Round your answer to 3 significant figures.
Pt(s), H2(g) l H2O(l), OH-(aq) ll O2(g) l OH-(aq) l Pt(s)
St. Red. Pot. (V) | ||||
| ||||
Faraday's Constant | ||||
|
5) The electrochemical cell described by the balanced chemical equation has a standard cell potential of -0.37 V. Calculate the value (kJ) for the standard free energy change of the cell. Round your answer to 3 significant figures.
Sn4+(aq) + 2Cu(s) â Sn2+(aq) + 2Cu+(aq)
St. Red. Pot. (V) | ||||
| ||||
Faraday's Constant | ||||
|
6)The electrochemical cell described by the cell notation has an Eocell of 4.05 V. Calculate the maximum electrical work (kJ) the cell has done if 375.44 g of F2(g) (Molar Mass - 38.00 g/mol) reacts. Round your answer to 3 significant figures.
Mn(s) l Mn2+(aq) ll F2(g) l F-(aq) l Pt(s)
St. Red. Pot. (V) | ||||
| ||||
Faraday's Constant | ||||
|