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![Nics) + 2H+ (?) - Ni2C1.00) +H2 cp) Ecell = E cathode - Eanode 30- (-0.25) = 0.25V E ceft = Eº - 0-0 S116 - Net] H , 2 CH+J2](http://img.homeworklib.com/questions/12a47520-1378-11ea-aef8-fd1cc42d9742.png?x-oss-process=image/resize,w_560)
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2reg Consider the following cell reaction: Ni(s) + 2 H'(? M) Nº*(1.00 M) + H2(g) 1.00 atm) If the cell potential at...
Consider the following cell reaction: Mn(s) + 2 H+(? M) Mn2+(1.00 M) + H2(g)(1.00 atm) If...
Consider the following cell reaction:
Mn(s) + 2 H+(? M) Mn2+(1.00
M) + H2(g)(1.00 atm)
If the cell potential at 298 K is 1.01 volts, what
is the pH of the hydrogen electrode?
pH = ???
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and...
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown [H+]. If the cell potential is 0.204 V, what is the pH of the unknown solution at 298 K? b.) An electrochemical cell is constructed in which a Cr3+(1.00 M)|Cr(s) half-cell is connected to an H3O+(aq)|H2(1 atm) half-cell with unknown H3O+ concentration. The measured cell voltage is 0.366...
Could someone help me? I slipped in a previous example for reference Consider the following cell...
Could someone help me? I
slipped in a previous example for reference
Consider the following cell reaction: Fe(s) + 2 H+(?M —Fe2+(1.00 M)+H gX1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH= Consider the following cell reaction: Ni(s) + 2 H (?M) —+NI+(1.00 M)+H(E)1.00 atm) If the cell potential at 298 K is 0.104 volts, what is the pH of the hydrogen electrode? pH - 1.75 x Incorrect...
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the...
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (PH,)= latm) immersed in a solution of unknown [HT]. If the cell potential is 0.208 V, what is the pH of the unknown solution at 298 K? pH = Submit Answer Retry Entire Group 9 more group attempts remaining
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 3.84x10-3 atm, the H concentration is 1.14M, and the Ni2+ concentration is 3.54x10-4M ? 24+ (aq) + Ni(8)— H2(g) + Ni2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations giver true false Retry Entire Group 8 more group attempts remaining Submit Answer
This is the third time I've posted this question. Can someone please help me with the...
This is the third time I've
posted this question. Can someone please help me with the top one.
I slipped in a similar example. And the answer is not 2.4135
Consider the following cell reaction Fe(s)2 H ? M)-Fe2(100 M) +H>(g\1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH Consider the following cell reaction Ni(s)2 H (? M) Ni(100 M)Hg100 atm) If the cell potential at 298 K...
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 7.48*10-3 atm, the H concentration is 1.31M, and the Fe2+ concentration is 2.73x10M? 2H+ (aq) + Fe(s)→ H2(g) + Fe2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations giver true false Submit Answer Retry Entire Group 7 more group attempts remaining
What is the calculated value of the cell potential at 298 K for an electrochemical cell...
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 5.79 x 10-4 M and the Mg2+ concentration is 1.03 M ? Hg2+ (aq) + Mg(s) → Hg(1) + Mg2+ (aq) Ecell = V The cell reaction as written above is for the concentrations given. Submit Answer Retry Entire Group 8 more group attempts remaining
A student ran the following reaction in the laboratory at 684 K: H2(g) + 12(g) 22HI(g)...
A student ran the following reaction in the laboratory at 684 K: H2(g) + 12(g) 22HI(g) When she introduced H2(g) and Iz() into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.88 atm and the initial partial pressure of I was 3.74 atm, she found that the equilibrium partial pressure of 12 was 0.465 atm. Calculate the equilibrium constant, Kp. she obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more...
A student ran the following reaction in the laboratory at 690. K: H2(g) +12(g) 22HI(g) When...
A student ran the following reaction in the laboratory at 690. K: H2(g) +12(g) 22HI(g) When he introduced H2(g) and 12(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.40 atm and the initial partial pressure of I was 3.28 atm, he found that the equilibrium partial pressure of HI was 5.78 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group...
Consider the following cell reaction:
Mn(s) + 2 H+(? M) Mn2+(1.00
M) + H2(g)(1.00 atm)
If the cell potential at 298 K is 1.01 volts, what
is the pH of the hydrogen electrode?
pH = ???
Could someone help me? I
slipped in a previous example for reference
Consider the following cell reaction: Fe(s) + 2 H+(?M —Fe2+(1.00 M)+H gX1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH= Consider the following cell reaction: Ni(s) + 2 H (?M) —+NI+(1.00 M)+H(E)1.00 atm) If the cell potential at 298 K is 0.104 volts, what is the pH of the hydrogen electrode? pH - 1.75 x Incorrect...
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (PH,)= latm) immersed in a solution of unknown [HT]. If the cell potential is 0.208 V, what is the pH of the unknown solution at 298 K? pH = Submit Answer Retry Entire Group 9 more group attempts remaining
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 3.84x10-3 atm, the H concentration is 1.14M, and the Ni2+ concentration is 3.54x10-4M ? 24+ (aq) + Ni(8)— H2(g) + Ni2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations giver true false Retry Entire Group 8 more group attempts remaining Submit Answer
This is the third time I've
posted this question. Can someone please help me with the top one.
I slipped in a similar example. And the answer is not 2.4135
Consider the following cell reaction Fe(s)2 H ? M)-Fe2(100 M) +H>(g\1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH Consider the following cell reaction Ni(s)2 H (? M) Ni(100 M)Hg100 atm) If the cell potential at 298 K...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 7.48*10-3 atm, the H concentration is 1.31M, and the Fe2+ concentration is 2.73x10M? 2H+ (aq) + Fe(s)→ H2(g) + Fe2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations giver true false Submit Answer Retry Entire Group 7 more group attempts remaining
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 5.79 x 10-4 M and the Mg2+ concentration is 1.03 M ? Hg2+ (aq) + Mg(s) → Hg(1) + Mg2+ (aq) Ecell = V The cell reaction as written above is for the concentrations given. Submit Answer Retry Entire Group 8 more group attempts remaining
A student ran the following reaction in the laboratory at 684 K: H2(g) + 12(g) 22HI(g) When she introduced H2(g) and Iz() into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.88 atm and the initial partial pressure of I was 3.74 atm, she found that the equilibrium partial pressure of 12 was 0.465 atm. Calculate the equilibrium constant, Kp. she obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more...
A student ran the following reaction in the laboratory at 690. K: H2(g) +12(g) 22HI(g) When he introduced H2(g) and 12(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.40 atm and the initial partial pressure of I was 3.28 atm, he found that the equilibrium partial pressure of HI was 5.78 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group...
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