La réaction A(aq) → B(aq) + C(aq) est une réaction d'ordre un. La demie-vie de A(aq) est 94,1 s à 25.0°C et sa demie-vie est 70,1 s à 45.0°C. Quelle est sa demi-vie (en s) à 65.0°C?

The picture below is a representation of H(g) and O(g) in a sealed container Ona • Hag 2H2(g) + O,(g) → 2H,O(g) Which of the following pictures would best describe the products of the following reaction O A O B O D O E 00

A certain half-reaction has a standard reduction potential E =-1.25 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.80 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. h Data Ag+ (aq) + e Ag (s) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. Ered = v !! Al3+ (aq) + 3e-- Al (s) -1.676 Au+ (aq) + e Au (s) 1.692 If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Au3+ (aq) + 3e - Au (s) 1.498 O no minimum Ba2+ (ag) + 2e - Ba (s) -2.912 Brz (1) + 2e- 2Br (aq) 1.066 Ca2+ (ag) + 2e - Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? E=…

4. Enter the chemical equation 2H+(aq)+S2−(aq)→H2S(g)2H+(aq)+S2−(aq)→H2S(g)?

3. Now that you know the physical state of each of the reactants and products in this chemical reaction lets think about what you might observe as the reaction is running. CH_3COOH(aq) + NaHCO_3(aq) → H_2O(l) + CO_2(g) + CH_3COONa(aq)   Upload a screenshot that shows how you performed all the calculations in Q3.

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Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Sn2+] = 0.0564 M, [Fe+] = 0.0453 M, [Snª+] = 0.00585 M, and [Fe²+] = 0.01002 M. Standard reduction potentials can be found in this table. Sn²+ (aq) + 2 Fe³+(aq) = Snt+(aq) + 2 Fe²+(aq) E = 0.4478 V

Consider each chemical equation and select all that represent a chemical reaction.     2NaI(aq)  +  Pb(NO3)2(aq)  →  2NaNO3(aq)  +  PbI2(s)     2KBr(aq) + MgCl2(aq) → 2KCl(aq) + MgBr2(aq)     HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

Part 1 A student carried out an investigation to observe the effect of changing concentration of sulfuric acid on the breakdown of calcium carbonate (marble) chips. They changed the concentration of the acid between each test but kept the size of the marble chips constant. The full equation for the reaction and a graph of the overall results can be seen below. CaCO3(s) + H₂SO4(aq) → CaSO4(aq) + CO2(g) + H₂O (1) a) b) Rate of Reaction * Concentration of Acid (mol dm³) Explain, using collision theory, why the student obtained these results, and state what they could conclude about the effect of changing concentration of acid on the rate of reaction between calcium carbonate and sulfuric acid. If the student had ground up the calcium carbonate chips into a powder and run the tests again, what would you expect to happen to the rate of reaction? Briefly explain why by applying collision theory. Part 2 The student ran the same experiment, but this time changed the temperature, increasing it…

8H2S(g) + 4O2(g) → 8H2O(g) + S8(g) If Δ[H2S]/Δt = -0.062 mol·L−1·s−1, find Δ[O2]/Δt. Express your answer to two significant figures.