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MArishka [77]
2 years ago
8

A current of 0.15 A is passed through an aqueous solution of K2PtCl4. How long will it take to deposit 1.00 g Pt(s) (M = 195.1)?

Chemistry
1 answer:
koban [17]2 years ago
7 0

First calculate the electric charge used to deposit 1.0 g Pt

C = (1.0 g Pt) (1 mol Pt / 195.1 g Pt) ( 2 mol e / 1 mol Pt) ( 96485 C / 1 mol e)

C = 989.08 C

C = It

Where I is the current

T is the time

T = C / i

T = 989.08 C / 0.15 A

T = 6593.88 s

T = 1.83 hrs

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2 years ago
When 1 mol of KBr(s) decomposes to its elements, 394 kJ of heat is absorbed. (a) Write a balanced thermochemical equation.
VladimirAG [237]

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<h3>What is thermochemical equation? </h3>

A Thermochemical Equation is defined as the balanced stoichiometric chemical equation which includes the enthalpy change, ΔH.

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KBr ----- K + Br2

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learn more about thermochemical equation:

brainly.com/question/2733624

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Answer:

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3 0
3 years ago
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