Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°c. (the equation is balanced.) 3 cl2(g) + 2 fe(s) → 6 cl⁻(aq) + 2 fe3+(aq) cl2(g) + 2 e⁻ → 2 cl⁻(aq) e° = +1.36 v fe3+(aq) + 3 e⁻ → fe(s) e° = -0.04 v
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Chemistry, 22.06.2019 04:40
*will mark you brainliest + 15 points ** why does the equilibrium of a system shift when the pressure is increased? a. to maximize the stress on the system b. to stop restoring equilibrium to the system c. to increase the total moles of gas in the system d. to decrease the total moles of gas in the system
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Chemistry, 22.06.2019 14:30
How does a noncompetitive inhibitor reduce an enzyme’s activity?
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Chemistry, 22.06.2019 16:30
For the reaction shown, calculate how many moles of no2 form when each of the following completely reacts. 2n2o5(g)→4no2(g)+o2(g) part a 1.0 mol n2o5 express your answer using two significant figures. nothing mol m o l request answer part b 5.4 mol n2o5 express your answer using two significant figures.
Answers: 2
Chemistry, 22.06.2019 17:00
Complete each row of the table below by filling in the missing prefix or missing exponent.
Answers: 1
Use the standard half-cell potentials listed below to calculate the standard cell potential for the...
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