The ionic equation for the reaction of aqueous potassium bromide with chlorine gas is shown. 2Br^ - +Cl 2 Br 2 +2Cl^ - Which statement is correct? A B Bromide ions are oxidised by losing electrons. Bromide ions are oxidised by gaining electrons. C Chlorine is oxidised by gaining electrons. D Chlorine is oxidised by losing electrons.

The correct statement : Bromide ions are oxidised by losing electrons

Redox=The reaction of addition/reduction of oxidation number

Oxidation is an increase in oxidation number, while reduction is a decrease in oxidation number.

In the redox reaction, it is also known

Reducing agents are substances that experience oxidation

The oxidizer is a substance that is reduced

Reaction

2Br⁻ + Cl₂⇒ Br₂ + 2Cl⁻

Oxidation : Br⁻ to Br₂ (-1 to 0)⇒oxidized

Reduction : Cl₂ to Cl⁻(0 to -1)⇒reduced

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer

is there any options? maybe im just not seeing them but i need the options to

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