What happens when KCl, K₂Cr₂O₇, and concentrated H₂SO₄ reacts? What happens when $\ce{KCl}$, $\ce{K2Cr2O7}$, and concentrated $\ce{H2SO4}$ reacts?

I have no idea how to approach these questions. I'd love if anybody can help me see the logic behind this.
Have a look at the properties of the compounds involved.

Dichromate ($\ce{Cr(VI), Cr2O7^{2-}}$) is a strong oxidant and is reduced to $\ce{Cr(III)}$ if it finds a suitable partner (which then is oxidized).

Here, a potential partner in a redox reaction is chloride: $\ce{2 Cl- + 2 e^{-} -&gt; Cl2}$.