What is the limiting reagent when 49.84 g of nitrogen react with 10.7 g of hydrogen according to this balanced equation? N₂(g) + 3H₂(g) → 2NH₃(g)

I'm a bit stuck, I'm not sure if I'm supposed to convert grams to moles then compare ratios. Can someone please explain how to do this?

The equilibrium constant kc for the reaction 2 nocl(g) → 2 no(g) + cl2(g) is 0.453 at a certain temperature. a mixture of nocl, no, and cl2 with concentrations 1.30, 1.20, and 0.600 m, respectively, was introduced into a container at this temperature. which of the following is true? 1. no apparent reaction takes place. 2. [cl2] = 0.30 m at equilibrium. 3. nocl(g) is produced until equilibrium is reached. 4. [nocl] = [no] = [cl2] at equilibrium. 5. cl2(g) is produced until equilibrium is