If you feed 10.0g of N2 gas and 10.0g of H2 into a reactor to make ammonia (NH3):a. What is the limiting reactant and the excess reactant?b. What is the maximum number of grams of NH3 that can be produced if 100% of the limiting reactant was reacted?c. If 5.0g of the limiting reactant actually react, what is the fractional conversion of the limiting reactant, and why would you want to make ammonia, what is it useful for?

Predict the product when the two substances mix. If the reaction occurs, write the balanced chemical equation. If the reaction does not happen, write "NA" A solution of nickel(III) nitrate is mixed with a solution of sodium hydroxide.

Please explain the atomic balances!

Now, let's use what we know about chemistry to infer how much acetic acid was in our sample. Let's look closely at the equation for the reaction we performed. HC2H3O2(aq) + NaHCO3(s) → NaC2H3O2(aq) + H2O(1) + CO2(g) Based on this balanced chemical reaction, we can see that for every one mole of CO2 that was produced one mole of acetic acid was consumed. Based on this, calculate the moles of acetic acid and grams of acetic acid that must have reacted in each sample. Sample Data for Vinegar Lab moles CO2 Produced Moles HC2H3O2 Consumed g HC2H302 Consumed by by Reaction by Reaction Reaction -2 g NaHCO3 0.0329 -4 g NaHCO3 0.0464 -6 g NaHCO3 0.0523 -8 g NaHCOз 0.0477 -10 g NaHCO3 0.0489