If you want 44.8 Liters of NH3 to be produced from the reaction below, then how many grams of N2 gas should you start with? There is excess hydrogen (H2) gas provided for the reaction.
N2 + 3H2  2NH3
Density of NH3 gas at STP is --- 0.761 g / L
Molar mass of NH3 is --- 17.04 g / mol
Molar mass of N2 is --- 28.02 g / mol
3. List the conversion steps below as shown in class for credit:

4. Write ALL of the math steps in the factor-label method in the same way as your text with the
same amount of detail as the text does for credit. Circle your final answer with the proper sig
figs.

Calculate the molarity of each of the following solutions. part a) 0.12 mol of lino3 in 5.5 l of solution part b) 60.7 g c2h6o in 2.48 l of solution part c) 14.2 mg ki in 100 ml of solution

Answer asap need to be answered by wednesday morning explain how a buffer works, using an ethanoic acid / sodium ethanoate system including how the system resists changes in ph upon addition of a small amount of base and upon addition of a small amount of acid respectively. include the following calculations in your i. calculate the ph of a solution made by mixing 25cm3 0.1m ch3cooh and 40cm3 0.1m ch3coo-na+. [ka = 1.74 x 10-5 m] ii. calculate the ph following the addition of a 10cm3 portion of 0.08 m naoh to 500cm3 of this buffer solution. iii. calculate the ph following the addition of a 10cm3 portion of 0.08 m hcl to 200cm3 of the original buffer solution.

The molecular weight of carbon dioxide, co2, is 44.00 amu, and the molecular weight of nitrous dioxide, no2, is 46.01 amu, so no2 diffuses co2