Question

QUESTION 1 What will be the pressure of 52.5 grams of oxygen gas in a glass container with a volume of 6 L at 15.4 °C? QUESTION 2 At what temperature in °C does 37.34 g of oxygen gas occupy 18.17 L at 622 mm Hg? QUESTION 3 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g)O2(g)-»2 H20(g) How many grams of water could be produced by the reaction of 5.1 liters of hydrogen with 4.11 liters of oxygen at STP? (Hint: check for limiting reagent) QUESTION 4 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s)2 Na(s)3 N2(g) Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 25.4 L of N2(g) at 48.9 °C and 1.00 atm?

Answer 1

p= nRT 52.29 2.0821 E XC" = 32 mal X 0.0821 tatm x (15.4 +273) tholik G+ preasure (p = 6:43 atm Q-2 Temp = pul = Se ayn x 18.174 37.34 3 ml x0.082 K. afm moik = 15522 K -273 Temp =-117 7 Ĉ =-117.70 mole = 22.4 Litres 51 Kx mol No of moles of H2= 22:44 1 = 00927 moles of H2 No. of moles of a=4011 fx mol = 0.183 moles 7 22:44 2 H2(g) + Org > 20 () amoles Hy react with one mole of give amol to Here Oz (6.183 moles) is limiting reactant cambleatly Gonson

Imole og give a mole H2O 0,183 mole og give how many moles of H2O = 0.183x9 moles of H2O = 0.366 moles of tzo mass (grame)of tzo = 0.366px 189lote = 6.589 [ 6.58 grams of the na pu RT 100 Am x 25oux 0.0821 X-gotin x(48.9+373) K 1 moliy = 0.961 mole of N2

a an'z - ana + 3 12) from ean amole NaNg give 3 mole N2 how many mole Nalla sive oogol mdeny = 0.964 X2 mole Mans = 0.64 mole Nana weight of Nana = 0064 mole x 65% ..=41.64 gram Manz