Sodium azide, the explosive compound in automobile air bags, decomposes according to the equation 1. 2NAN3(s) → 2Na(s) + 3N2(g) What mass of sodium azide is required to provide the nitrogen to inflate a 25.0 L bag to a pressure of 1.30 atm at 25°C?

A gas is formed in the reaction shown below. The gas laws can help determine the volume of gas produced. Zn(s) + 2 HCl(aq) → ZnCl₂ + H₂(g) Assume that 131.0 grams of Zn was used in this reaction. To determine the number of moles of hydrogen gas formed, you need to know the number of moles of Zn reactant was used. How many moles of Zn were used?

please give a full explanation

9. How many liters of oxygen are required to react completely with 2.4 liters of hydrogen to form water? 2H 2H.O

Using the reaction below write out a complete setup for the following stoichiometry on a sheet of paper. Make sure to have complete conversion factors with units in the correct order of calculation and sig figs for final answer. Upload as a pdf file or write in text box. C4H8(g) + 6 O2(g) 4 CO2(g) + 4 H20(g) How many liters of carbon dioxide gas can be created if I start with 45.63 grams of oxygen gas?

use 17.89 mL (experimental volume) and 0.00074044 mol H2 (theoretical moles of hydrogen gas) to calculate the value of R. Include correct units

Hydrogen sulfide and oxygen react to form sulfur dioxide and water, like this: 2 H, S(9)+30,(g) → 2 SO,(g)+2H,0(g9) Use this chemical equation to answer the questions in the table below. Suppose 160. mmol of H,S and None. 240. mmol of O, are added to an Some, but less than 160. mmol. empty flask. How much H,S will be O 160. mmol. in the flask at equilibrium? More than 160. mmol. None. Suppose 125. mmol of SO, and 125. mmol of H,0 are added to an O Some, but less than 125. mmol. 125. mmol. empty flask. How much SO, will be in the flask at equilibrium? O More than 125. mmol.

Assuming all gases are the same temperature and pressure how many milliliters of hydrogen gas must react to give 41.0 mL of NH3? 3H2(g)+N2(g)-->2NH3(g) Express your answer with the appropriate units. VH2=

Consider the following chemical reactions: KClO3 (s) ----------> KCl(s) + O2(g)  NaNO3(s) ---------> NaNO2(s) + O2(g)  5.0000 g mixture of potassium chlorate and sodium nitrate is decomposed and the mass of residuals is 3.8600 g.  The oxygen gas is collected in 359. mL. container at 25 oC by water displacement technique.  Calculate the total pressure in mmHg. the vapor pressure of H2O at 25oC is 18.3 mmHg.       K = 39.10 g/mole,   Cl = 35.45 g/mole,  Na = 22.99 g/mole,  N = 14.00 g/mole  and O = 16.00 g/mole

Please don't provide handwriting solution