Chemistry! Gaseous state help!?

Ammonia and hydrogen chloride react with each other to solid ammonium chloride:

NH₃(g) + HCl(g) → NH₄Cl(s)

Initially the were

n₀_NH₃ = 5.00 g / 17.031 g∙mol⁻¹ = 0.29358 mol

and

n₀_HCl = 5.00 g / 36.46 g∙mol⁻¹ = 0.13714 mol

in the two flask

You need on e mole of each reactant to form one mole of ammonium chloride. That means you have an excess of ammonia. Therefore all HCl will consumed an

n_NH₃ = 0.29358 mol - 0.13714 mol = 0.15644 mol

of gaseous ammonia are left over after reaction is complete.

The remaining ammonia occupies the total free space in the two flasks. Since the solid is much denser, you can ignore the tiny volume occupied by it, and the take the gaseous volume to be identical to the initial gas volume in the two flasks, which is

V = 2 ∙ 2 dm³ = 4 dm³ = 4.0×10⁻³ m³

Assuming ideal gas behavior you can compute the final pressure form ideal gas law:

P = n∙R∙T/V

= 0.15644 mol ∙ 8.3145 Pa∙m³∙K⁻¹∙mol⁻¹ ∙ 298 K / 4.0×10⁻³ m³

= 96904 Pa

= 0.956 atm

the entire mass of CO2 is interior the 500ml can is two.0g Saturated CO2 answer is a million.5g/dm^3 (that's the comparable as a million.5g per liter) So, after that's flat, there will be 0.500L x a million.5g/L = 0.75g last interior the cola. for this reason the burden misplaced while it is going flat would be: 2.0 - 0.75g = a million.25g To get quantity of this quantity of CO2 at STP, first be sure moles of CO2 from grams: a million.25g/(12.01 + (2 x sixteen.00)) = 0.0284 mole they do no longer specially state to calculate the quantity decrease than STP situations, yet that's what i visit apply, you could plug different values into the equation if needed. Now use the perfect gasoline equation employing STP situations: PV=nRT remedy for V: V = nRT/P V = 0.0284 x 0.08206Latm/molK x 273K/a million atm = 0.636L