A 2.14 L sample of hydrogen chloride gas at 2.61 atm and 28 degree C is complete

Question

A 2.14 L sample of hydrogen chloride gas at 2.61 atm and 28 degree C is completely dissolved in 668 mL o1 water to 1orm hydrochloric acid solution. Assume no volume change. (Calculate the moles then of the acid solution. Calculate the volume of oxygen at 80 degree C and 823 mm Hg required for the complete combustion of 7.64 L of acetylene (C_2H_2) at ST P. Write and balance the equation first. Forty miles above the earth's surface the temperature is -23degree C, and the pressure is only 0.20 mm Hg. What is the density of air (molar mass = 29.0 g/mol) at this altitude?

Explanation / Answer

A 2.14 L sample of HCl gas @ 2.61 atm and 28 degrees Celsius is completely dissolved by 668 ml of water to form hydrochloric acid. Calculate the molarity of the acid solution, assuming no change in volume.

2.14 L HCl,

2.61 atm,

(28 + 273)k

From above information, we can calc the mole of HCl by using the ideal gas law:

PV = nRT

2.61atm x 2.14 L = n x 0.0821 Latm/kmol x (28+ 273)k

n = 0.226 mol HCl

volume of water = volume of soln = 0.668 L solution

Recap: we got 0.226 mol HCl and we know 0.668 L Solution

Molarity of solution = 0.226 mol HCl / 0.668 L solution = 0.338 mol/L or 0.338 M --------answer

==========================================================================

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.