2.0 L of gas A at 1.0 atm and 1.0 L of gas B at 1.0 atm are combined in a 3.0 L flask. The flask is sealed and over time they react completely to give gas C according to the following chemical equation: 2A(g) + B(g) →C(g) Assuming the temperature stays constant, what will be the pressure after the reaction goes to completion?

0.993 atm

Explanation:

This can be calculated using Dalton's law of partial pressure which states that if two or more gases are mixed together, the total pressure exerted by the mixture of the gases is eqaul to the sum of the pressure which individual gas woud exert if it occupied the volume of of the mixture alone.

Therefore P (total) = P (gas A) + P (gas B)

Since pressure of gas A = 1.0 atm  

          pressure of gas B = 1.0 atm

          gas constant R = 0.08206 atm L mol-1 K-1

          standard temperature = 273K

Note that atm is a unit for pressure

Number of mole of gas A, n=PV/RT

= 1 x 2 / 0.08206 x 273

= 0.088306 mole

Number of mole of gas B

= 1 x 1 / 0.08206 x 273

= 0.044644 mole

Total pressure can be gotten using P(total) = (n(total)RT)/V(total)

= [(0.044644 + 0.088306) x 0.08206 x 273] / 3

= 0.993 atm

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.