Consider the generic reaction: . If a flask initially contains 1.0 atm of A and 1.0 atm of B, what will be the pressure in the flask if the reaction proceeds to completion? (Assume constant volume and temperature.)
a) 1.0 atm
b) 1.5 atm
c) 2.0 atm
d) 3.0 atm
Solution 14SAQ Step 1: Establish relationship of Pressure and number of moles. Using the ideal gas equation PV = nRT, it can be observed that pressure is directly proportional to the number of moles of gas. Since the two gases both have the same pressure, and assuming constant volume and temperature, this means both gases have the same number of moles. Step 2: Determine limiting reactant. Two moles of A is required to react per mole of B. Since the two gases have the same initial number of moles, this means A will be the limiting reactant and B will be the excess reactant. Step 3: Compute for pressure of C produced.
Textbook: Chemistry: A Molecular Approach
Author: Nivaldo J. Tro
The full step-by-step solution to problem: 14SAQ from chapter: 5 was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. This full solution covers the following key subjects: atm, reaction, flask, Generic, constant. This expansive textbook survival guide covers 82 chapters, and 9454 solutions. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. The answer to “Consider the generic reaction: . If a flask initially contains 1.0 atm of A and 1.0 atm of B, what will be the pressure in the flask if the reaction proceeds to completion? (Assume constant volume and temperature.)a) 1.0 atmb) 1.5 atmc) 2.0 atmd) 3.0 atm” is broken down into a number of easy to follow steps, and 46 words. Since the solution to 14SAQ from 5 chapter was answered, more than 473 students have viewed the full step-by-step answer. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247.