Consider the reaction:
2Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g)
What minimum volume of 4.0 M H2SO4 is required to produce 15.0 L of H2 at STP?
Step 1</p>write a balanced chemical equation for this single replacement reactionuse the molar volume of a gas at STP to find the number of moles of hydrogen gas present in that volumeuse the mole ratio that exists between sulfuric acid and hydrogen gas to find the number of moles of the former needed to produce that many moles of the latteruse the sulfuric acid solution's molarity to find the volume that would contain that many moles of sulfuric acid.
So, the balanced chemical equation for this reaction looks like this
As you know, STP conditions are characterized by a pressure of 100.0 kPa and a temperature of 0∘C. Under these conditions, one mole of any ideal gas occupies exactly 22.71 L - this is the molar volume of a gas at STP.
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
The full step-by-step solution to problem: 115P from chapter: 13 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The answer to “Consider the reaction:2Al(s) + 3 H2SO4(aq) ? Al2(SO4)3(aq) + 3 H2(g)What minimum volume of 4.0 M H2SO4 is required to produce 15.0 L of H2 at STP?” is broken down into a number of easy to follow steps, and 27 words. Since the solution to 115P from 13 chapter was answered, more than 341 students have viewed the full step-by-step answer. This full solution covers the following key subjects: consider, minimum, produce, reaction, required. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295.