2. sulfur dioxide gas (so2) reacts with excess oxygen gas (o2) and excess liquid water (h2o) to form liquid sulfuric acid (h2so4) in the unbalanced equation below: so2 + o2 + h2o  h2so4 in the laboratory, a chemist carries out this reaction at stp with 67.2 l of sulfur dioxide (so2). how many liters of h2so4 did the chemist produce? 1 mole of any gas = 22.4 l of that same gas at stp • part a: write a balanced equation for the reaction. • part b: calculate the number of liters of h2so4 produced.

Part A:

Part B: Volume of =0.16L

Explanation:

According to law of conservation of mass, the atoms on product side must be equal to the atoms on reactant side so that the mass remains conserved.

Part A: The balanced chemical reaction is:

Part B: 1 mole of occupies 22.4 L at STP

2 moles of will occupy and produce 2 moles of

mass of 2 moles of

Thus 44.8 L of   will produce 196 g of          

67.2 L of   will produce of

mass of  = 294 g

density of

Thus Volume of

no statements shown

the atomic number of carbon is six, which means that a carbon atom has six protons. carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. which of these statements are true about carbon and its isotopes? select all that appl