160 g of SO3 are needed to make 400 g of 49% H2SO4.
<h3>How many grams of SO3 are required to prepare 400 g of 49% H2SO4?</h3>
The equation of the reaction for the formation of H2SO4 from SO3 is given below as follows:
1 mole of SO3 produces 1 mole of H2SO4
Molar mass of SO3 = 80 g/mol
Molar mass of H2SO4 = 98 g/mol
80 g of SO3 are required to produce 98 og 100%H2SO4
mass of SO3 required to produce 400 g of 100 %H2SO4 = 80/98 × 400 = 326.5 g of SO3
Mass of SO3 required to produce 49% of 400 g H2SO4 = 326.5 × 49% = 160 g
Therefore, 160 g of SO3 are needed to make 400 g of 49% H2SO4.
Learn more about mass and moles at: brainly.com/question/15374113
#SPJ1
Answer:
D
Explanation:
I think it's D Student C says soil is a vital for life on earth because it contains small mineral fragments, organic material, water, and air that can support the growth of vegetation.
The type of solvent that is needed to remove an oil stain would be an organic solvent. This is would dissolve the oil from the fabric to the solvent. Oil is nonpolar which would have the same polarity of an organic solvent. Hope this answers the question. Have a nice day.
<em>Kinds of monomers in nucleic acids:</em>
<em>There are 5 types of monomers in nucleic acids they are called nucleutides. </em><span><em>The five pieces are</em><em> uracil</em><em>, </em><em>cytosine</em><em>, </em><em>thymine</em><em>, </em><em>adenine</em><em>, and</em><em>guanine</em><em>.</em></span>
