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This means that one liter of the solution of sulfuric acid contains 0.2 gram-equivalent mass of sulfuric acid. For this acid, the equivalent mass is one half the molar mass, since each molecule of H2SO4 supplies two hydrogen atoms to neutralize alkaline materials.

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How many moles of excess sulfuric acid are left over after the complete reaction of 300.0 g of ammonia with 36.0 moles of sulfuric acid producing ammonium sulfate?

The equation for the reaction is: H{2}SO{4} + 2NH{3} → (NH{4}){2}SO{4} [Numbers in braces are supposed to be subscripts, but I can't do them here.] This says that 1 mole of sulphuric acid reacts with 2 moles of nitrogen to create 1 mole of ammonium sulphate. 1 mole of a substance weighs the same as its atomic weight in grams. 1 mole of NH{3} weighs 14 + 3 × 1 = 17 g Thus 2 × 17 g = 34 g of ammonia react with 1 mole of sulphuric acid. To react with 300 g of ammonia requires 300 g ÷ 34 g/mol ≈ 8.8 moles of sulphuric acid Therefore there will be 36.0 - 8.8 = 27.2 moles of sulphuric acid left.


300.0g of ammonia react with 36.0 moles of sulfuric acid to produce ammonium sulfate how many moles of excess sulfuric acid are left over after the reaction is complete?

The equation for the reaction is: H{2}SO{4} + 2NH{3} → (NH{4}){2}SO{4} [Numbers in braces are supposed to be subscripts, but I can't do them here.] This says that 1 mole of sulphuric acid reacts with 2 moles of nitrogen to create 1 mole of ammonium sulphate. 1 mole of a substance weighs the same as its atomic weight in grams. 1 mole of NH{3} weighs 14 + 3 × 1 = 17 g Thus 2 × 17 g = 34 g of ammonia react with 1 mole of sulphuric acid. To react with 500 g of ammonia requires 500 g ÷ 34 g/mol ≈ 14.7 moles of sulphuric acid Therefore there will be 51.0 - 14.7 = 36.3 moles of sulphuric acid left.


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Eating soda is not a common phrase. Soda is a carbonated beverage meant to be drunk, not eaten. If someone says they are "eating soda," it could be a misunderstanding or meant in a figurative or humorous sense.


What is balance equation borax with sulfuric acid?

Na2B4O7 + H2SO4 = H3BO3 + Na2SO4This unbalanced equation is given in my chemistry book (Zumdahl World of Chemistry) and we are supposed to balance it in order to find the mole ratios.Every resource I have used says this equation is impossible to balance.The answers in Zumdahl imply that there is a ratio of 1 mol borax to 4 moles boric acid, and 1 mol borax to 1 mol sodium sulfate, but no coefficients are ever given.


Is it true that sulfuric acid is dangerous to living organisms?

Sulfuric acid is outrightly nasty when it comes to your health.Contact with skinSulfuric acid corrodes skin and bone by chemical combination. It also has a nasty trait of stripping water from other compounds like sugars and starches to comnine with its own molecules. This doesn't sound bad, but it will reduce organic material to just carbon in short order, this is a standard "impressive" demonstration of the dangers of sulfuric acid.It will also eat away your clothes while chewing on the skin below.Contact with eyesAll the problems with skin exposure apply to eyes. Eyes however are not as forgiving for the resulting scar tissue. Always wear goggles when working with sulfuric acid.VapoursSulfuric acid at high concentrations fumes, it also can become an aerosol when poured or stirred. The gases or minute droplets will combine with wet areas of your body (eyes, the inside of your nose and lungs, sweaty clothes) to mkae a high strength liquid acid. All problems noted earlier apply, except you can corrode from the inside out.Addition to waterWhen sulfuric acid is exposed to water it grabs onto the water molecules and releases heat. If the heat is not dissipated the water can turn to stream suddenly (explosively) covering everyone nearby with drops of concentrated acid. This is worst when water is poured into the acid not the other way around.An old lab poem and warning says:"May his rest be long and placidWho adds water to the acid!"

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How many moles of excess sulfuric acid are left over after the complete reaction of 300.0 g of ammonia with 36.0 moles of sulfuric acid producing ammonium sulfate?

The equation for the reaction is: H{2}SO{4} + 2NH{3} → (NH{4}){2}SO{4} [Numbers in braces are supposed to be subscripts, but I can't do them here.] This says that 1 mole of sulphuric acid reacts with 2 moles of nitrogen to create 1 mole of ammonium sulphate. 1 mole of a substance weighs the same as its atomic weight in grams. 1 mole of NH{3} weighs 14 + 3 × 1 = 17 g Thus 2 × 17 g = 34 g of ammonia react with 1 mole of sulphuric acid. To react with 300 g of ammonia requires 300 g ÷ 34 g/mol ≈ 8.8 moles of sulphuric acid Therefore there will be 36.0 - 8.8 = 27.2 moles of sulphuric acid left.


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300.0g of ammonia react with 36.0 moles of sulfuric acid to produce ammonium sulfate how many moles of excess sulfuric acid are left over after the reaction is complete?

The equation for the reaction is: H{2}SO{4} + 2NH{3} → (NH{4}){2}SO{4} [Numbers in braces are supposed to be subscripts, but I can't do them here.] This says that 1 mole of sulphuric acid reacts with 2 moles of nitrogen to create 1 mole of ammonium sulphate. 1 mole of a substance weighs the same as its atomic weight in grams. 1 mole of NH{3} weighs 14 + 3 × 1 = 17 g Thus 2 × 17 g = 34 g of ammonia react with 1 mole of sulphuric acid. To react with 500 g of ammonia requires 500 g ÷ 34 g/mol ≈ 14.7 moles of sulphuric acid Therefore there will be 51.0 - 14.7 = 36.3 moles of sulphuric acid left.


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