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Alevel Chemistry - Moles

A chemical company receives an order to supply 1.96x10^10dm3 of ammonia at room temperature and pressure. The Haber process produces a 95.0% yield. Calculate the mass of hydrogen, in tonnes, required to produce the ammonia. Give your answer to 3 significant figures.

Hi, I'm stuck on this question, I honestly have no clue how to answer it, if someone could please help me, thank you!
1. Moles of ammonia needed using molar volume of gas. 24dm3
2. Use molar ratio of ammonia to hydrogen to give moles of hydrogen 2:3.
3. Convert from 95% to 100%
4. Convert to mass of hydrogen using Mr.
Original post by Old man1234
1. Moles of ammonia needed using molar volume of gas. 24dm3
2. Use molar ratio of ammonia to hydrogen to give moles of hydrogen 2:3.
3. Convert from 95% to 100%
4. Convert to mass of hydrogen using Mr.

Hi, thank you, what do you mean by convert 95% to 100% ? What equation is this, or how are we doing this?
(edited 1 year ago)
÷95 x 100

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