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6.02 molecules of urea are present in100 ml of its solution . The concentration of urea solution is
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I am wondering what .02 molecules looks like, and how were they counted?
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the concentration of urea in a solution prepared by dissolving 16g of urea in 39 g of H2O is ________% by mass. The molar mass
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(g solute/g solution)*100 = [16/(16 + 39)]*100 = ?
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the concentration of urea (MW=60.0g/mol) in a solution prepared by dissolving 23g of urea in 64g of H2O is ____ molal
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molal means moles of solute per kg of solvent moles of urea ... (mass of urea) / (molar mass of
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Given the two substances Sodium Nitrate (NaNO3) and Urea ([NO2]2CO), why is it that urea has a lower boiling point? I thought
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To understand why urea has a lower boiling point than sodium nitrate, you need to consider the
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what is the effect of concentration of urea on urea based precipitation of copper nitrate?
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The effect of concentration of urea on urea-based precipitation of copper nitrate can be determined
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the concentration of urea (MW=60.0g/mol) in a soltuion prepared by dissolving 16g of urea in 39g of H2O is ____ molal
Top answer:
moles of urea:16(g)/60(g/mol)=0.267(mol) 39(g)*1(kg)/1000(g)=0.039kg m=0.267/0.039=6.846(mol/kg)
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1.00 tonne of ammonium from the harber process is reacted with carbon dioxide to prepare the fertiliser urea and 1.35 tonnes of
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74%
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The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol) in 39 g of
H2O is __________ M. The
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OH, ok thanks!
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The molarity of urea in a solution prepared by dissolving 16 g of urea (MW 60.0g/mol) in 39 g of H2O is ______M. The density of
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you have you add the total grams. so its 16g+39g=55g. so 55g/1.3g/ml=0.0421 L 0.267/.0421=6.3 M
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Find the mass of urea needed to prepare 50.1 of a solution in water in which the mole fraction of urea is 7.50×10−2.
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50.1 what?
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Find the mass of urea needed to prepare 51.7 of a solution in water in which the mole fraction of urea is 7.80×10−2.
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I worked this for you. As far as I can tell you never looked at the answer.
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