Answer:
I think the answers D. Hope this helps you.
Explanation:
This problem is simply converting the concentration from molality to molarity. Molality has units of mol solute/kg solvent, while molarity has units of mol solute/L solution.
2.24 mol H2SO4/kg H2O * (0.25806 kg H2SO4/mol H2SO4) = 0.578 kg H2SO4/kg H2O
That means the solution weighs a total of 1 kg + 0.578 kg = 1.578 kg. Then, convert it to liters using the density data:
1.578 kg * (1000g / 1kg) * (1 mL/1.135 g) = 1390 mL or 1.39 L.
Hence, the molarity is
2.24/1.39 = 1.61 M
Notice q=3/2, is half of the original q = 3(<span>1/2</span>)<span>t/28.8
your welcome
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Partial pressure (N2) = mole fraction * total pressure
{ 1 mole of any ideal gas occupy same volume of 1 mole of any other ideal gas under same condition of temperature and pressure so mole fraction in the sample is simply 78.08% = 0.7808 this is because equal volume of each gas has equal moles
partial pressure N2 = 0.7808 * 760 .0
partial pressure = 593.4 mmhg ( 1 torr = 1mmhg )
