Calculate the mass of the solution used if a student added 35.569 grams of ammon

Question

Calculate the mass of the solution used if a student added 35.569 grams of ammonium sulfate to enough water to give 80.0 mL of solution. The density of the solution was 1.00 g;mL For the neutralization reaction (i.c- Part I of this experiment), calculate the number of moles of the limiting reactant when 25.0 ml. of 2.085 M H_2SO_4 (aq) is mixed with 50.0 mL of 1.873 M NH_3 using the molar ratio of the reaction. Show your work with the correct units and number of significant figures If a student calculated the number moles of limiting reactant for the above neutralization reaction (See Question 4 above) to be 0.00568 moles of ammonium sulfate and the heat (/>., Q) of the reaction to be 5680 J. calculate the enthalpy change of this reaction. Show your work with the correct units and number of significant figures.

Explanation / Answer

mass of solution

m = 35.569 g of (NH4)2(SO4)

V = 80 ml solution

D = 1 g/ml

Find mass of oslution

V = 80 ml * 1 g/ml = 80g

MT =Mw + Ms

80g = MW + 35.569

Mw = 80-35.569 = 44.431 g

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