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apricotdeer375Lv1

28 Sep 2019

For the following reaction between Mohr\'s salt (iron asFeSO4(NH4)2SO4

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Tod ThielLv2

28 Sep 2019

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The salt ammonium sulfate dissolves in water according to the reaction:

(NH₄)₂SO₄(s) ------>2NH₄⁺(aq) + SO₄^2-(aq)

(a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data:

ΔH°f(NH₄)₂SO₄(s) = -1180.9 kJ mol^-1
ΔH°f NH₄⁺(aq) = -132.5 kJ mol^-1
ΔH°f SO₄^2-(aq) = -909.3 kJ mol^-1

^{(b) Calculate the temperature reached by the solution formed when 147 g of (NH₄)₂SO₄ is dissolved in 0.167L of water at 23.1 °C. Approximate the heat capacity of the solution by the heat capacity of 167 g of pure water (specific heat capacity = 4.18 J g-1 °C-1), ignoring the mass of the salt.}

^{c) Heats of reaction find practical application in hot packs or cold packs. Would this dissolution reaction be appropriate for the preparation of a hot pack or a cold pack?}

blackprairie-dog787

If 45.0 mL of 0.250 M PbCl4 solution reacts with 20.0 mL of (NH4)2SO4 to reach the equivalence point, what is the molarity of the (NH4)2SO4? PbCl4(aq) + 2(NH4)2SO4(aq) â Pb(SO4)2(s) + 4NH4Cl(aq)

Compute the mass of solute and water needed to prepare the following solutions:1. 150 g of 1.00 m (NH4)2SO4: (a) from pure solid (NH4)2SO4 (b) from solid (NH4)2SO4 with a purity of 87.2 wt-%2. 1.50 L of a 20 wt-% Pb(NO3)2 solution whose density is 1.20 g/mLThis is the work I've done so far (please check):1. a) Molality = (moles of solute) / (kilograms of solvent) moles of (NH4)2SO4 = 150 g (NH4)2SO4

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For the following reaction between Mohr\'s salt (iron asFeSO4(NH4)2SO4

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