A sample of \(\mathrm{N}_{2} \mathrm{O}_{3}\) contains 1 moles of nitrogen. Use the following atomic masses: \(\mathrm{N}=14, \mathrm{O}=16\).
$$ \begin{array}{|l|l|l|} \hline \text { The number of moles of } \mathrm{N}_{2} \mathrm{O}_{3} \text { present }= & \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{3} \\ \hline \text { The mass of the sample }= & \mathrm{g} \mathrm{N}_{2} \mathrm{O}_{3} \\ \hline \text { The number of moles of oxygen in the sample }= & & \mathrm{mol} \mathrm{O} \\ \hline \text { The mass of oxygen in the sample }= & \mathrm{g} \mathrm{O} \\ \hline \end{array} $$
Balance the following equation using the smallest integer coefficients.
a)
$$ \mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{KOH} \rightarrow \quad \mathrm{K}_{3} \mathrm{PO}_{4}+\mathrm{H}_{2} \mathrm{O} $$
b)
$$ \mathrm{N}_{2} \mathrm{O}_{5}+\quad \mathrm{H}_{2} \mathrm{O} \rightarrow \quad \mathrm{HNO}_{3} $$
c)
$$ \begin{array}{llll} \mathrm{Al}+ & \mathrm{H}_{2} \mathrm{O} \rightarrow & \mathrm{Al}(\mathrm{OH})_{3}+ & \mathrm{H}_{2} \end{array} $$
Homework Answers
Aquatic Chemistry
1. A river contains a relatively low concentration of dissolved salts, so that the ideal assumption applies. The river has the same \(\mathrm{pH}(8.1)\) and total carbonate concentration \(\left(2 \times 10^{-3} \mathrm{M}\right)\) as bulk seawater. The work of Garrels and Thompson (1962) indicates that the total ion activity coefficients of \(\mathrm{H}^{+}, \mathrm{OH}^{-}\), and various carbonate-containing species in seawater are as follows:$$ \begin{array}{|c|c|} \hline & \begin{array}{c} \text { activity } \\ \text { coefficient } \\ \text { lon } \end{array} &...
Which of the following reactions are redox reactions?
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A sample of N2O3 contains 2.26 moles of nitrogen. Use the following atomic masses: N =14,...
A sample of N2O3 contains 2.26 moles of nitrogen. Use the following atomic masses: N =14, O=16. The number of moles of N2O3 present = mol N2O3 The mass of the sample = g N2O3 The number of moles of oxygen in the sample = mol O The mass of oxygen in the sample = g O
Gases are different from solids and liquids
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2. a) Balance the equation below and use it to calculate the moles of Fe formed from 0.50 moles of Fe,O3: Fe2O3(...
2. a) Balance the equation below and use it to calculate the moles of Fe formed from \(0.50\) moles of \(\mathrm{Fe}_{2} \mathrm{O}_{3}:\)$$ \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+\mathrm{CO}(\mathrm{g}) \stackrel{\Delta}{\rightarrow} \mathrm{Fe}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g}) $$3. Balance the equation below then calculate the mass of \(\mathrm{ZnCl}_{2}\) by obtained by reacting \(10.0 \mathrm{~g}\) of zinc metal with an excess (more than is required) of hydrochloric acid$$ \mathrm{Zn}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{ZnCl}_{2}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g}) $$
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Which of the following reactions are redox reactions?Check all that apply.$$ \begin{array}{l} \mathrm{Mg}(\mathrm{s})+\mathrm{Br}_{2}(\mathrm{l}) \rightarrow \mathrm{MgBr}_{2}(\mathrm{~s}) \\ \mathrm{Al}(\mathrm{s})+3 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{Ag}(\mathrm{s}) \\ 4 \mathrm{~K}(\mathrm{~s})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{~K}_{2} \mathrm{O}(\mathrm{s}) \\ \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \end{array} $$
Gases are different from solids and liquids. In a sample of gas, the molecules are far apart. The gas molecules also move around and collide with each other as well as with the walls of the container. These collisions generate pressure. The pressure of a gas can be measured in different units. One convenient unit of measure is called the atmosphere (atm) because it is based on atmospheric pressure. At sea level, the average pressure is 1 atm. As you...
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Given the standard enthalpy changes for the following two reactions:(1) \(2 \mathrm{C}(\mathrm{s})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=\mathbf{5 2 . 3} \mathrm{kJ}\)(2) \(2 \mathbf{C}(\mathbf{s})+\mathbf{3 H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{8 4 . 7} \mathrm{kJ}\)what is the standard enthalpy change for the reaction:(3) \(\mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{4}}(\mathbf{g})+\mathbf{H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=?\)Given the standard enthalpy changes for the following two reactions:(1) \(\mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=66.4 \mathrm{~kJ}\)(2) \(2 \mathbf{N}_{2} \mathrm{O}(\mathrm{g}) \longrightarrow \mathbf{2 N}_{2}(\mathbf{g})+\mathbf{O}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{1 6...
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