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Chapter 4: Problem 5

Write balanced equations based on the information given. (a) solid magnesium + oxygen gas \(\longrightarrow\) solid magnesium oxide (b) nitrogen monoxide gas + oxygen gas \(\longrightarrow\) nitrogen dioxide gas (c) gaseous ethane(C \(_{2} \mathrm{H}_{6}\) ) + oxygen gas \(\longrightarrow\) carbon dioxide gas + liquid water (d) aqueous silver sulfate \(+\) aqueous barium iodide \(\longrightarrow\) solid barium sulfate + solid silver iodide

Short Answer

Expert verified
The balanced equations are \n(a) 2Mg (s) + O2 (g) -> 2MgO (s) \n(b) 2NO (g) + O2 (g) -> 2NO2 (g) \n(c) C2H6 (g) + 7/2O2 (g) -> 2CO2 (g) + 3H2O (l) \n(d) Ag2SO4 (aq) + BaI2 (aq) -> BaSO4 (s) + 2AgI (s).

Step by step solution

01

Write and balance the equation for the reaction of solid magnesium and oxygen gas

We write the reactants and products as \( \text{Mg (s)} + \text{O} _2 \text{(g)} \rightarrow \text{MgO (s)} \). This equation is not balanced because there are two oxygen atoms on the left while there is one on the right. Balancing the equation gives \( 2 \text{Mg (s)} + \text{O} _2 \text{(g)} \rightarrow 2 \text{MgO (s)} \).
02

Write and balance the equation for the reaction of nitrogen monoxide gas and oxygen gas

We write the reactants and products as \( 2 \text{NO (g)} + \text{O} _2 \text{(g)} \rightarrow 2 \text{NO} _2 \text{(g)} \). This equation is balanced.
03

Write and balance the equation for the reaction of gaseous ethane and oxygen gas

We write the reactants and products as \( \text{C} _2 \text{H} _6 \text{(g)} + \text{O} _2 \text{(g)} \rightarrow \text{CO} _2 \text{(g)} + \text{H} _2 \text{O (l)} \). This equation is not balanced. Balancing the equation gives \( \text{C} _2 \text{H} _6 \text{(g)} + 7/2\text{O} _2 \text{(g)} \rightarrow 2\text{CO} _2 \text{(g)} + 3\text{H} _2 \text{O (l)} \). This equation is now balanced.
04

Write and balance the equation for the reaction of aqueous silver sulfate and aqueous barium iodide

We write the reactants and products as \( \text{Ag} _2 \text{SO}_4 \text{(aq)} + \text{BaI} _2 \text{(aq)} \rightarrow \text{BaSO}_4 \text{(s)} + 2 \text{AgI (s)} \). This equation is balanced.

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Most popular questions from this chapter

A reaction mixture contains \(1.0 \mathrm{mol} \mathrm{CaCN}_{2}\) (calcium cyanamide) and \(1.0 \mathrm{mol} \mathrm{H}_{2} \mathrm{O}\). The maximum number of moles of \(\mathrm{NH}_{3}\) produced is (a) \(3.0 ;\) (b) 2.0 (c) between 1.0 and 2.0; (d) less than 1.0. $$\mathrm{CaCN}_{2}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow \mathrm{CaCO}_{3}+2 \mathrm{NH}_{3}(\mathrm{g})$$

The minerals calcite, \(\mathrm{CaCO}_{3},\) magnesite, \(\mathrm{MgCO}_{3}\) and dolomite, \(\mathrm{CaCO}_{3} \cdot \mathrm{MgCO}_{3},\) decompose when strongly heated to form the corresponding metal oxide(s) and carbon dioxide gas. A 1.000 -g sample known to be one of the three minerals was strongly heated and \(0.477 \mathrm{g} \mathrm{CO}_{2}\) was obtained. Which of the three minerals was it?

The manufacture of ethyl alcohol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) yields diethyl ether, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{O}\) as a by-product. The complete combustion of a \(1.005 \mathrm{g}\) sample of the product of this process yields \(1.963 \mathrm{g} \mathrm{CO}_{2} .\) What must be the mass percents of \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\right),\) and of \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{O}\) in this sample?

When a solid mixture of \(\mathrm{MgCO}_{3}\) and \(\mathrm{CaCO}_{3}\) is heated strongly, carbon dioxide gas is given off and a solid mixture of \(\mathrm{Mg} \mathrm{O}\) and \(\mathrm{CaO}\) is obtained. If a \(24.00 \mathrm{g}\) sample of a mixture of \(\mathrm{MgCO}_{3}\) and \(\mathrm{CaCO}_{3}\) produces \(12.00 \mathrm{g} \mathrm{CO}_{2}\) then what is the percentage by mass of \(\mathrm{MgCO}_{3}\) in the original mixture?

Given two liters of \(0.496 \mathrm{M} \mathrm{KCl},\) describe how you would use this solution to prepare \(250.0 \mathrm{mL}\) of \(0.175 \mathrm{M} \mathrm{KCl} .\) Give sufficient details so that another student could follow your instructions.
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