Home
/
Chemistry
/
Using moles to balance equations 1. Use the following masses of reactants and products to write balanced symbol equations. a) 237.0 g of sodium thiosulfate (Na_(2)S_(2)O_(3)) reacts with 109.5 g of hydrochloric acid to produce g of sodium chloride,48.0 g of sulfur 96.0 g of sulfur dioxide and 27.0 g of water.

Question

Using moles to balance equations 1. Use the following masses of reactants and products to write balanced symbol equations. a) 237.0 g of sodium thiosulfate (Na_(2)S_(2)O_(3)) reacts with 109.5 g of hydrochloric acid to produce g of sodium chloride,48.0 g of sulfur 96.0 g of sulfur dioxide and 27.0 g of water.

Using moles to balance equations 1. Use the following masses of reactants and products to write balanced symbol equations. a) 237.0 g of sodium thiosulfate (Na_(2)S_(2)O_(3)) reacts with 109.5 g of hydrochloric acid to produce g of sodium chloride,48.0 g of sulfur 96.0 g of sulfur dioxide and 27.0 g of water.

expert verifiedVerification of experts

Answer

4.6242 Voting
avatar
SaffronVeteran · Tutor for 10 years

Answer

## Calculating Moles:<br />### Sodium Thiosulfate (\(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\)):<br />\[<br />\mathrm{Moles} = \dfrac{\mathrm{Mass}}{\mathrm{Molar \ Mass}} = \dfrac{237.0 \ \mathrm{g}}{158.11 \ \mathrm{g/mol}} = 1.5 \ \mathrm{mol}<br />\]<br />### Hydrochloric Acid (\(\mathrm{HCl} \)):<br />\[<br />\mathrm{Moles} = \dfrac{\mathrm{Mass}}{\mathrm{Molar \ Mass}} = \dfrac{109.5 \ \mathrm{g}}{36.461 \ \mathrm{g/mol}} = 3.0 \ \mathrm{mol}<br />\]<br />### Sodium Chloride (\( \mathrm{NaCl} \)):<br />\[<br />\mathrm{Moles} = \dfrac{\mathrm{Mass}}{\mathrm{Molar \ Mass}} = \dfrac{175.5 \ \mathrm{g}}{58.44 \ \mathrm{g/mol}} = 3.0 \ \mathrm{mol}<br />\]<br />### Sulfur (\( \mathrm{S} \)):<br />\[<br />\mathrm{moles}=\dfrac{\mathrm{mass}}{\mathrm{molar \ mass}}=\dfrac{48.0 \ \mathrm{g}}{32.065 \ \mathrm{g/mol}} =1.5 \ \mathrm{mol}<br />\]<br />### Sulfur Dioxide (\( \mathrm{SO}_{2} \)):<br />\[<br />\mathrm{moles}=\dfrac{\mathrm{mass}}{\mathrm{molar \ mass}}=\dfrac{96.0 \ \mathrm{g}}{64.06 \ \mathrm{g/mol}} =1.5 \ \mathrm{mol}<br />\]<br />### Water (\( \mathrm{H}_{2}\mathrm{O} \)): <br />\[<br />\mathrm{moles}=\dfrac{\mathrm{mass}}{\mathrm{molar \ mass}}=\dfrac{27.0 \ \mathrm{g}}{18.015 \ \mathrm{g/mol}} =1.5 \ \mathrm{mol}<br />\]<br /><br />## Balancing the equation: <br />The balanced chemical equation is:<br />### \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3} + 2\mathrm{HCl} \rightarrow 2\mathrm{NaCl} + \mathrm{S} + \mathrm{SO}_{2} + \mathrm{H}_{2}\mathrm{O}\)<br /><br />## Validating the balance:<br />From the chemical equation, we can always see that reactants and products from both sides are correctly balanced in mole ratios thus the equation must be a correct.<br />Chemical reaction equation double checked is once again:<br />### \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3} + 2\mathrm{HCl} \rightarrow 2\mathrm{NaCl} + \mathrm{S} + \mathrm{SO}_{2} + \mathrm{H}_{2}\mathrm{O}\)

Explain

## Step1: Calculate the moles of each substance:<br />Moles are the mass of a substance divided by its molar mass. Recall that the molar mass is the sum of the masses of all the elements in the compound.<br />-Sodium thiosulfate (\(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\))<br />-Hydrochloric acid (\(\mathrm{HCl}\))<br />-Sodium chloride (\(\mathrm{NaCl}\))<br />-Sulfur (\(\mathrm{S}\))<br />-Sulfur dioxide (\(\mathrm{SO}_{2}\))<br />-Water (\(\mathrm{H}_{2} \mathrm{O}\))<br /><br />## Step2: Balance the equation using the moles found:<br />Next, determine a balanced chemical equation that accounts for all reactants and produces all products in the measured amounts. <br /><br />## Step3: Validate the equation balanced is correct:<br />The last step would be to check if our balance equation is correct, by ensuring that both the moles of reactants and products are balanced correctly.
Click to rate:

Hot Questions

More x