When a beverage is carbonated, the carbon dioxide reacts...

When a beverage is carbonated, the carbon dioxide reacts with water to produce carbonic acid, which gives soft drinks a bitterness that is balanced with a large amount of sugar. Over time, carbonic acid converts back into carbon dioxide and water: $$ \mathrm{H}_2 \mathrm{CO}_3(\mathrm{aq}) \rightarrow \mathrm{H}_2 \mathrm{O}(f)+\mathrm{CO}_2(g) $$ In this reaction, what volume of $\mathrm{CO}_2$ can be produced from 2.0 grams of $\mathrm{H}_2 \mathrm{CO}_3$ at standard temperature and pressure? (Standard temperature and pressure is 273 K and 1.0 atmosphere.)

When a beverage is carbonated, the carbon dioxide reacts with water to produce carbonic acid, which gives soft drinks a bitterness that is balanced with a large amount of sugar. Over time, carbonic acid converts back into carbon dioxide and water:

$$
\mathrm{H}_2 \mathrm{CO}_3(\mathrm{aq}) \rightarrow \mathrm{H}_2 \mathrm{O}(f)+\mathrm{CO}_2(g)
$$

In this reaction, what volume of $\mathrm{CO}_2$ can be produced from 2.0 grams of $\mathrm{H}_2 \mathrm{CO}_3$ at standard temperature and pressure? (Standard temperature and pressure is 273 K and 1.0 atmosphere.)

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Key Concepts

Ideal Gas Law

The Ideal Gas Law, expressed as PV = nRT, establishes a relationship between the pressure, volume, temperature, and number of moles of a gas. Under STP conditions, this relationship allows one to easily calculate the volume of gas produced or consumed in a reaction by using the standard molar volume.

Standard Temperature and Pressure (STP)

Standard Temperature and Pressure (STP) refers to a set of conditions used as a reference in calculations involving gases, typically 273 K and 1 atmosphere. At STP, one mole of an ideal gas occupies 22.4 liters, which simplifies the conversion between moles of a gas and its volume.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to determine the quantitative relationships between reactants and products. It enables one to calculate the moles or mass of a product formed from a given amount of reactant, as every substance in the equation contributes in exact proportions.

Molar Mass

Molar mass is the mass of one mole of a substance. It is used to convert between the mass of a substance and the number of moles, which is essential in stoichiometric calculations and helps in relating the given mass of a compound to the number of moles available for the reaction.

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