Propane burns according to the following equation: C3 H8+5 O2 ⟶3 CO2+4 H2 O (a) How many grams o

Name: Problem 115, Chapter 3: Chemistry: The Molecular Nature of Matter
Uploaded: 2021-06-10T23:23:53-08:00
Duration: 3 min 29 s
Channel: Dr. Satish Ingale
Description: Propane burns according to the following equation: C3 H8+5 O2 ⟶3 CO2+4 H2 O (a) How many grams of O2 are needed to react fully with 3.45 mol of propane? (b) How many grams of CO2 can form from 0.177 mol of propane? (c) How many grams of water are produced by the combustion of 4.86 mol of propane?

step 1 Hi everyone so in this question they ask that is propane but second following equation c3 h8 plu

Question

Propane burns according to the following equation: $$ \mathrm{C}_{3} \mathrm{H}_{8}+5 \mathrm{O}_{2} \longrightarrow 3 \mathrm{CO}_{2}+4 \mathrm{H}_{2} \mathrm{O} $$ (a) How many grams of $\mathrm{O}_{2}$ are needed to react fully with $3.45 \mathrm{~mol}$ of propane? (b) How many grams of $\mathrm{CO}_{2}$ can form from $0.177 \mathrm{~mol}$ of propane? (c) How many grams of water are produced by the combustion of $4.86 \mathrm{~mol}$ of propane?

   Propane burns according to the following equation:
$$
\mathrm{C}_{3} \mathrm{H}_{8}+5 \mathrm{O}_{2} \longrightarrow 3 \mathrm{CO}_{2}+4 \mathrm{H}_{2} \mathrm{O}
$$
(a) How many grams of $\mathrm{O}_{2}$ are needed to react fully with $3.45 \mathrm{~mol}$ of propane?
(b) How many grams of $\mathrm{CO}_{2}$ can form from $0.177 \mathrm{~mol}$ of propane?
(c) How many grams of water are produced by the combustion of $4.86 \mathrm{~mol}$ of propane?

Chemistry: The Molecular Nature of Matter

Neil D. Jespersen,… 7th Edition

Chapter 3, Problem 115

Instant Answer

Solved by Expert Dr. Satish Ingale

06/10/2021

Step 1

Step 1: We know that the balanced chemical equation is: $$ \mathrm{C}_{3} \mathrm{H}_{8}+5 \mathrm{O}_{2} \longrightarrow 3 \mathrm{CO}_{2}+4 \mathrm{H}_{2} \mathrm{O} $$ This tells us that one mole of propane reacts with five moles of oxygen to produce three moles Show more…

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Propane burns according to the following equation: $$ \mathrm{C}_{3} \mathrm{H}_{8}+5 \mathrm{O}_{2} \longrightarrow 3 \mathrm{CO}_{2}+4 \mathrm{H}_{2} \mathrm{O} $$ (a) How many grams of $\mathrm{O}_{2}$ are needed to react fully with $3.45 \mathrm{~mol}$ of propane? (b) How many grams of $\mathrm{CO}_{2}$ can form from $0.177 \mathrm{~mol}$ of propane? (c) How many grams of water are produced by the combustion of $4.86 \mathrm{~mol}$ of propane?

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Key Concepts

Balanced Chemical Equations

A balanced chemical equation provides the stoichiometric ratios between the reactants and products based on the law of conservation of mass. The coefficients in the equation indicate how many moles of each substance are involved in the reaction, which is crucial when calculating the amounts of substances consumed or formed.

Stoichiometry

Stoichiometry is the quantitative study of reactants and products in a chemical reaction. It uses the mole ratios from the balanced chemical equation to determine the relationship between the amounts (in moles or grams) of different substances involved in the reaction.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is used to convert between the mass of a substance and the number of moles, which is a key step in stoichiometric calculations.

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