Living by Chemistry

Angelica M. Stacy

Chapter 19 Measuring Energy - all with Video Answers

Educators

Section 1

Combustion

02:03

Problem 1

What should you look for in a chemical formula to decide if a compound or element will not combust?

Vishal S.

Numerade Educator

04:05

Problem 2

Name three things that are true of every combustion reaction.

Vishal S.

Numerade Educator

03:43

Which of the substances listed below will combust? Explain your reasoning.
$\begin{array}{ll}{\text { a. } \mathrm{Na}_{2} \mathrm{SO}_{4}(s)} & {\text { b. } \mathrm{Cu}(s)} & {\text { c. } \mathrm{MgO}(s)} \\ {\text { d. } \mathrm{Na}(s)} & {\text { e. } \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(l)} & {\text { f. } \mathrm{Ar}(g)}\end{array}$

Vishal S.

Numerade Educator

07:08

Problem 4

Balance the following equations for combustion reactions. Circle the fuel for each reaction.
a. $\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
b. $\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{6}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
c. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
d. $\mathrm{C}_{21} \mathrm{H}_{24} \mathrm{N}_{2} \mathrm{O}_{4}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NO}_{2}(g)$
e. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{SH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{2}(g)$

Vishal S.

Numerade Educator

05:41

Problem 5

What are the products of these combustion reactions? Write balanced chemical equations for each reaction.
$\begin{array}{ll}{\text { a. } \mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}(l)+\mathrm{O}_{2}(g) \longrightarrow} & {\text { b. } \mathrm{CH}_{3} \mathrm{COCH}_{3}(l)+\mathrm{O}_{2}(g) \longrightarrow} \\ {\text { c. } \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(s)+\mathrm{O}_{2}(g) \longrightarrow} & {\text { d. } \mathrm{Ca}(s)+\mathrm{O}_{2}(g) \longrightarrow} \\ {\text { e. } \mathrm{Li}(s)+\mathrm{O}_{2}(g) \longrightarrow} & {\text { f. } \operatorname{Si}(s)+\mathrm{O}_{2}(g) \longrightarrow}\end{array}$

Vishal S.

Numerade Educator