Question

the equation for the decomposition of potassium chlorate is shown below.\\(\ce{kclo_{3}(s) \
ightarrow kcl(s) + o_{2}(g)}\\)\
which of the following shows the correctly balanced equation?\
choose 1 answer:\
a \\(\ce{2kclo_{3}(s) \
ightarrow 2kcl(}\\,\
\
b \\(\ce{2kclo_{3}(s) \
ightarrow kcl(s)}\\)\
\
c \\(\ce{2kclo_{3}(s) \
ightarrow 2kcl(}\\,\
\
scroll answers

Explanation:

Step1: Balance K and Cl

On the left, we have 1 K and 1 Cl in \( \text{KClO}_3 \). On the right, in \( \text{KCl} \), we have 1 K and 1 Cl. Let's start by balancing O. The left has 3 O (in \( \text{KClO}_3 \)), the right has 2 O (in \( \text{O}_2 \)). The least common multiple of 3 and 2 is 6. So we need 6 O on both sides. For the left, \( \text{KClO}_3 \) has 3 O, so we put a coefficient of 2 in front of \( \text{KClO}_3 \) (giving \( 2 \times 3 = 6 \) O). Then, for the right, \( \text{O}_2 \) needs a coefficient of 3 (since \( 3 \times 2 = 6 \) O). Now, with 2 \( \text{KClO}_3 \), we have 2 K and 2 Cl on the left, so we need 2 K and 2 Cl on the right, so we put a coefficient of 2 in front of \( \text{KCl} \). So the balanced equation is \( 2\text{KClO}_3(s)
ightarrow 2\text{KCl}(s) + 3\text{O}_2(g) \). Looking at the options (assuming option A is \( 2\text{KClO}_3(s)
ightarrow 2\text{KCl}(s) + 3\text{O}_2(g) \) as the visible part suggests), option A should be correct.

Step2: Analyze options

• Option B: \( 2\text{KClO}_3(s)

ightarrow \text{KCl}(s) \) – K and Cl are not balanced (2 on left, 1 on right), and O is not balanced.

• Option C: (assuming the full equation for C is incorrect, but from the visible, A has the correct balancing for K, Cl, and O when considering the standard decomposition.

Answer:

A. \( 2 \text{KClO}_3(s)
ightarrow 2 \text{KCl}(s) + 3 \text{O}_2(g) \) (assuming the full option A is this balanced equation)