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mestny [16]
3 years ago
11

2 KClO_2 produces 2 KCl+ 3O_2 when heated. If this reaction produces 82.8 g of KCl how many grams of O2 were produced?

Chemistry
1 answer:
Ad libitum [116K]3 years ago
4 0

Answer:

37.046 grams of oxygen gas were produced.

Explanation:

2KClO_2\rightarrow 2KCl+ 3O_2

Moles of potassium chlorite = \frac{82.2 g}{106.5 g/mol}=0.7718 mol

According to reaction 2 moles of potassium chlorite gives 3 moles of oxygen gas.

Then 0.7718 moles of potassium chlorite will give:

\frac{3}{2}\times 0.7718 mol=1.1577 mol of oxygen gas.

Mass of 1.1577 moles of oxygen gas:

1.1577 mol × 32 g/mol = 37.046 g

37.046 grams of oxygen gas were produced.

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When the burner in a hot air balloon is turned on, the temperature of the air in the balloon ________ causing its volume to ____
raketka [301]

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4 0
3 years ago
If the half-life of Carbon-14 is 5700 years, how many years would it take a sample to decay from 1 gram to 31.3 mg
andrew-mc [135]

Answer:

28500 years

Explanation:

Applying,

A = A'(2^{x/y})............... Equation 1

Where A = Original mass of Carbon-14, A' = Final mass of carbon-14 after decaying, x = total time, y = half-life.

From the question,

Given: A = 1 g, A' = 31.3 mg = 0.0313 g, y = 5700 years.

Substitute these values into equation 1

1 = 0.0313(2^{x/5700})

2^{x/5700} = 1/0.0313

2^{x/5700}  = 31.95

2^{x/5700} ≈ 32

2^{x/5700} ≈ 2⁵

Equating the base and solve for x

x/5700 ≈ 5

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x ≈ 28500 years

3 0
3 years ago
A compound is found to contain 7.523% phosphorus and 92.48% iodine by weight. what is the empirical formula for this compound?
RUDIKE [14]
The answer is PI3
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5 0
3 years ago
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