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2 years ago

14

What is the mass of solute dissolved in 10.0 g of 5.00% Sugar solution?

1 answer:

cupoosta [38]2 years ago

3 0

Answer:

0.5 g or D

Explanation:

what is the mass of solute dissolved in 10.0 g of 5.00% Sugar solution?

A. 0.900 g

B. 0.180 g

C. 10.0 g

D. 0.500 g

E. 9.50 g

5% of the solution is sugar

o 10 g of the solution will have 9.5 g H2O and 0.5 g of sugar

0.5 /(9.5 +0.5) = 0.5/10 = 0.05 = 5 PER HUNDRED = 5%

so 0.5 g or D

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A fossil was analyzed and determined to have a carbon-14 level that is 70 % that of living organisms. The half-life of C-14 is 5

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2 years ago

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When methane ( CH4 ) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reac

slega [8]

<h2>Answer:</h2> $1.33*10^{-2}grams$

<h2>Explanations</h2>

The complete balanced equation for the given reaction is expressed as;

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Determine the moles of methane

$\begin{gathered} moles\text{ of CH}_4=\frac{mass}{molar\text{ mass}} \\ moles\text{ of CH}_4=\frac{0.0059}{16.04} \\ moles\text{ of CH}_4=0.000368moles \end{gathered}$

According to stoichimetry, 1 mole of methane produces 2 moles of water, hence the moles of water required will be:

$\begin{gathered} moles\text{ of H}_2O=\frac{2}{1}\times0.000368 \\ moles\text{ of H}_2O=0.000736moles \end{gathered}$

Determine the mass of water produced

$\begin{gathered} Mass\text{ of H}_2O=moles\times molar\text{ mass} \\ Mass\text{ of H}_2O=0.000736\times18.02 \\ Mass\text{ of H}_2O=0.0133grams=1.33\times10^{-2}grams \end{gathered}$

Therefore the mass of water produced from the complete combustion of 5.90×10−3 g of methane is 1.33 * 10^-2grams

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