What is the mass of water that results from combining 2.0 g of hydrogen with 16.0 g of oxygen?

1 answer:

8 0

The formula for water is H2O so there would have to be two Hyrdogens and one oxygen. Therefore it would be 4g of Hydrogen and 16g of Oxygen leaving you with 20g.
The answer is D.

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Answer:

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Explanation:

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Answer:

$\boxed{\text{3.1 g}}$

Explanation:

We will need an equation with masses and molar masses, so let’s gather all the information in one place.

M_r: 315.46 76.12

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m/g: 6.5

1. Moles of Ba(OH)₂·8H₂O

$\text{Moles of Ba(OH)$_{2}\cdot $8H$_{2}$O}\\= \text{ 6.5 g Ba(OH)$_{2}\cdot $8H$_{2}$O} \times \dfrac{\text{1 mol Ba(OH)$_{2}\cdot $8H$_{2}$O}}{\text{ 315.46 g Ba(OH)$_{2}\cdot $8H$_{2}$O}}\\= \text{0.0206 mol Ba(OH)$_{2}\cdot $8H$_{2}$O}$

2. Moles of NH₄SCN

The molar ratio is 2 mol NH₄SCN:1 mol Ba(OH)₂·8H₂O

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3. Mass of NH₄SCN

$\text{Mass of NH$_{4}$SCN} = \text{0.0412 mol NH$_{4}$SCN} \times \dfrac{\text{76.12 g NH$_{4}$SCN}}{\text{1 mol NH$_{4}$SCN}} =\\\textbf{3.1 g NH$_{4}$SCN}\\\\\text{You must use }\boxed{\textbf{3.1 g}}\text{ NH$_{4}$SCN}$