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frozen [14]
4 years ago
14

Write a procedure that you would follow to demonstrate the effect of increasingly higher concentrations of hydrochloric acid on

its rate of reaction with antacid tablets.
Chemistry
1 answer:
Hitman42 [59]4 years ago
7 0
The reaction would produce bubbles of gas.

We can prepare 3-5 test tubes of acid with increasing concentrations. Then, we add antacid tablets to each and note the time taken for the tablet to dissolve and stop producing bubbles. The lesser the time taken, the greater the rate of reaction.
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After 5 minutes, 1.98x10^-23 moles of hydrogen gas is produced. How many grams of magnesium reacted?
yarga [219]

Answer:

\large \boxed{4.81 \times 10^{-22} \text{ g Mg}}

Explanation:

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

Mᵣ:         24.30

                Mg + 2H⁺ ⟶ Mg²⁺  +  H₂  

n/mol:                                      1.98 × 10⁻²³

1. Calculate the moles of Mg

The molar ratio is 1 mol Mg:1 mol H₂

\rm  \text{Moles of Mg} =1.98 \times 10^{-23} \text{ mol H}_{2} \times \dfrac{\text{1 mol Mg}}{\text{1 mol H}_{2}} = 1.98 \times 10^{-23} \text{ mol Mg}

2. Calculate the mass of Mg

\text{Mass of Mg} = 1.98 \times 10^{-23} \text{ mol Mg}  \times \dfrac{\text{24.30 g Mg}}{\text{1 mol Mg}} = \mathbf{4.81 \times 10^{-22}} \textbf{ g Mg}\\\\\text{The mass of Mg reacted is $\large \boxed{\mathbf{4.81 \times 10^{\mathbf{-22}} \textbf{ g Mg}}}$}

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