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Yuri [45]
3 years ago
6

How many milliners of hydrogen gas ar produced by the reaction 0.020 moles of magnesium with excess of hydrochloride acid at sto

p
Chemistry
1 answer:
jeyben [28]3 years ago
5 0

Answer:- 448 mL of hydrogen gas are formed.

Solution:- It asks to calculate the volume of hydrogen gas formed in milliliters at STP when 0.020 moles of magnesium reacts with excess HCl acid. The balanced equation is:

Mg+2HCl\rightarrow MgCl_2+H_2(g)

There is 1:1 mol ratio between Mg and hydrogen gas. So, the moles of hydrogen gas is also equals to the moles of Mg reacted.

moles of Hydrogen gas formed = 0.020 mol

At STP, volume of 1 mol of the gas is 22.4 L. We need to calculate the volume of 0.02 moles of hydrogen gas.

0.02mol(\frac{22.4L}{1mol})

= 0.448 L

They want answer in mL. So, let's convert L to mL using the conversion formula, 1L = 1000mL

0.448L(\frac{1000mL}{1L})

= 448 mL

So, 0.020 moles of magnesium would produce 448 mL of hydrogen gas at STP on reacting with excess of HCl acid.

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A compound accepts electrons from another substance to form a covalent bond. The compound acts as a Lewis base.

<h3>What are the most common acid-base theories?</h3>
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A compound accepts electrons from another substance to form a covalent bond. Which term best describes this compound’s behavior?

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A compound accepts electrons from another substance to form a covalent bond. The compound acts as a Lewis base.

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A first-order reaction is 45% complete at the end of 43 minutes. What is the length of the half-life of this reaction
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  • Type of reaction = first order
  • Amount of Completion = 45%

<h3>Reaction Constant</h3>

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The reactant left = (1 - 0.45) X_0 = 0.55 X_0 = X

For a first order reaction

\ln(\frac{x}{x_o}) = -kt\\ k = \frac{1}{t}\ln (\frac{x_o}{x}) \\ k = \frac{1}{43}\ln (\frac{x_o}{0.55_o})\\ k = 0.013903 min^-^1

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The half-life of a reaction is said to be the time required for the initial amount of the reactant to reach half it's original size.

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Substitute the values

t_\frac{1}{2} = \frac{1}{k}\ln(2)=\frac{0.6931}{0.013903}\\t_\frac{1}{2}= 49.85 min = 50 min

The half-life of the reaction is 50 minutes

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