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3 years ago

While Cameron is intensely working out, his muscles begin to get sore and start to burn. What type of cellular

Chemistry

1 answer:

max2010maxim [7]3 years ago

4 0

Answer:

1) Anaerobic respiration

2) Lactic acid

3) Stop the work out

Explanation:

1) Anaerobic respiration

Muscular anaerobic respiration to produce energy during exercises or workout, takes place when the level of oxygen available for the amount of energy being generated is not sufficient, and the balance generated energy is produced along with lactic acid by anaerobic respiration

2) Lactic acid

The produced lactic acid from the anaerobic respiration at the muscle sites results in a burning sensation being felt during strenuous muscular activity in the presence of low oxygen supply

3) Stop the work out

In order to stop the burning, the muscular activity is to be stopped, to allow the resumption of the aerobic process of energy production, and to allow the produced lactic acid to be cleared

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Answer:

k = 1.3 x 10⁻³ s⁻¹

Explanation:

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Ln [A]t/[A]₀ = - kt

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We are given the half life for the concentration of acetaldehyde to fall to one half its original value, thus

Ln [A]t/[A]₀ = Ln 1/2[A]₀/[A]₀= Ln 1/2 = - kt

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3 years ago

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Answer:

89.6L

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1mole of CO2 occupies 22.4L at stp.

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3 years ago

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Magnesium metal (0.100 mol) and a volume of aqueous hydrochloric acid that contains 0.500 mol of HCl are combined and react to c

jok3333 [9.3K]

Answer:

2.24 L of hydrogen gas, measured at STP, are produced.

Explanation:

Given, Moles of magnesium metal, $Mg$ = 0.100 mol

Moles of hydrochloric acid, $HCl$ = 0.500 mol

According to the reaction shown below:-

$Mg_{(s)} + 2HCl_{(aq)}\rightarrow MgCl_2_{(aq)} + H_2_{(g)}$

1 mole of Mg reacts with 2 moles of $HCl$

0.100 mol of Mg reacts with 2*0.100 mol of $HCl$

Moles of $HCl$ must react = 0.200 mol

Available moles of $HCl$ = 0.500 moles

Limiting reagent is the one which is present in small amount. Thus, $Mg$ is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

1 mole of $Mg$ on reaction forms 1 mole of $H_2$

0.100 mole of $Mg$ on reaction forms 0.100 mole of $H_2$

Mole of $H_2$ = 0.100 mol

At STP,

Pressure = 1 atm

Temperature = 273.15 K

Volume = ?

Using ideal gas equation as:

$PV=nRT$

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

1 atm × V L = 0.100 × 0.0821 L.atm/K.mol × 273.15 K

2.24 L of hydrogen gas, measured at STP, are produced.

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3 years ago