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Natasha2012 [34]

3 years ago

8

in an experiment forest, a sample of leaves is weighed over a one year period and is found to lose 83% of its mass. assuming fir

st order kinectics, what is the rate constant for their decomposition

1 answer:

Darina [25.2K]3 years ago

4 0

Rate constant = .17 maybe I don't really know tho so don't take my word for it. #woot woot

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Applications of chemistry in medical field

OLga [1]

Answer:

Explanation:

Drug for the treatment of disease. Chemistry contributes to the preparation and use of materials for surgery (sutures, artificial skin, and sterile materials). ...

Surgical procedure. ...

Blood samples for laboratory testing. ...

Blood glucose testing device.

6 0

2 years ago

Gallionella bacteria can get energy from the reaction fe2+ → fe3+. This reaction is an example of

djverab [1.8K]

The gallionella bacteria reaction

that is Fe2+ → Fe3+ is example of oxidation reaction (answer A)

Explanation

oxidation reaction reaction occurs when electrons are lost during reaction by a molecule or ion or atom. when oxidation occurs the oxidation state of the molecule or ion or atom increases. For this reason Fe2+ → Fe3+ is a oxidation reaction since the oxidation state move from oxidation state 2 to 3

4 0

3 years ago

Read 2 more answers

The Big Bang theory states that ________.

cluponka [151]

I believe the correct answer is B

8 0

3 years ago

Determine the heat of reaction (ΔHrxn) for the combustion of ethanol (C2H5OH) by using heat of formation data: C2H5OH (l) + 3 O2

egoroff_w [7]

Answer:

$\Delta H_{rxn}=-1234.782kJ$

Explanation:

$\Delta H_{rxn}=\sum [n_{i}\times \Delta H_{f}^{0}(product)_{i}]-\sum [n_{j}\times \Delta H_{f}^{0}(reactant_{j})]$

Where $n_{i}$ and $n_{j}$ are number of moles of product and reactant respectively (equal to their stoichiometric coefficient).

$\Delta H_{f}^{0}$ is standard heat of formation.

So, $\Delta H_{rxn}=[2mol\times \Delta H_{f}^{0}(CO_{2})_{g}]+[3mol\times \Delta H_{f}^{0}(H_{2}O)_{g}]-[1mol\times \Delta H_{f}^{0}(C_{2}H_{5}OH)_{l}]-[3mol\times \Delta H_{f}^{0}(O_{2})_{g}]$

or, $\Delta H_{rxn}=[2mol\times -393.509kJ/mol]+[3mol\times -241.818kJ/mol]-[1mol\times -277.69kJ/mol]-[3mol\times 0kJ/mol]$

or, $\Delta H_{rxn}=-1234.782kJ$

4 0

3 years ago

Helga [31]

I think it’s tissue I just did it

5 0

2 years ago