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3 years ago

How could weathering by release of pressure affect the amount of weathering by freezing and thawing?

1 answer:

7 0

When the water in the cracks freezes, it expands by 9 to 10 percent, exerting pressure on the rock, according to BBC Bitesize. This action can widen the cracks in the rock, and when the temperature rises above freezing, the ice thaws, allowing the water to seep further into the cracks.

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The strength of the gravitational force between two objects depends on __________.

irga5000 [103]

Should be their masses. Because t<span>he strength of the gravitational force between two objects depends on two factors, mass and </span>distance<span>. the force of gravity the masses exert on each other. If one of the masses is doubled, the force of gravity between the objects is doubled. increases, the force of gravity decreases.</span>

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3 years ago

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Classifying Chemical Reactions

olga2289 [7]

Answer:

chemestry

Explanation:

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3 years ago

How many molecules are there in 6.73 moles of phosphorus trichloride? (write your answer in scientific notation).

anyanavicka [17]

Answer: There are $4.05\times 10^{24}$ molecules in 6.73 moles of phosphorus trichloride

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

1 mole of $PCl_3$ contains = $6.023\times 10^{23}$ molecules

Thus 6.73 moles of $PCl_3$ contains = $\frac{6.023\times 10^{23}}{1}\times 6.73=4.05\times 10^{24}$ molecules

Thus there are $4.05\times 10^{24}$ molecules in 6.73 moles of phosphorus trichloride

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3 years ago

The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: NO(g) + NO(g) → N2O2(g) (fast)

Karo-lina-s [1.5K]

Answer:

b. Second order in NO and first order in O₂.

Explanation:

A. The mechanism

$\rm 2NO\xrightarrow[k_{-1}]{k_{1}}N_{2}O_{2} \, (fast)\\\rm N_{2}O_{2} + O_{2}\xrightarrow{k_{2}} 2NO_{2} \, (slow)$

B. The rate expressions

$-\dfrac{\text{d[NO]} }{\text{d}t} = k_{1}[\text{NO]}^{2} - k_{-1} [\text{N}_{2}\text{O}_{2}]^{2}\\\\\rm -\dfrac{\text{d[N$_{2}$O$_{2}$]}}{\text{d}t} = -\dfrac{\text{d[O$_{2}$]}}{\text{d}t} = k_{2}[ N_{2}O_{2}][O_{2}] - k_{1} [NO]^{2}\\\\\dfrac{\text{d[NO$_{2}$]}}{\text{d}t}= k_{2}[ N_{2}O_{2}][O_{2}]$

The last expression is the rate law for the slow step. However, it contains the intermediate N₂O₂, so it can't be the final answer.

C. Assume the first step is an equilibrium

If the first step is an equilibrium, the rates of the forward and reverse reactions are equal. The equilibrium is only slightly perturbed by the slow leaking away of N₂O₂ to form product.

$\rm k_{1}[NO]^{2} = k_{-1} [N_{2}O_{2}]\\\\\rm [N_{2}O_{2}] = \dfrac{k_{1}}{k_{-1}}[NO]^{2}$

D. Substitute this concentration into the rate law

$\rm \dfrac{\text{d[NO$_{2}$]}}{\text{d}t}= \dfrac{k_{2}k_{1}}{k_{-1}}[NO]^{2} [O_{2}] = k[NO]^{2} [O_{2}]$

The reaction is second order in NO and first order in O₂.

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3 years ago

What type of potential energy do fuels contain

NISA [10]

Kinetic energy maybe or something

6 0

3 years ago

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