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2 years ago

Help me! Who ever gets to answer and has the best answer gets brainliest

Chemistry

2 answers:

Troyanec [42]2 years ago

7 0

Answer:

Fires - These consume fuel and covert chemical energy stored in that fuel into thermal, light and sound energy

Decay - The breakdown of dead plants and animals produces thermal energy

Earth - Thermal energy comes from deep inside and is called geothermal energy

Explanation:

Fires, when you burn wood, you convert chemical energy from the wood into thermal (warmth from the fire), light (glow from the fire), sound (crackling sound of wood burning)

Decay - I can't explain that one to you but there are power plants that use decomposition to produce energy

Earth - Beneath the crust there is the mantle, which consists of molten rock which produces a lot of thermal energy. This can be seen in geysers, where the molten rock heats water and hot water can burst out of the surface. Applies to hot springs too

gayaneshka [121]2 years ago

6 0

Answer:

Decay-the breakdown of dead plants..

Earth- thermal energy comes from deep inside...

Fires- these consume feul...

Explanation:

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A sample of a pure substance with a density of 3 g/mL is separated into two pieces. One piece has a mass of 50 g and the other p

pshichka [43]

Answer:

8.3ml

Explanation:

to get volume u have to divide 25g over the density, i rounded to the nearest tenth, if you don't want to then write out the full number with all the decimals

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2 years ago

Match the correct simple with the correct elements of safety

grigory [225]

c. 12. preparing data tables and gathering safety equipment

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2 years ago

A student dissolved 1.805g of a monoacidic weak base in 55mL of water. Calculate the equilibrium pH for the weak monoacidic base

yawa3891 [41]

Answer:

11.39

Explanation:

Given that:

$pK_{b}=4.82$

$K_{b}=10^{-4.82}=1.5136\times 10^{-5}$

Given that:

Mass = 1.805 g

Molar mass = 82.0343 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{1.805\ g}{82.0343\ g/mol}$

$Moles= 0.022\ moles$

Given Volume = 55 mL = 0.055 L ( 1 mL = 0.001 L)

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$Molarity=\frac{0.022}{0.055}$

Concentration = 0.4 M

Consider the ICE take for the dissociation of the base as:

B + H₂O ⇄ BH⁺ + OH⁻

At t=0 0.4 - -

At t =equilibrium (0.4-x) x x

The expression for dissociation constant is:

$K_{b}=\frac {\left [ BH^{+} \right ]\left [ {OH}^- \right ]}{[B]}$

$1.5136\times 10^{-5}=\frac {x^2}{0.4-x}$

x is very small, so (0.4 - x) ≅ 0.4

Solving for x, we get:

x = 2.4606×10⁻³ M

pOH = -log[OH⁻] = -log(2.4606×10⁻³) = 2.61

pH = 14 - pOH = 14 - 2.61 = 11.39

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2 years ago

Which of the following is true for a chemical reaction at equilibrium?

victus00 [196]

Answer:

youre gonna have to include the answers for me to help

Explanation:

7 0

1 year ago

A 1.26 m aqueous solution of an ionic compound with the formula mx2 has a boiling point of 101.63 ∘c. part a calculate the van't

12345 [234]

Answer is: Van't Hoff factor (i) for this solution is 1.051 .
Change in boiling point from pure solvent to solution: ΔT =i · Kb · b.
Kb - molal boiling point elevation constant is 0.512°C/m.
b - molality, moles of solute per kilogram of solvent.
b = 1.26 m.
ΔT = 101.63°C - 100°C = 1.63°C.

i = 1.63°C ÷ (0.512°C/m · 1.26 m).

i = 1.051.

5 0

2 years ago

Read 2 more answers