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2 years ago

1. Define anthracite.

Chemistry

2 answers:

AnnZ [28]2 years ago

7 0

Answer:

Antharacite refers to a hard coal of hard variety that contains relatively pure carbons ...

faltersainse [42]2 years ago

6 0

Answer:

a hard natural coal of high luster differing from bituminous coal in containing little volatile matter and in burning very cleanly is called anthracite . called also hard coal

Explanation:

Answer from Gauth math

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The compound trimethylamine, (CH3)3N, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibr

GREYUIT [131]

Answer:

The $K_b$ expression for the weak base equilibrium is:

$K_b=\frac{[(CH_3)_3NH^+][OH^-]}{[(CH_3)_3N]}$

Explanation:

$(CH_3)_3N(aq)+H_2O(l)\rightlefharpoons (CH_3)_3NH^++OH^-(aq)$

The expression of the equilibrium constant of base $K_c$ can be given as:

$K_c=\frac{[(CH_3)_3NH^+][OH^-]}{[(CH_3)_3N][H_2O]}$

] $K_b=K_c\times [H_2O]=\frac{[(CH_3)_3NH^+][OH^-]}{[(CH_3)_3N]}$

As we know, water is pure solvent, we can put $[H_2O]=1$

$K_b=K_c\times 1=\frac{[(CH_3)_3NH^+][OH^-]}{[(CH_3)_3N]}$

So, the the $K_b$ expression for the weak base equilibrium is:

$K_b=\frac{[(CH_3)_3NH^+][OH^-]}{[(CH_3)_3N]}$

6 0

2 years ago

750.0g of water that was just boiled (heated to 100.0/c loses 78.45KJ of heat as it cools.What is the final temperature of water

Iteru [2.4K]

Mass=m=750g=0.75kg
Q=78.45\times 10^3J=78450J
T_i=100°C
T_f=?
Specific heat capacity=c=4200J/kg°C

According to thermodynamics

$\\ \tt\bull\rightarrowtail Q=mc\Delta T$

$\\ \tt\bull\rightarrowtail Q/mc=\Delta T$

$\\ \tt\bull\rightarrowtail \Delta T=\dfrac{78450}{0.75(4200)}$

$\\ \tt\bull\rightarrowtail \Delta T=24.9°C$

$\\ \tt\bull\rightarrowtail T_i-T_f=24.9$

$\\ \tt\bull\rightarrowtail T_f=100-24.9=76.1°C$

4 0

2 years ago

Pls help :(

Ilia_Sergeevich [38]

I would say only two

7 0

2 years ago

Read 2 more answers

Methanol, CH3OH, has been considered as a possible fuel. Consider its oxidation: 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) ΔG =

Inessa [10]

<u>Answer:</u> Maximum work that can be obtained by given amount of methanol is -343kJ.

<u>Explanation:</u>

For the given chemical reaction:

$2CH_3OH(l)+3O_2(g)\rightarrow 2CO_2(g)+4H_2O(g);\Delta G_{rxn}=-1372kJ/mol$

By Stoichiometry of the reaction:

2 moles of methanol does a work of 1372 kJ.

So, 0.5 moles of methanol will do a work of = $\frac{1372kJ}{2}\times 0.5=343kJ$

Hence, maximum work that can be obtained by given amount of methanol is -343kJ.

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2 years ago

Please help due today

Murljashka [212]

The answer for the question is c.

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2 years ago

1. Define anthracite.​

1. Define anthracite.