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bagirrra123 [75]
3 years ago
5

This is a type of element or substance that is not a metal.

Chemistry
1 answer:
Aloiza [94]3 years ago
3 0
Non-metal elements are Noble gases,Halogens,nonmetals,semimetals(metalloids). ( and maybe other metals)
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What would happen to the pressure if the volume were reduced to 0.5 l and the temperature increased to 260 ∘c?
Vsevolod [243]
<span>The ideal gas law. PV=nRT pressure x volume = moles x Faraday's constant x Temp Kelvin (C+273) Original data Pressure 1 atmosphere Volume 1 liter Temp 25C = 298K New data Volume 0.5 liter pressure X Temp 260C = 533K P1v1T1 = P2v2T2 plug and chug. (1)(1)(293) = (x)(0.5)(533) Solve for X, which is the new pressure. </span>
8 0
3 years ago
What volume would 0.853 moles of Nitrogen gas occupy at STP?
beks73 [17]

Answer:

19.12 L

Explanation:

At STP(i.e. Standard temperature and pressure).

The volume occupied by one mole of gas = 22.4 L

The pressure = 1 atm

The temperature = 273 K

Thus, since 1 mole of gas = 22.4 L;

Then 0.853 moles of N2 gas will occupy:

= (0.853 moles of N2 gas × 22.4 L)/ 1 mole of N2 gas

= 19.12 L

6 0
3 years ago
A 275 g sample of a metal requires 10.75 kJ to change its temperature from 21.2 oC to its melting temperature, 327.5 oC. What is
Vlada [557]

Answer:

c=0.127\ J/g^{\circ} C

Explanation:

Given that,

Mass of the sample, m = 275 g

It required 10.75 kJ of heat to change its temperature from 21.2 °C to its melting temperature, 327.5 °C.

We need to find the specific heat of the metal. The heat required by a metal sample is given by :

Q=mc\Delta T

c is specific heat of the metal

c=\dfrac{Q}{m\Delta T}\\\\c=\dfrac{10.75\times 10^3\ J}{275\times (327.5 -21.2)}\\\\=0.127\ J/g^{\circ} C

So, the specific heat of metal is 0.127\ J/g^{\circ} C.

4 0
2 years ago
Calculate the amount of heat required to raise the temperature of a 24 g sample of water from 9°C to 23°C.
borishaifa [10]

Answer:

1400KJ/mol⁻¹

Explanation:

Amount of heat required can be found by:

Q = m × c × ΔT

<em>Where m is the mass, c is the specific heat capacity (4.2KJ for water) and ΔT is the change in temperature.</em>

Q = 24 × 4.2 × (23 - 9)

= 24 × 4.2 × 14

=   1411.2KJ/mol⁻¹

= <u>1400KJ/mol⁻¹</u>  (to 2 significant figures)

7 0
3 years ago
Match these items with their examples.
kiruha [24]
Here you go! Feel free to ask questions!

7 0
3 years ago
Read 2 more answers
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