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Bond [772]
3 years ago
10

What happens to the particles of a gas when the gas turns to a liquid

Chemistry
2 answers:
vovangra [49]3 years ago
6 0
Pacticles of gas are more compact, but still have the ability to move.
Maurinko [17]3 years ago
6 0
It melts from evaporation in a liquid version of water
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What is the solubility of NH4Cl at 50°C?
NISA [10]

Answer : Option E) 50 grams.

Explanation : According to the solubility curves the compound NH_{4}Cl to dissolve at 50 °C in 100 mL of water will need 50 grams of the compound. It is clearly indicated in the graph which is marked with red that at 50°C approximately 50.4 grams of the compound NH_{4}Cl will be needed to dissolved in 100 mL of water to form a solution.


8 0
3 years ago
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!!NEED URGENT SCIENCE HELP!! Please help me with this I am so lost. I will mark you brainliest and like ur answer and rate it 5
Citrus2011 [14]

Answer:

1. D   2. C   3. B

Explanation:

1. The product is always what is being yielded from the equation, or what is created. Since both 4H2O and 3CO2 are created from the reactants, they are both products of the reaction.

2. The Law of Conservation of Matter states that matter cannot be created, nor destroyed. Therefore, C is not true because new atoms cannot be created in a reaction.

3. The second formula is balanced, but the first is not

5 0
2 years ago
What kind of molecule is depicted here?
mina [271]

Explanation:

Methane molecule is depicted here

3 0
3 years ago
Read 2 more answers
Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. Δ H°(kJ) K(s) → K(g) 89 K(g)
AURORKA [14]

Explanation:

The net equation will be as follows.

          K(s) + Cl_{2}(g) \rightarrow KCl(s)

So, we are required to find \Delta H_{formation} for this reaction.

Therefore, steps involved for the above process are as follows.

Step 1:  Convert K from solid state to gaseous state

          K(s) \rightarrow K(g),    \Delta H_{1} = 89 kJ

Step 2:  Ionization of gaseous K

           K(g) \rightarrow K^{+}(g) + e^{-},    H_{2} = 418 KJ

Step 3:  Dissociation of Cl_{2} gas into chlorine atom .

            \frac{1}{2} Cl_{2}(g) \rightarrow Cl(g),   \Delta H_{3} = \frac{244}{2} = 122 KJ

Step 4: Iozination of chlorine atom.

              Cl(g) + e^{-} \rightarro Cl^{-}(g),      H_{4} = -349 KJ

Step 5:  Add K^{+} ion and Cl^{-} ion formed above to get KCl .

              K^{+}(g) + Cl^{-}(g) \rightarrow KCl(s),   H_{5} = -717 KJ

Now, using Born-Haber cycle, value of enthalpy of the formation is calculated as follows.

      \Delta H_{f} = \DeltaH_{1} + \Delta H_{2} + \Delta H_{3} + \Delta H_{4} + \Delta H_{5}

                  = 89 + 418 + 122 - 349 - 717

                  = - 437 KJ/mol

Thus, we can conclude that the heat of formation of KCl is - 437 KJ/mol.

5 0
3 years ago
What is the molar mass of 4.23 g of an elemental gas in a 2.5L container at 282K and 1.4 atm?
balu736 [363]

Answer:

27.98g/mol

Explanation:

Using ideal gas law equation;

PV = nRT

Where;

P = pressure (atm)

V = volume (L)

T = temperature (K)

n = number of moles (mol)

R = gas law constant (0.0821 Latm/molK)

According to the information given:

V = 2.5L

P = 1.4 atm

T = 282K

n = ?

Using PV = nRT

n = PV/RT

n = 1.4 × 2.5/0.0821 × 282

n = 3.5/23.1522

n = 0.151mol

Using the formula to calculate molar mass of the elemental gas:

mole = mass/molar mass

Molar mass = mass/mole

Molar mass = 4.23g ÷ 0.151mol

Molar mass = 27.98g/mol

6 0
3 years ago
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