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Temka [501]
2 years ago
10

If 3.11 mol of an ideal gas has a pressure of 2.91 atm and a volume of 78.13 L, what is the temperature of the sample in degrees

Celsius?
Chemistry
1 answer:
nadezda [96]2 years ago
7 0

Answer: 617.35 °C

Explanation:

Using the ideal gas law,

PV = nRT

P = Pressure in (atm or pascal)

V = Volume in (litres or cubic metres)

n = number of moles.

R = Gas constant in (0.0821L .atm/mol.K or 8.314J/mol/K)

T = Temperature in degree Kelvin or Celsius.

PV = nRT

P = 2.91atm, V= 78.13L , n= 3.11

R = 0.0821L .atm/mol.K

T = ?

T = 2.91 x 78.13 / 3.11 x 0.0821 = 227.3583/ 0.255331 = 890.5 K

Converting from Kelvin to Celsius, using: °C = K - 273.15

= 890.5 - 273.15

°C = 617.35

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Answer: KNO_3 incorporates both ionic bonding and covalent bonding.

Explanation:

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An ionic bond is formed when an element completely transfers its valence electron to another element. The element which donates the electron is known as electropositive element and the element which accepts the electrons is known as electronegative element. This bond is formed between a metal and an non-metal.

For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.

Here potassium is having an oxidation state of +1 called as K^{+} cation and nitrate NO_3^{-} is an anion with oxidation state of -1. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral KNO_3. NO_3^- is formed by sharing of electrons between two non metals nitrogen and oxygen.

Thus KNO_3 incorporates both ionic bonding and covalent bonding.

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A solution has a [OH−] of 1 x 10−12. What is the pOH of this solution?<br> 2<br> 7<br> 10<br> 12
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How many mL of a 1.48 M calcium hydroxide solution are needed to neutralize 36.0 mL of a 1.63 M hydrochloric acid solution
Lelechka [254]

The volume (in mL) of calcium hydroxide, Ca(OH)₂ needed for the reaction is 19.8 mL

<h3>Balanced equation </h3>

2HCl + Ca(OH)₂ —> CaCl₂ + 2H₂O

From the balanced equation above,

  • The mole ratio of the acid, HCl (nA) = 2
  • The mole ratio of the base, Ca(OH)₂ (nB) = 1

<h3>How to determine the volume of Ca(OH)₂ </h3>
  • Molarity of base, Ca(OH)₂ (Mb) = 1.48 M
  • Volume of acid, HCl (Va) = 36 mL
  • Molarity of acid, HCl (Ma) = 1.63 M
  • Volume of base, Ca(OH)₂ (Vb) =?

MaVa / MbVb = nA / nB

(1.63 × 36) / (1.48 × Vb) = 2

58.68 / (1.48 × Vb) = 2

Cross multiply

2 × 1.48 × Vb = 58.68

2.96 × Vb = 58.68

Divide both side by 2.96

Vb = 58.68 / 2.96

Vb = 19.8 mL

Learn more about titration:

brainly.com/question/14356286

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