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2 years ago

The ideal gas law equation is: PV = nRT

Chemistry

1 answer:

nignag [31]2 years ago

8 0

Answer:

The answer is the first option 0.37 moles

Explanation:

the ideal gas law is PV = nRT, so in the terms of n,

n = PV/RT (divide both sides by RT to let n stand alone)

given: P = 700 kpa, V = 2L, T = 450 K , R = 8.31

n = (700 * 2) / (8.31 * 450)

= 1400/3739.5

= 0.34

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Write the autoionization reaction for methanol, ch3oh.

aliina [53]

Autoionization Reactions are those reactions in which ions or molecules ionizes spontaneously without adding any external reagent.

For Example,
Autoionization of water.

H₂O + H₂O ⇆ H₃O⁺ + OH⁻

Autoionization reaction of Methanol is shown below,

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3 years ago

Which element would have properties most similar to those of

zysi [14]

Answer:

Explanation:

This is because they are in the same group which means they share similar properties.

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3 years ago

What are the differences between thermoplastics and thermosetting plastics? Give examples and draw a simple diagram to show what

Olenka [21]

on the basis of the reaction of heat in plastic , their are two types of plastics : 

<h2>Thermoplastic & Thermosetting plastics </h2>

Thermoplastics : Plastics which easily get deformed (become soft )on heating and also get bend easily are known as thermoplastics .

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4 0

3 years ago

A substance is analyzed and found to contain 85.7% carbon and 14.3% hydrogen by weight. A gaseous sample of the substance is fou

atroni [7]

Answer:

The empirical formula of the compound is CH2

Explanation:

Step 1: Data given

A substance contains 85.7 % carbon and 14.3 % hydrogen.

The substance has a density of 1.87 g/L

1 mol occupies 22.4 L

Molar mass of carbon = 12 g/mol

Molar mass of hydrogen = 1.01 g/mol

Step 2: Calculate molar mass of the substance

Since 1 mol occupies 22.4 L;

1 mol of this substance = 1.87g/L *22.4 = 41.888 grams

This means the molar mass of the substance is 41.888 g/mol

Step 3: Calculate mass of carbon:

85.8 % is carbon

this means 41.888 * 0.858 = 35.94 grams

Step 4: Calculate moles of carbon

moles C = mass C/ Molar mass C

Moles C = 35.94 grams / 12 g/mol

Moles C = 2.995 moles

Step 5: Calculate mass of hydrogen:

14.3 % is hydrogen

this means 41.888 * 0.143 = 5.99 grams

Step 6 :Calculate moles of hydrogen

Moles H = 5.99 grams / 1.01 g/mol

Moles H = 5.93 moles

Step 7: Calculate mol ratio

Ratio C:H = 1:2

The empirical formule = CH2

Step 8: calculate molar formule

Molar mass of empirical formule = 14.02 g/mol

n = Molar mass of substance / molar mass of empirical formule

n = 41.888 / 14.02 = 3

This means we have to multiply the empirical formula by 3

3*(CH2) = C3H6

C3H6 can be propene or cyclopropane

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3 years ago

Calculate the work (kJ) done during a reaction in which the internal volume expands from 20 L to 43 L against an outside pressur

Alenkinab [10]

Answer:

$\large \boxed{\text{-10.0 kJ}}$

Explanation:

1. Calculate the work

w = - pΔV = -4.3 atm × (43 L - 20 L) = -4.3 × 23 L·atm = -98.9 L·atm

2. Convert litre-atmospheres to joules

$w = \text{-98.9 L\cdot$atm } \times \dfrac{\text{101.3 J}}{\text{1 L$\cdot$atm }} = \text{-10000 J} = \textbf{-10.0 kJ}\\\\\text{The work done is $\large \boxed{\textbf{-10.0 kJ}}$}$

The negative sign indicates that the work was done against the surroundings.

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3 years ago