As we move ACROSS the periodic table in a row, the electronegativity

When dinitrogen pentaoxide, a white solid, is heated, it decomposes to produce nitrogen dioxide gas and

AysviL [449]

9.5314 L is the volume of nitrogen dioxide formed at 103.25 kPa and 22.75 °C.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Given data:

Oxygen produced - 1.618 gram

Decomposition of $N_2O_5$ takes place.

Find - Amount of $NO_2$ produced.

The decomposition reaction is as follows -

$2N_2O_5$ --> $4NO_2 + O_2$

Moles of $O_2$ gas = $\frac{1.6}{16}$ =0.1 moles.

1 mole of $O_2$ is produced from 2 moles of dinitrogen pentoxide

0.1 mole of $O_2$ will be produced from = 0.2 moles.

Now, 2 moles of dinitrogen pentoxide produce 4 moles of $NO_2$

$NO_2$ produced will be - 0.4 moles.

Weight of $NO_2$ produced - 0.4 X 46

Weight of $NO_2$ produced - 18.4 gram

Thus, grams of $NO_2$ produced are 18.4

Now calculate the volume of $NO_2$

Given data are:

P=103.25 kPa =1.01899827 atm

T= 22.75 °C +273 = 295.75 K

n=0.4 moles

V=?

R= 0.0821 liter·atm/mol·K

Putting the value in PV=nRT

V = $\frac{nRT}{P}$

V = $\frac{0.4 \;moles \;X \;0.0821\; liter\;atm/\;mol \;K X \;295.75 \;K}{1.01899827 atm}$

V= 9.5314 L

Hence, 9.5314 L is the volume of nitrogen dioxide formed at 103.25 kPa and 22.75 °C.

Learn more about the ideal gas equation here:

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8 0

2 years ago

What is the name of this hydrocarbon?

Deffense [45]

Answer:

1-Fluoro-4-nitrobenzene

Step-by-step explanation:

Step 1. Identify the substituents on the ring,

The groups are fluoro and nitro. They have no priority as functional groups, so the base name is benzene.

Step 2. Identify their relative priorities.

F and NO₂ have no functional group priority, so we list them in alphabetical order. F has alphabetical priority over NO₂. The name becomes fluoronitrobenzene.

Step 3. Number the atoms of the ring.

The C atom bearing the F is C1. Count around the ring, and the NO₂ group is on C4.

Step 4. Name the compound.

Insert the locating numbers immediately in front of the substituents. Use hyphens to join letters to numbers.

The name becomes 1-fluoro-4-nitrobenzene.

7 0

4 years ago

Complete the nuclear equation 42 K → 0 e 19____-1

kenny6666 [7]

Answer:

42 19 K→42 20 Ca+e−

Explanation:

Naturally-occurring potassium atoms have a weighted average atomic mass of 39.10 (as seen on most modern versions of the periodic table.) Each potassium atom contains 19 protons p+ and thus an average potassium atom contains about 39.10−19≈20 neutrons n0.

This particular isotope of potassium-42 contains 42 nucleons (i.e., protons and neutrons, combined;) Like other isotopes of potassium 19 out of these nucleons are protons; the rest 42−19=23 are therefore neutrons.

5 0

3 years ago

What is thermite reaction

barxatty [35]

Answer and Explanation:

$Hello!~$

$Let's~answer~your~question!$

$A~ thermite~ reaction ~is~ basically ~when~iron$ $~oxide~ (rust)~ reacting ~with ~aluminum~ to ~produce ~molten ~iron.$

$Hope~this~helped!$

$Have~a~blessed~day~ahead!$

7 0

3 years ago

Read 2 more answers

A chemist adds of a aluminum chloride solution to a reaction flask. Calculate the mass in grams of aluminum chloride the chemist

andreyandreev [35.5K]

Answer:

10.8 g

Explanation:

A chemist adds 480.0 mL of a 0.169 mol/L aluminum chloride solution to a reaction flask. Calculate the mass in grams of aluminum chloride the chemist has added to the flask. Round your answer to 3 significant digits.

Step 1: Given data

Volume of the solution: 480.0 mL

Concentration of the aluminum chloride solution: 0.169 mol/L

Step 2: Calculate the moles of aluminum chloride in the solution

We will multiply the volume of the solution by the molarity.

0.4800 L × 0.169 mol/L = 0.0811 mol

Step 3: Calculate the mass corresponding to 0.0811 moles of AlCl₃

The molar mass of AlCl₃ is 133.34 g/mol.

0.0811 mol × 133.34 g/mol = 10.8 g

3 0

3 years ago