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3 years ago

If you had 20,000 litres of NO2 how many moles would you have

Chemistry

1 answer:

vova2212 [387]3 years ago

6 0

Answer:

The correct answer is 0.89 mol.

Explanation:

At STP (Standard Temperature and Pressure) conditions, 1 mol of an ideal gas occupies a volume of 22.4 L. If we assume STP conditions, we can consider a convertion factor of 1 mol/22.4 L to convert the volume of NO₂ from liters to moles:

20,00 L x 1 mol/22.4 L = 0.89 mol

So, at STP, we would have 0.89 mol of NO₂

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Whats the balanced equation for sodium hydroxide + ammonium sulphate=sodium sulphate + amonia + h2o

Nady [450]

Answer:

2NaOH + (NH4) 2SO4 = Na2SO4(s) + 2NH3(g) + 2H2O(l)

Two moles of sodium hydroxide reacts with 1 Mike of ammonium sulphate to give 1 mole of Sodium sulphate, 2 moles of ammonia gas and 2 moles of water

Explanation:

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3 years ago

Why is the bond between two single hydrogen atoms stable?

Len [333]

B ia the correct one .

Hydrogen only uses the first energy shell, which holds 2 electrons, not 8.

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3 years ago

Read 2 more answers

The N2O4−NO2 reversible reaction is found to have the following equilibrium partial pressures at 100∘C. Calculate Kp for the rea

timofeeve [1]

Answer:

$K_{p}$ for the reaction is 18.05

Explanation:

Equilibrium constant in terms of partial pressure ( $K_{p}$ ) for this reaction can be written as-

$K_{p}=\frac{P_{NO_{2}}^{2}}{P_{N_{2}O_{4}}}$

where $P_{NO_{2}}$ and $P_{N_{2}O_{4}}$ are equilibrium partial pressure of $NO_{2}$ and $N_{2}O_{4}$ respectively

Hence $K_{p}=\frac{(0.095)^{2}}{(0.0005)}$ = 18.05

So, $K_{p}$ for the reaction is 18.05

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4 years ago

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denis-greek [22]

Answer:

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3 years ago

A sample of hydrogen was collected by water displacement at 23.0°C and an atmospheric pressure of 735 mmHg. Its volume is 568 mL

ziro4ka [17]

Answer:

V = 552 mL or 0.552 L

Explanation:

First, we need to calculate the number of moles of H2 using the ideal gas equation which is:

PV = nRT

Solving for n:

n = PV / RT

Where:

P = Pressure

V = Volume

R = Gas constant (0.082 L atm / K mol)

T = Temperature in K

Let's convert first both pressure in atm, remember that 1 atm = 760 mmHg

P = 735 / 760 = 0.967 atm

Pwater = 21 / 760 = 0.028 atm

Finally temperature to Kelvin:

T = 23 + 273.15 = 296.15 K

Now, at first the hydrogen was collected by water displacement so pressure is:

P = 0.967 - 0.028 = 0.939 atm

Now the moles of hydrogen:

n = 0.939 * 0.568 / 0.082 * 296.15

n = 0.022 moles

Now that we have the moles, let's calculate the volume when the pressure is 735 mmHg

V = nRT/P

V = 0.022 * 0.082 * 296.15 / 0.967

V = 0.552 L or 552 mL

This is the volume that hydrogen occupies.

6 0

3 years ago