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3 years ago

What is the mass of 2.15 liters of N2 gas at STP?

Chemistry

2 answers:

Musya8 [376]3 years ago

5 0

Explanation: molar mass of N2=28

Volume occupied at stp=22.4 so 28/22.4=1.25 so mass nitrogen will be 56 multiply 1.25 =70g

IgorLugansk [536]3 years ago

4 0

Answer: 2.68 grams

Explanation:

According to avogadro's law, 1 mole of the substance occupies 22.4 liters at STP and contains avogadro's number $6.023\times 10^{23}$ of particles and weighs equal to its molecular mass.

1 mole of $N_2$ weighs 28 grams.

Also 1 mole of $N_2$ occupies 22.4 Liters.

Thus 22.4 L $N_2$ weigh = 28 grams

2.15 L of $N_2$ weigh = $\frac{28}{22.4}\times 2.15=2.68g$

Thus the mass of nitrogen gas is 2.68 grams.

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Using the average initial pH of your acetic acid solutions (2.96), and the average molarity of those solutions(.0602), calculate

Orlov [11]

Answer : The value of Ka for acetic acid is, $2.03\times 10^{-5}$

Explanation :

The chemical formula of acetic acid is, $CH_3COOH$ .

The chemical equilibrium reaction will be:

$CH_3COOH\rightleftharpoons CH_3COO^-+H^+$

Given:

pH = 2.96

First we have to calculate the concentration of hydrogen ion.

$pH=-\log [H^+]$

$2.96=-\log [H^+]$

$[H^+]=1.096\times 10^{-3}M$

That means,

$[H^+]=[CH_3COO^-]=1.096\times 10^{-3}M$

$[CH_3COOH]=0.0602-(1.096\times 10^{-3})=0.0591M$

The expression for reaction is:

$K_a=\frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$

$K_a=\frac{(1.096\times 10^{-3})\times (1.096\times 10^{-3})}{0.0591}$

$K_a=2.03\times 10^{-5}$

Thus, the value of Ka for acetic acid is, $2.03\times 10^{-5}$

3 0

3 years ago

What is the percent by mass of water in Na S04.10H20?

dalvyx [7]

Answer:

Percent by mass of water is 56%

Explanation:

First of all calculate the mass of hydrated compound as,

Mass of Sodium = Na × 2 = 22.99 × 1 = 45.98 g

Mass of Sulfur = S × 1 = 32.06 × 1 = 32.06 g

Mass of Oxygen = O × 14 = 16 × 14 = 224 g

Mass of Hydrogen = H × 20 = 1.01 × 20 = 20.2 g

Mass of Na₂S0₄.10H₂O = 322.24 g

Secondly, calculate mass of water present in hydrated compound. For this one should look for the coefficient present before H₂O in molecular formula of hydrated compound. In this case the coefficient is 10, so the mass of water is...

Mass of water = 10 × 18.02

Mass of water = 180.2 g

Now, we will apply following formula to find percent of water in hydrated compound,

%H₂O = Mass of H₂O / Mass of Hydrated Compound × 100

Putting values,

%H₂O = 180.2 g / 322.24 g × 100

%H₂O = 55.92 % ≈ 56%

3 0

3 years ago

You have a balloon filled with hellum that has a volume of 4.91 cubic decimeters

juin [17]

Answer:

Explanation:

because the number of heliem is your aswer

5 0

2 years ago

Read 2 more answers

You carefully weigh out 11.00 g of caco3 powder and add it to 44.55 g of hcl solution. you notice bubbles as a reaction takes pl

Zinaida [17]

The bubbles that were observed after the mixing of the two substances is one of the products of the reaction. It is the carbon dioxide that is produced. To determine the mass of this gas produced, we need to remember the Law of conservation of mass where mass cannot be created or destroyed. With this, we can say that the total mass that goes in a process should be equal to the mass that is goes out of the process no matter what the reaction is. We do as follows:

Mass of reactants = mass of products
11.00 + 44.55 = 51.04 + mass of carbon dioxide
mass of carbon dioxide = 4.51 g

8 0

3 years ago

A 5 gram round ball has a density of 1.25 grams/milliliter. What is the volume of the round ball?

Arlecino [84]

Explanation:

m=5g

density=1.25g/ml

density=m/v

v=m/density=5/1.25

4 0

3 years ago