The amount of gas that occupies 36.52 L at 68.0°C and 672 mm Hg is __________ mol.

Answers

Answer 1

Answer: We assume that this gas is an ideal gas. We use the ideal gas equation to calculate the amount of the gas in moles. It is expressed as:

PV = nRT
(672) (1/760) (36.52) = n (0.08206) ( 68 +273.15)
n = 1.15 mol of gas

Hope this answers the question. Have a nice day.

Related Questions

a length of #8 copper wire (radius = 1.63 mm) has a mass of 24.0 kg and a resistance of 2.061 ohm per km. what is the overall resistance of the wire
A chemist titrates 160.0mL of a 0.3403M aniline C6H5NH2 solution with 0.0501M HNO3 solution at 25°C . Calculate the pH at equivalence. The pKb of aniline is 4.87 . Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO3 solution added.
A cool, yellow-orange flame is used to heat the crucible. Would this affect the mass of the crucible? If so, how?
The federal limit for cadmium in drinking water is 0.010 mg per liter of solution. What is the molar concentration of a Cd solution that has reached the limit?
Identify which location in the periodic table you would have thelargest atomic radii.

What is the mass in grams of H₂ that can be formed from 54.6 grams of NH₃ in the following reaction?2 NH₃(g) → 3 H₂(g) + N₂(g)

Answers

9.6 grams of H₂ can be formed from 54.6 grams of NH₃ in the following reaction: 2NH₃(g) → 3H₂(g) + N₂(g).

According to this question, the following balanced equation is given: 2NH₃(g) → 3H₂(g) + N₂(g).

First, we convert the mass of ammonia (NH3) to moles as follows:

moles of NH3 = 54.6g ÷ 17g/mol

moles of NH3 = 3.2mol.

If 2 moles of NH3 produces 3 moles of H2.
3.2 moles of NH3 will produce 4.8 moles of H2.

Next, we convert 4.8moles of H2 to mass as follows:

mass of H2 = 4.8 × 2

mass of H2 = 9.6g of H2.

Therefore, 9.6 grams of H₂ can be formed from 54.6 grams of NH₃ in the following reaction: 2NH₃(g) → 3H₂(g) + N₂(g).

Learn more at: brainly.com/question/8732513?referrer=searchResults

Answer : The mass of $H_2$ is, 9.64 grams.

Explanation : Given,

Mass of $NH_3$ = 54.6 g

Molar mass of $NH_3$ = 17 g/mol

Molar mass of $H_2$ = 2 g/mol

First we have to calculate the moles of $NH_3$ .

$\text{Moles of }NH_3=\frac{\text{Given mass }NH_3}{\text{Molar mass }NH_3}$

$\text{Moles of }NH_3=(54.6g)/(17g/mol)=3.21mol$

Now we have to calculate the moles of $H_2$

The balanced chemical equation is:

$2NH_3(g)\rightarrow 3H_2(g)+N_2(g)$

From the balanced reaction we conclude that

As, 2 mole of $NH_3$ react to give 3 moles of $H_2$

So, 3.21 mole of $NH_3$ react to give $(3)/(2)* 3.21=4.82$ mole of $H_2$

Now we have to calculate the mass of $H_2$

$\text{ Mass of }H_2=\text{ Moles of }H_2* \text{ Molar mass of }H_2$

$\text{ Mass of }H_2=(4.82moles)* (2g/mole)=9.64g$

Therefore, the mass of $H_2$ is, 9.64 grams.

Weathering and erosion can turn metamorphic rock into sediment. Which of the following processes would turn that sediment into sedimentary rock? * 10 points weathering and erosion compaction and cementation heat and pressure melting

Answers

Answer:

compaction and cementation

Explanation:

sedimentary rock is layered rock, in order to become sedimentary it most be compacted to form layers and cemented to become hard. This is what i think. Hope i can help :)

PLZZZZZZZZZZZZ HELPPPPPPPPP BRAINLIEST FOR WHO GETS IT RIGHTTTTTTWhat is the mass of reactants in the following equation?N2 + 3H2 ----> 2NH3
Question 3 options:

34.05 amu

31.03 amu

30.02 amu

15.01 amu

Answers

Answer: 34.05

Explanation:

2N and 6H = abt 34

What is the correct equilibrium constant expression for the following reaction? 3A2 = 2B3 when the reaction started with the initial concentrations of A2 = 3 M and B3 = 2 M and continued until the equilibrium concentrations of A2 = 2.5 M and B3 = 2.5 M

Answers

Answer:

Kc = [B₃]²/[A₂]³ = 0.40

Explanation:

3A₂ ⇄ 2B₃

Given at equilibrium => [A₂] =2.5 and [B₃] = 2.5

Kc = [B₃]²/[A₂]³ = (2.5)²/(2.5)³ = (2.5)⁻¹ = 0.40

What type of matter do alloys fall under?a) Element
b) Compound
c) Heterogeneous mixture
d) Homogeneous mixture

Answers

An alloy, a metallic substance composed of two or more elements, as either a compound or a solution is a homogeneous mixture. The correct option is d.

What is an alloy?

An alloy is a mixture of chemical elements of which at least one is a metal. Unlike chemical compounds with metallic bases, an alloy will retain all the properties of metal in the resulting material, such as electrical conductivity, ductility, opacity, and lustre, but may have properties that differ from those of pure metals, such as increased strength or hardness.

In some cases, an alloy may reduce the overall cost of the material while preserving important properties. In other cases, the mixture imparts synergistic properties to the constituent metal elements such as corrosion resistance or mechanical strength. Alloys are defined by a metallic bonding character. The alloy constituents are usually measured by mass percentage for practical applications, and in atomic fraction for basic science studies.

Alloys are usually classified as substitutional or interstitial alloys, depending on the atomic arrangement that forms the alloy.

Learn more about alloy, here:

brainly.com/question/3718729

#SPJ6

Answer:

An alloy is a homogeneous mixture

Explanation:

Using a density of 1.0 g/mL for the water added and adding in the mass of the lithium nitrate, what is the total mass of the solution?

Answers

The total mass of the solution of lithiumnitrate solution has been 99.7 grams.

Density can be defined as the mass of the solute per unit volume. The density can be expressed as g/ml or kg/L.

The mass of given Lithium nitrate = 2.5 grams.

The mass of water can be given as:

Density = $\rm (Mass)/(Volume)$

Volume of water = 97.2 ml.

The total mass of solution:

Mass of water = Density $*$ Volume

Mass of water = 1 $*$ 97.2 grams

Mass of water = 97.2 grams

The total mass = Mass of lithium nitrate + mass of water

= 2.5 + 97.2 grams

= 99.7 grams.

The total mass of the solution of lithiumnitrate solution has been 99.7 grams.

For more information about density, refer to the link:

brainly.com/question/14940265

Answer:

The total mass of the solution = 99.7 g

Note: The question is incomplete. The complete question is given below:

A "coffee-cup" calorimetry experiment is run for the dissolution of 2.5 g of lithium nitrate placed into 97.2 mL of water. The temperature of the solution is initially at 23.5oC. After the reaction takes place, the temperature of the solution is 28.3 oC.

1. Using a density of 1.0 g/mL for the water added and adding in the mass of the lithium nitrate, what is the total mass of the solution and solid?

Explanation:

mass = density * volume

density of water = 1.0 g/mL; volume of water = 97.2 mL

mass of water = 1.0 g/L * 97.2 mL

mass of water = 97.2 g

mass of lithium nitrate = 2.5 g

A solution is made by dissolving a solute (usually solid) in a solvent (usually a liquid). The solute in this reaction is lithium nitrate and the solvent is water.

Total mass of solution = mass of water + mass of lithium nitrate

Total mass of solution = 97.2 g + 2.5 g = 99.7 g

Therefore, total mass of the solution = 99.7 g

Other Questions

What is colloidal solutions

Which is the limiting reactant when 5.00g of H2 and 10.00g of O2 react and form water?

Which two structures will provide a positive identification of a plant cell under a microscope? A.) Lysosomes, cell wall. B.) large central vacuole, cell wall. C.) large central vacuole ribosomes. D.)nucleoid, chloroplasts.

The correct electron configuration for magnesium is: 1s 22s 22p 63s 3 True False