Chemistry: How many grams of Ammonia (NH3) are needed to completely react with 50 grams of sulfric acid (H2SO4)?

How many grams of Ammonia (NH3) are needed to, №14319276, 21.01.2023 10:28

Chemistry

Ammonia (NH3) is one of the most common chemicals produced in the united states. it is used to make fertilizer and other products. Ammonia is produced by the following chemical reaction. N2(g)+3h2(g)= 2nh3(g) If you have 1.00 x 10^3g of N2 a. If you have 1.00 x 10 g of N2 and 2.50 x 10 of H2, which is the limiting reactant in the reaction? b. How many grams of ammonia can be produced from the amount of limiting reactant available? c. Calculate the mass of excess reactant that remains after the reaction is complete.

Step-by-step answer

P Answered by PhD

3

a) N2 is the limiting reactant

b) 1215.9 grams NH3

c) 2283.6 grams H2

Explanation:

Step 1: Data given

Mass of N2 = 1000 grams

Molar mass N2 = 28 g/mol

Mass of H2 = 2500 grams

Molar mass H2 = 2.02 g/mol

Step 2: The balanced equation

N2(g) +3H2(g) → 2NH3(g)

Step 3: Calculate moles N2

Moles N2 = mass N2 / molar mass N2

Moles N2 = 1000 grams / 28.0 g/mol

Moles N2 = 35.7 moles

Step 4: Calculate moles H2

Moles H2 = 2500 grams / 2.02 g/mol

Moles H2 = 1237.6 moles

Step 5: Calculate limiting reactant

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

N2 is the limiting reactant. There will be consumed 35.7 moles.

H2 is in excess. There will react 3*35.7 = 107.1 moles

There will remain 1237.6 - 107.1= 1130.5 moles H2

This is 1130.5 * 2.2 = 2283.6 grams H2

Step 6: Calculate moles NH3

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

For 35.7 moles N2 we'll have 2*35.7 = 71.4 moles NH3

Step 7: Calculate mass NH3

Mass NH3 = moles NH3 * molar mass NH3

Mass NH3 = 71.4 moles * 17.03 g/mol

Mass NH3 = 1215.9 grams NH3

Chemistry

Ammonia (NH3) is one of the most common chemicals produced in the united states. it is used to make fertilizer and other products. Ammonia is produced by the following chemical reaction. N2(g)+3h2(g)= 2nh3(g) If you have 1.00 x 10^3g of N2 a. If you have 1.00 x 10 g of N2 and 2.50 x 10 of H2, which is the limiting reactant in the reaction? b. How many grams of ammonia can be produced from the amount of limiting reactant available? c. Calculate the mass of excess reactant that remains after the reaction is complete.

Step-by-step answer

P Answered by PhD

3

a) N2 is the limiting reactant

b) 1215.9 grams NH3

c) 2283.6 grams H2

Explanation:

Step 1: Data given

Mass of N2 = 1000 grams

Molar mass N2 = 28 g/mol

Mass of H2 = 2500 grams

Molar mass H2 = 2.02 g/mol

Step 2: The balanced equation

N2(g) +3H2(g) → 2NH3(g)

Step 3: Calculate moles N2

Moles N2 = mass N2 / molar mass N2

Moles N2 = 1000 grams / 28.0 g/mol

Moles N2 = 35.7 moles

Step 4: Calculate moles H2

Moles H2 = 2500 grams / 2.02 g/mol

Moles H2 = 1237.6 moles

Step 5: Calculate limiting reactant

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

N2 is the limiting reactant. There will be consumed 35.7 moles.

H2 is in excess. There will react 3*35.7 = 107.1 moles

There will remain 1237.6 - 107.1= 1130.5 moles H2

This is 1130.5 * 2.2 = 2283.6 grams H2

Step 6: Calculate moles NH3

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

For 35.7 moles N2 we'll have 2*35.7 = 71.4 moles NH3

Step 7: Calculate mass NH3

Mass NH3 = moles NH3 * molar mass NH3

Mass NH3 = 71.4 moles * 17.03 g/mol

Mass NH3 = 1215.9 grams NH3

Chemistry

One mole of zinc has a mass of 65.4 grams. Approximately how many atoms of zinc are present in one mole of zinc? (5 points) a 32 x 1023 atoms b 6 x 1023 atoms c 66 atoms d 65 atoms Question 2 (5 points) (05.01 LC) Which of the following best defines Avogadro s number? (5 points) a Mass, in grams, of each particle of the substance b Number of particles in one mole of a pure substance c Mass, in grams, of the nucleus of the substance s atoms d Total mass, in grams, of all the particles in one mole of the substance Question 3 (5 points) (05.01 MC)

Step-by-step answer

P Answered by PhD

1) Answer: b. 6 x 1023 atoms
1 mole of a substance is 6*10^23 atoms (Avogadro number) and the ratio of the mass of zinc to the molar mass is 1:1.
2) Answer: b
Number of particles in one mole of a pure substance
3) Answer: b
2.408 x 1024
Explanation: let's find the amount of substance
n=m/M=97.22 g/24g / mol= 4.05 mol
let's find the number of atoms
N=n*Na=4,05*6,02*10²³=24,08*10²³
4) Answer: c
molar mass of N + 3 x molar mass of H
Explanation: In order to calculate the molar mass of a compound (complex substance), the index indicating the number of atoms of each element in one mole should be multiplied by the molar mass of this element and the data obtained should be added.
5) Answer: b. 3
Explanation: Molar mass of mgco3 = 84.3139 g/mol.
n=m/M= 252,939 / 84,3139 = 3
6) Answer: a
Write the mole ratio.
7) Answer: b
15.1 grams
Explanation: Molar mass of Na2CO3 = 105.99 g/mol
n(Na2CO3) = 20 / 105,99 = 0,188
n(NaOH)=2n(Na2CO3)=2*0,188=0,376
m(NaOH)=0,376*40=15.1 grams
8) Answer: b
4.2 moles
Explanation: 2С2Н6+7О2=4СО2+6Н2О
3n(С2Н6)=n(H2O)
n(H2O)= 1,4*3=4,2
9) Answer: b
The ratio of measured yield over theoretical yield
10) Answer: c
87.3%
Explanation: 2,72 / 3,12 × 100% = 87,3 %
11) Answer: 145,314 g
Explanation: 61,33 / 22,9898 = 2,7
M (NaCl) = 58.5 g/mol
m(NaCl) = 2,7 × 58,5 = 157,95 g - the theoretical yield
the percentage yield of the reaction is 157,95*0.92=145,314 g

Chemistry

When nitrogen gas (N2) reacts with hydrogen gas(H) ammonia gas (NH3) is formed. How many grams of hydrogen gas are required to react completely with 3.5 L of nitrogen at STP? Show your work for full credit.

Step-by-step answer

P Answered by PhD

Mass of Hydrogen gas required to react : 0.936 g

Further explanation

Reaction on Nitrogen gas and Hydrogen gas to produce Ammonia gas

N₂ (g) + 3 H₂ (g) ⇒ 2 NH₃ (g)

Conditions at T 0 ° C and P 1 atm are stated by STP (Standard Temperature and Pressure). At STP, Vm is 22.4 liters / mol

so mol Nitrogen for 3.5 L at STP :

$\tt mol=\dfrac{3.5~L}{22.4~L}=0.156$

From the equation, mol ratio of N₂ : H₂ = 1 : 3, so mol H₂ :

$\tt \dfrac{3}{1}\times 0.156=0.468$

then mass of Hydrogen(MW= 2 g/mol) :

$\tt mass=mol\times MW\\\\mass=0.468\times 2\\\\mass=0.936~g$

Chemistry

How many moles of HF are in 30.mL of 0.15MHF(aq) ?

Step-by-step answer

P Answered by Master

Answer: 0.0045 mol
Explanation: Convert 30 ml to l: 30 mL = 0.03 L
Molarity = mol/l
mol = molarity * L
mol = 0.15 * 0.03 = 0.0045 mol
Answer: 0.0045 mol
Explanation: Convert 30 ml to l: 30 mL = 0.03 L
Molarity = mol/l
mol = molarit

Chemistry

LaToya uses 50 newtons (N) of force to pull a 500 N cart. Which statements are correct about calculating LaToya s mechanical advantage? Select all that apply.A. The input force is 50 N.B. The output force is 50 N.C. The input force is 500 N.D. The output force is 450 N.E. The mechanical advantage is 10.F. The mechanical advantage is 100.

Step-by-step answer

P Answered by Master

Answer:

A

Step-by-step explanation:

The input force is 50 N. But it will not create not any change. No mechanical advantage is observed.

Chemistry

Fiona claims that the diagram below shows simple machines, but Chad claims that it shows a compound machine. A man pushes a shopping cart up a ramp. Which statement best explains who is correct? Fiona is correct because less than three machines are shown in the diagram. Fiona is correct because the diagram shows two individual simple machines. Chad is correct because more than one machine is shown in the diagram. Chad is correct because the diagram shows two simple machines doing a job.

Step-by-step answer

P Answered by Specialist

Answer: b. Fiona is correct because the diagram shows two individual simple machines.

Explanation:
A mechanical device using which we can change the direction or magnitude of force applied is known as simple machine.
For example, in the given diagram there are two individual simple machines.
The machine helps in changing the direction or magnitude of force applied by the man. As a result, it becomes easy for him to carry different things easily from one place to another.
Thus, we can conclude that the statement Fiona is correct because the diagram shows two individual simple machines, is correct.
Answer: b. Fiona is correct because the diagram shows two individual simple machines.

Explanation

Chemistry

Based on the equation, how many grams of Br2 are required to react completely with 29.2 grams of AlCl3 (5 points)? 2AlCl3 + 3Br2 → 2AlBr3 + 3Cl2

Step-by-step answer

P Answered by PhD

1

Answer:

52.6 gram

Step-by-step explanation:

It is clear by the equation 2(27+3×35.5)= 267 gm of AlCl3 reacts with 6× 80 = 480 gm of Br2 . So 29.2 gm reacts = 480× 29.2/267= 52.6 gm

Chemistry

Which of the following will have a lower ionization energy than scandium

Step-by-step answer

P Answered by Master

Calcium (Ca)(On the periodic table, ionization energy increases as you go up and to the right of the periodic table)

Chemistry

what is the volume of a container that contains 24.0 grams of N2 gas st 328K and .884 atm?

Step-by-step answer

P Answered by PhD

Answer:

Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances.

Explanation:

In this case, you know:

P= 0.884 atm

V= ?

n= Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N 0.857 moles (where 28 g/mole is the molar mass of N₂, that is, the amount of mass that the substance contains in one mole.)

R=0.082 Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N

T= 328 K

Replacing in the ideal gas law:

0.884 atm×V= 0.857 moles× 0.082 Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N ×328 K

Solving:

Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N

V= 26.07 L

The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.

How many grams of Ammonia (NH3) are needed to completely react with 50 grams of sulfric acid (H2SO4)?

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