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Hoochie [10]
4 years ago
5

Scientists use this method to create plants that have higher nutritional values

Chemistry
1 answer:
tamaranim1 [39]4 years ago
7 0
They genetically modify them
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How many grams of NO are required to produce 145 g of N2 in the following reaction?
V125BC [204]

Answer:

b. 186 g

Explanation:

Step 1: Write the balanced equation.

4 NH₃(g) + 6 NO(g) → 5 N₂(g) + 6 H₂O(l)

Step 2: Calculate the moles corresponding to 145 g of N₂

The molar mass of nitrogen is 28.01 g/mol.

145g \times \frac{1mol}{28.01 g} =5.18 mol

Step 3: Calculate the moles of NO required to produce 5.18 moles of N₂

The molar ratio of NO to N₂ is 6:5.

5.18molN_2 \times \frac{6molNO}{5molN_2} = 6.22molNO

Step 4: Calculate the mass corresponding to 6.22 moles of NO

The molar mass of NO is 30.01 g/mol.

6.22mol \times \frac{30.01g}{mol} =186 g

4 0
3 years ago
Q1. Briefly explain why the Zeff experienced by a valence electron in Cl is larger than in Mg. Q2. Briefly explain why the Zeff
Inessa05 [86]

Answer:

See explanation

Explanation:

Q1:

Chlorine has 17 protons while magnesium has only 12 protons. Recall that the Zeff depends on the size of the nuclear charge. The greater the size of the nuclear charge, the larger the Zeff experienced by a valence electron.

Q2:

The larger the Zeff, the smaller the atomic radius. Since the valence electrons of Cl experience a greater Zeff than those of Mg due to greater size of the nuclear charge, the atomic radius of chlorine will be smaller than that of Mg.

Q3:

The radius of an atom increases as the value of the principal quantum number (n) increases down the group due to addition of more shells. The greater the number of shells added, the greater the principal quantum number (n) and the greater the atomic radius, hence the answer.

5 0
3 years ago
For the following reaction, KP = 0.455 at 945°C: At equilibrium, is 1.78 atm. What is the equilibrium partial pressure of CH4 in
Alborosie

Answer:

See explanation below

Explanation:

The question is incomplete. However, here's the missing part of the question:

<em>"For the following reaction, Kp = 0.455 at 945 °C: </em>

<em>C(s) + 2H2(g) <--> CH4(g). </em>

<em>At equilibrium the partial pressure of H2 is 1.78 atm. What is the equilibrium partial pressure of CH4(g)?"</em>

With these question, and knowing the value of equilibrium of this reaction we can calculate the partial pressure of CH4.

The expression of Kp for this reaction is:

Kp = PpCH4 / (PpH2)²

We know the value of Kp and pressure of hydrogen, so, let's solve for CH4:

PpCH4 = Kp * PpH2²

*: You should note that we don't use Carbon here, because it's solid, and solids and liquids do not contribute in the expression of equilibrium, mainly because their concentration is constant and near to 1.

Now solving for PpCH4:

PpCH4 = 0.455 * (1.78)²

<u><em>PpCH4 = 1.44 atm</em></u>

6 0
4 years ago
Products and reactants are used and created at the same rate when a reaction is at this stage
V125BC [204]

This means that the reaction is in dynamic equilibrium.

Hope this helps because I don't really know the question you asked :)))

7 0
4 years ago
Read 2 more answers
How many sulfur atoms are generated when 9.42 moles of H2S react according to the following equation: 2H2S+SO2→3S+2H2O
8_murik_8 [283]

Answer:

A) 8.51 × 10²⁴  

Explanation:

1. Gather all the information

            2H₂S + SO₂ ⟶ 3S + 2H₂O

n/mol:   9.42

2. Calculate the moles of S atoms

The molar ratio is 3 mol S:2 mol H₂S

\text{Moles of S} = \text{9.42 mol H$_{2}$S} \times \dfrac{\text{3 mol S }}{\text{2 mol H$_{2}$S }} = \text{14.13 mol S}

3. Calculate the atoms of S

\text{Atoms of S } = \text{14.13 mol S} \times \dfrac{6.022 \times 10^{23}\text{ S atoms}}{\text{1 mol S}} = \mathbf{8.51 \times 10^{24}}\textbf{ S atoms}

 

6 0
3 years ago
Read 2 more answers
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