What is number one I need help

The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In t

const2013 [10]

Answer:

$\boxed{\text{47.4 g}}$

Explanation:

We are given the mass of two reactants, so this is a limiting reactant problem.

We know that we will need mases, moles, and molar masses, so, let's assemble all the data in one place, with molar masses above the formulas and masses below them.

M_r: 17.03 32.00 18.02

4NH₃ + 5O₂ ⟶ 4NO + 6H₂O

m/g: 70.1 70.1

Step 1. Calculate the moles of each reactant

$\text{Moles of CO } = \text{70.1 g} \times \dfrac{\text{1 mol}}{\text{17.03 g}} = \text{4.116 mol}\\\\\text{Moles of H$_{2}$O} = \text{70.1 g} \times \dfrac{\text{1 mol}}{\text{32.00 g}} = \text{2.191 mol}$

Step 2. Identify the limiting reactant

Calculate the moles of H₂O we can obtain from each reactant.

From NH₃:

The molar ratio of H₂O:NH₃ is 6:4.

$\text{Moles of H$_{2}$O} = \text{4.116 mol NH$_{3}$} \times \dfrac{\text{6 mol H$_{2}$O}}{\text{4 mol NH$_{3}$}} = \text{6.174 mol H$_{2}$O}$

From O₂:

The molar ratio of H₂O:O₂ is 6:5.

$\text{Moles of H$_{2}$O} = \text{2.191 mol O$_{2}$} \times \dfrac{\text{6 mol H$_{2}$O}}{\text{5 mol O$_{2}$}} = \text{2.629 mol H$_{2}$O}$

O₂ is the limiting reactant because it gives the smaller amount of H₂O.

Step 3. Calculate the theoretical yield.

$\text{Theor. yield } = \text{2.629 mol H$_{2}$O}\times \dfrac{\text{18.02 g H$_{2}$O}}{\text{1 mol H$_{2}$O}} = \textbf{47.4 g H$_{2}$O}\\\\\text{The maximum yield of H$_{2}$O is }\boxed{\textbf{47.4 g}}$

6 0

3 years ago

Marshall determines that a gas has a gage pressure of 276 kPa what's the absolute pressure of this gas

Wittaler [7]

To determine the absolute pressure of this gas, all you need to do is to add the value of atmospheric pressure and the value of gage pressure.

Atmospheric pressure is equivalent to 100 kPa.
Gage pressure is 276 kPa.

Then, we add both values.

N = 100 kPa + 276 kPa
N = 376 kPa

The absolute pressure of this gas is 376 kPa.

Hope this helps :)

3 0

3 years ago

Read 2 more answers

3Al + 3NH4ClO4 → Al2O3 + AlCl3 + 3NO + 6H2O<br> How many moles of AlCl3 are produced?

zhuklara [117]

Answer: 1 mol of $AlCl_3$ will be produced from this reaction.

Explanation: Reaction follows,

$3Al+3NH_4ClO_4\rightarrow Al_2O_3+AlCl_3+3NO+6H_2Oc$

As seen from the balanced chemical equation above, we get

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 1 mole of $Al_2O_3$ is formed.

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 1 mole of $AlCl_3$ is formed.

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 3 moles of $NO$ is formed.

For every 3 moles of Aluminium and 3 moles of $NH_4ClO_4$ , 6 moles of $H_2O$ is formed.

7 0

3 years ago

Read 3 more answers

What is the molecular shape of hydrogen?

anzhelika [568]

The eletron pairs repel each other in a tetrahedral shape.

3 0

3 years ago

Assume the solubility of benzoic acid in ice-cold water is 1.70 g/L and the solubility of benzoic acid in hot water is 68.0 g/L.

lana [24]

Answer:

The volume of water needed to recrystallize 0.700 g of benzoic acid is 10.29 mL.

Explanation:

For the complete recrystalization,

the amount of hot water should be such that, the benzoic acid is completely soluble in it.

As we are given that the solubility of benzoic acid in hot water is 68.0 g/L. Now we have to determine the volume of water is needed to recrystallize 0.700 g of benzoic acid.

we conclude that,

As, 68.0 grams of benzoic acid soluble in 1 L of water.

So, 0.700 grams of benzoic acid soluble in of water.

The volume of water needed = 0.01029 L = 10.29 mL

conversion used : (1 L = 1000 mL)

Therefore, the volume of water needed to recrystallize 0.700 g of benzoic acid is 10.29 mL.

4 0

3 years ago