2 pts

What substance is added to cordial to make it more dilute?

shusha [124]

The answer is water.

That is water is added to cordial to make it more dilute.

Cordial is basically used to describe sweeter distilled spirits . Or it can be used to describe non-alcoholic drink. These drinks can be diluted using water.

So the answer is water, that is water is added to cordial to make it more dilute.

7 0

3 years ago

What type of habitat does an animal that lives in trees inhabit

Lostsunrise [7]

That would be a bark habitat, love!

8 0

3 years ago

Read 2 more answers

How many molecules of F2 react with 66.6 g NH3 ? (stoichiometry)

stiks02 [169]

<h3>Answer:</h3>

5.89 × 10^23 molecules of F₂

<h3>Explanation:</h3>

The equation for the reaction between fluorine (F₂) and ammonia (NH₃) is given by;

5F₂ + 2NH₃ → N₂F₄ + 6 HF

We are given 66.6 g NH₃

We are required to determine the number of fluorine molecules

<h3>Step 1: Moles of Ammonia </h3>

Moles = Mass ÷ Molar mass

Molar mass of ammonia = 17.031 g/mol

Moles of NH₃ = 66.6 g ÷ 17.031 g/mol

= 3.911 moles

<h3>Step 2: Moles of Fluorine </h3>

From the equation 5 moles of Fluorine reacts with 2 moles of ammonia

Therefore,

Moles of fluorine = Moles of Ammonia × 5/2

= 3.911 moles × 5/2

= 9.778 moles

<h3>Step 3: Number of molecules of fluorine </h3>

We know that 1 mole of a compound contains number of molecules equivalent to the Avogadro's number, 6.022 × 10^23 molecules

Therefore;

1 mole of F₂ = 6.022 × 10^23 molecules

Thus,

9.778 moles of F₂ = 9.778 moles × 6.022 × 10^23 molecules/mole

= 5.89 × 10^23 molecules

Therefore, the number of fluorine molecules needed is 5.89 × 10^23 molecules

5 0

3 years ago

Gaseous butane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . If of water is produced from

krek1111 [17]

The given question is incomplete. The complete question is :

Gaseous butane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . If 1.31g of water is produced from the reaction of 4.65g of butane and 10.8g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.

Answer: 28.0 %

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of butane}=\frac{4.65g}{58g/mol}=0.080moles$

$\text{Moles of oxygen}=\frac{10.8g}{32g/mol}=0.34moles$

$2C_4H_{10}(g)+13O_2(g)\rightarrow 8CO_2(g)+10H_2O(g)$

According to stoichiometry :

13 moles of $O_2$ require 2 moles of butane

Thus 0.34 moles of $O_2$ will require= $\frac{2}{13}\times 0.34=0.052moles$ of butane

Thus $O_2$ is the limiting reagent as it limits the formation of product and butane is the excess reagent.

As 13 moles of $O_2$ give = 10 moles of $H_2O$

Thus 0.34 moles of $O_2$ give = $\frac{10}{13}\times 0.34=0.26moles$ of $H_2O$

Mass of $H_2O=moles\times {\text {Molar mass}}=0.26moles\times 18g/mol=4.68g$

${\text {percentage yield}}=\frac{\text {Experimental yield}}{\text {Theoretical yield}}\times 100\%$

${\text {percentage yield}}=\frac{1.31g}{4.68g}\times 100\%=28.0\%$

The percent yield of water is 28.0 %

6 0

4 years ago

One cup of fresh orange juice contains 115 mg of ascorbic acid (vitamin c, c6h8o6). given that one cup

kodGreya [7K]

The question is incomplete. Complete question is read as:
'<span>One cup of fresh orange juice contains 115 mg of ascorbic acid (vitamin C, C6H8O6). Given that one cup = 218.0 mL calculate the molarity of vitamin C in organic juice.'
..........................................................................................................................
Answer:
Given: weight of solute (ascorbic acid) = 115 mg = 0.115 g
Volume of solution = 218.0 mL = 0.218 L
Molecular weight of ascorbic acid = 176.12 g/mol.

Now, Molarity = </span> $\frac{\text{weight of solute(g)}}{\text{Molecular weight X Vol. of solution(l)}}$
= $\frac{\text{0.115}}{\text{176.12 X 0.218}}$
<span> = 0.002995 mol/dm3

Answer: Molarity of solution = </span>0.002995 mol/dm3<span>

</span>

4 0

3 years ago