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ivolga24 [154]
1 year ago
14

How many grams are in 4 5 moles of sodium fluoride naf

Chemistry
1 answer:
nekit [7.7K]1 year ago
3 0

There are 618.68 g in 4.5 moles of NaF.

The total number of moles of any substance equals the ratio of its given mass in a chemical reaction to the mass of one mole or molar mass of that substance.

It is known that one mole of NaF or molar mass of NaF is 41.98 g/mol.

Given that number of moles is 4.5 moles.

Therefore, calculate the mass of NaF in grams as follows.

No. of moles = Given mass / Molar mass

mass in grams = No. of moles × Molar mass

                        = 4.5moles × 41.98 g/mol

                        = 188.91 g

Hence, we can conclude that there are 188.91 g in 4.5 moles of NaF.

Learn more about NaF from the link given below.

brainly.com/question/21321048

#SPJ4

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the pH of a solution is a measure of the acidity or alkalinity of a solution. Water has a pH of 7 and, in general, acids have a
Sliva [168]

Answer:

7.1

Explanation:

equation to calculate pH is

pH=-Log_{10}(a_{H^+})=-Log_{10}(8*10^-8) = -Log_{10}(8)-Log_{10}(10^{-8})=-0.9+8=7.1

6 0
3 years ago
what volume of co2 is produced at stp when 270g of glucose are consumed in the following reaction? c6h12o6 + 6o2(g) -> 6co2 (
lana [24]

Answer:

202 L

Explanation:

Step 1: Write the balanced equation

C₆H₁₂O₆ + 6 O₂(g) ⇒ 6 CO₂(g) + 6 H₂O(l)

Step 2: Calculate the moles corresponding to 270 g of C₆H₁₂O₆

The molar mass of C₆H₁₂O₆ is 180.16 g/mol.

270 g × 1 mol/180.16 g = 1.50 mol

Step 3: Calculate the moles of CO₂ generated from 1.50 moles of glucose

The molar ratio of C₆H₁₂O₆ to CO₂ is 1:6. The moles of CO₂ formed are 6/1 × 1.50 mol = 9.00 mol

Step 4: Calculate the volume of 9.00 moles of CO₂ at STP

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4 0
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All the substances listed below are fertilizers that contribute nitrogen to the soil.
kvv77 [185]

Answer:

Ammonia is the richest source of nitrogen on a mass percentage basis because it has 82.35% of nitrogen by mass.

Explanation:

Percentage of element in compound :

=\frac{\text{number of atoms}\times text{Atomic mass}}{\text{molar mas of compound}}\times 100

(a) Urea, (NH_2)_2CO

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(c) Nitric oxide, NO

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