Answer:
John Dalton's Atomic Model Below ⬇
Explanation:
What volume of 1.75 h2so4 would be needed to neutralize 350 ml of 3.33 m sodium hydroxide?
1 answer:
Answer:
1.332 L
Explanation:
The reaction that takes place is:
- H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O
First we <u>calculate the number of NaOH moles</u>, using the <em>given volume and concentration</em>:
- 350 mL * 3.33 M = 1165.5 mmol NaOH
Then we <u>convert NaOH moles into H₂SO₄ moles</u>, using the <em>stoichiometric coefficients</em>:
- 1165.5 mmol NaOH *
= 2331 mmol H₂SO₄
Finally we <u>calculate the required volume of a 1.75 M solution of H₂SO₄</u>, using the<em> concentration and number of moles:</em>
- 2331 mmol / 1.75 M = 1332 mL
We can <u>convert mL into L</u>:
- 1332 mL / 1000 = 1.332 L
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Complete Question:
An iron atom has a mass of 9.27*(10)⁻²³ g and a cooking pot has a mass of 0.500 kg.
Use this information to answer the questions below:
1) What is the mass of 1 mole of iron atoms? Round your answer to 3 significant digits.
The mass of 1 mole of iron atoms is 55.8 g
Why?
The key to solve this question is the use of the Avogadro's Number (NA). This number tells us the amount of atoms found in 1 mole of a substance. So, to find the mass of 1 mole of iron atoms, we're actually finding the mass of 6.022 x 10²³ atoms.
The equation we are going to use to find the mass is shown below:
2) How many moles of iron atoms have a mass equal to the mass of a cooking pot? Round your answer to 3 significant digits.
The moles of iron atoms that have a mass equal to the mass of a cooking pot is 8.96 moles
Why?
In this case, we are also going to use the mass of the cooking pot. We have to find first how many atoms are there in the cooking pot, and then we will find how many moles are represented by that mole of atoms:
Atoms in the cooking pot:
Moles in the cooking pot:
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A sample of an ideal gas has a volume of 2.30 L at 281 K and 1.02 atm. 1.76 atm is the pressure when the volume is 1.41 L and the temperature is 298 K.
<h3>What is Combined Gas Law ?</h3>This law combined the three gas laws that is (i) Charle's Law (ii) Gay-Lussac's Law and (iii) Boyle's law.
It is expressed as
where,
P₁ = first pressure
P₂ = second pressure
V₁ = first volume
V₂ = second volume
T₁ = first temperature
T₂ = second temperature
Now put the values in above expression we get
P₂ = 1.76 atm
Thus from the above conclusion we can say that A sample of an ideal gas has a volume of 2.30 L at 281 K and 1.02 atm. 1.76 atm is the pressure when the volume is 1.41 L and the temperature is 298 K.
Learn more about the Combined gas Law here: brainly.com/question/13538773
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