Answer:
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Explanation:
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Answer : You can make 4.68 moles of SO₂
Explanation:
Step 1 : Write balanced equation.
S₈ can combine with oxygen to form SO₂ gas. The balanced equation for this reaction is written below.
Step 2 : Find moles of S₈
The formula to calculate mol is
Molar mass of S₈ is 256.5 g/mol
we have 0.585 mol of S₈
Step 3: Use mole ratio to find moles of SO₂
The mole ratio of S₈ and SO₂ can be found using balanced equation which is 1:8
That means 1 mol of S₈ can form 8 moles of SO₂.
Let us use this as a conversion factor to find moles of SO₂
Therefore we have 4.68 moles of SO₂
When a sample of a gas is heated in a sealed, rigid
container from 200 degree Kelvin to 400 degree Kelvin, the pressure exerted by
the gas is increased by a factor 2. Heating any gas actually increases the
volume of the gas within a container. As the temperature of the gas rises, the
molecules of the gas start moving faster and start striking the walls of the
container in which it is kept with more force. The volume of the container
tries to expand to accommodate the fast colliding molecules of the gas.
Answer: 20) 2365 g
21) 22.39 grams.
22) 29.99 g
Explanation: 20) molarity is the no of moles of solute per unit volume.
We can calculate amount of CaCl2 required to prepare 0.1 M CaCl2 1000 ml solution.
we know that to prepare one ltr of 1 M solution of CaCl2 111 g required
Now consider x gram will require to prepare to
so that comparing above both condition
1000ml ×1M×X g=1000ml×0.1M×111g
X= 11.1 gram
X= 11.1 g of CaCl2
Hence 11.1 g of CaCl2 would be dissolved in 1.0L of a 0.100 M solution of CaCl2
21) How many moles of CaCl₂ in that solution?
;
;
.
What's the mass of that 0.20172 moles of CaCl₂?
Molar mass from a modern periodic table:
Ca- 40.078;
Cl- 35.45.
Molar mass of CaCl₂:
.
Mass of that 0.20172 moles of CaCl₂:
22) its a 3.0m solution so 1 litre of solution contains 3 moles of NaOH, 250ml of solution contains 0.25x39.9971 g/mol, so 250ml of this solution contains 0.75x39.9971=29.99g, or if you round it up 30.0g
Answer:
<u>49.54 g</u>
Explanation:
Let's take the masses of both calcium sulfate and sulfur dioxide formed.
Sulfur dioxide = 32 + 2(16) = <u>64 g</u>
Calcium sulfate = 40 + 32 + 4(16) = <u>136 g</u>
So, under ideal conditions, to produce 136 g of Calcium sulfate, we require 64 g of Sulfur dioxide.
But, it mentions the process is only 95% efficient.
Hence, taking the ratio :
x = <u>49.54 g</u> (approximately)
