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Kay [80]
3 years ago
7

What mass of ammonium thiocyanate must be used if it is to react completely with 6.5 g barium hydroxide octahydrate?

Chemistry
1 answer:
Molodets [167]3 years ago
6 0
<span>The reaction equation is:
Ba(OH)</span>₂<span>*8H</span>₂<span>O + 2NH</span>₄<span>SCN(s) </span>→<span> Ba(SCN)</span>₂<span>(s) + 10H</span>₂<span>O(l) + 2NH</span>₃<span> (g)

The molecular mass of barium hydroxide octahydrate is 315 grams /mol.
We determine the number of moles of barium hydroxide octahydrate:
moles = mass / Mr
moles = 6.5 / 315
moles = 0.02 mol

Using the equation, we can determine that the moles of ammonium thiocyanate required are:
2 * 0.02 = 0.04 mol

The molecular weight of ammonium thiocyanate is 76.1 grams / mol

Weight = moles * Mr
Weight = 0.04 * 76.1
Weight = 3.04 grams


3.04 grams of ammonium thicyanate are required.</span>
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What is the product of reduction of ethyl 4-oxobutanoate with sodium borohydride in ethanol at room temperature for 30 minutes?
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4 0
1 year ago
What is the pressure of 0.5 mol of nitrogen gas in a 5 L container at 203 K
vlada-n [284]

Answer:

=1.666 liters

Explanation:

1 mole of a has at standard temperature and pressure occupies a volume of 22.4 liters.

0.5 moles of nitrogen occupy a volume of (0.5 moles×22.4 dm³/mol)/ 1

=11.2 liters.

Standard pressure= 1 atmosphere (Atm)

Standard temperature = 273.15 Kelvin

According to Combined gas equation, P₁V₁/T₁=P₂V₂/T₂

Let us take the conditions under standard conditions as the reference, with the subscript 1 and the conditions under the 5L container to be scenario 2 with subscript 2.

Therefore P₂ =P₁V₁T₂/T₁V₂

Substituting for the values we get:

P₂= (1 atm× 11.2L ×203K)/ (273K×5L)

=1.666 atm

5 0
3 years ago
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