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Alex_Xolod [135]
3 years ago
12

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N 2 (g) 3H 2 (g) 2NH3 (g) I

f the reaction yield is 87.5%, how many moles of N 2 are needed to produce 3.00 mol of NH 3
Chemistry
1 answer:
balandron [24]3 years ago
5 0

Answer:

We need 1.714 moles N2

Explanation:

Step 1: Data given

The reaction yield = 87.5 %

Number of moles NH3 produced = 3.00 moles

Step 2: The balanced equation

N2(g)+ 3H2(g) →2NH3(g)

Step 3: Calculate moles N2

For 2 moles NH3 produced we need 1 mol N2 and 3 moles H2

This means, if the yield was 100%, for 3.00 moles NH3 produced , we need 1.5 moles N2

For a 87.5 % yield:  

we need more N2, increased by a ratio of 100/87.5.

100/87.5 * 1.5 =  1.714 moles N2

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Thus, Ca(NO_{3})_{2} is correct answer.

5 0
3 years ago
Identify each substance as an acid or a base.
svp [43]

Explanation:

<u>The first one is a base</u>

<u>The second one is an acid</u>

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Hope I helped!!! Have a great day!

4 0
3 years ago
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8 0
3 years ago
A gas is at a pressure of 4.30 atm. what is this pressure in kilopascals? in mm hg?
Monica [59]
Units to measure pressure are as follows
atm - atmospheric pressure units
kPa - kilo Pascals
mm Hg - milimeters Hg
conversion units are;
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therefore 4.30 atm = 101 325 Pa / atm x 4.30 atm = 435.7 Pa

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answers are 435.7 Pa and 3268 mm Hg
5 0
3 years ago
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