Consider the equation: 2 nan3 (s) 2 na (s) + 3 n2. what is the mass of nan3 needed to produce 17.2 l nitrogen at stp?

1 answer:

3 0

The mass of NaN3 needed to produce 17.2 L nitrogen at STP is calculated as follows

find the moles of N2 produced at STP
At STP 1mole of gas = 22.4 L , what about 17.2 L of nitrogen

by cross multiplication

= (1 mole x17.2 L)/ 22.4 L= 0.768 moles

2NaN3 =2Na +3 N2
by use of mole ratio between NaN3 to N2 (2:3) the moles of NaN3 = 0.768 x2/3 = 0.512 moles of NaN3

mass of NaN3 is therefore =moles of NaN3 xmolar mass of NaN3

=0.512moles x 65 g/mol =33.28 grams of NaN3

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Draw the products of the acid-base reaction between stearic acid and OH-

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Products are stearate anion and water.

Explanation:

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When $OH^{-}$ is added into stearic acid, $OH^{-}$ removes a proton ( $H^{+}$ ) from acidic -COOH group and forms stearate anion and water as products.