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solong [7]
3 years ago
9

Suppose 215 g of NO3- flows into a swamp each day. What volume of CO2 would be produced each day at 17.0°C and 1.00 atm?

Chemistry
1 answer:
charle [14.2K]3 years ago
8 0

Answer:

The answer is "41.23 \ L\  N_2"

Explanation:

2 NO_3^{-} + 10 e^{-} + 12 H^{+} \longrightarrow N_2 + 6 H_2O\\\\= \frac{( 215 \ g \ NO_3^{-})}{(62.0049  \frac{\ g NO_3^{-}}{mol})} \times  \frac{(1 \ mol \ N_2}{ 2 \ mol \ NO_3^{-})}\\\\

=3.46746789 \times 0.5\\\\= 1.733 \ mol \ N_2 \\\\\to V = \frac{nRT}{P} \\\\= (1.733 \ mol) \times (0.08205746 \frac{L\ atm}{Kmol}) \times \frac{ (17 + 273) K}{(1.00 atm)}\\\\= 41.23

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A gas is collected at 30 Celsius and has a pressure of 200 kPa. What pressure would it exert if the temperature changed to 40 Ce
garik1379 [7]

Answer:

206.6\ \text{kPa}

Explanation:

P_1 = Initial pressure = 200 kPa

P_2 = Final pressure

T_1 = Initial temperature = 30^{\circ}\text{C}

T_2 = Final temperature = 40^{\circ}\text{C}

We have the relation

\dfrac{P_2}{P_1}=\dfrac{T_2}{T_1}\\\Rightarrow P_2=\dfrac{T_2}{T_1}P_1\\\Rightarrow P_2=\dfrac{40+273.15}{30+273.15}\times 200\\\Rightarrow P_2=206.6\ \text{kPa}

The pressure that would be exerted after the temperature change is 206.6\ \text{kPa}.

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2 years ago
A physician has ordered 0.50 mg of atropine, intramuscularly. If atropine were available as 0.25 mg/mL of solution, how many mil
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