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$Na_3N$ decomposes to form sodium and nitrogen gas at STP. If 13.7 L of nitrogen is produced, how many moles of $Na_3N$ was used (22.4 L = 1 mole of any gas) ?
Given: $Na_3N$ decomposes to form sodium (Na) and Nitrogen ($N_2)$ at STP (standard temperature and pressure). At STP $22.4 L = 1$ mole of gas First you need to write...
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Under certain conditions of temperature and pressure, hydrogen gas and nitrogen gas react to form ammonia gas. Determine the mass of ammonia produced if 3.50 moles of hydrogen has reacts with 5.00 moles of nitrogen gas?
Start by balancing the equation for the reaction between hydrogen $"H"_2$ and nitrogen $"N"_2$, which produces ammonia $"NH"_3$: $color(darkgreen)(1) color(white)(.) "N"_2 (g) + color(darkgreen)(3) color(white)(.) "H"_2 to color(darkgreen)(2) color(white)(.) "NH"_3...
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Calculate the volume of ammonia gas produced at STP when 140g of nitrogen gas reacts with 30g of hydrogen gas.(atomic mass: N=14u,H=1u) how to do this?
Simply, the reaction is $N_2+3H_2=2NH_3$ $140g$ $"N"_2$ means $140/28=5$ mol; $30g$ $H_2$ means $30/2=15$mol From 1 mol of $N_2$ 2 mol $NH_3$ is prepared in perfect presence of $H_2$...
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When an airbag is inflated the nitrogen gas has a pressure of 1.30 atmospheres, a temperature of 301 K, and a volume of 40.0 liters. What is the volume of the nitrogen at STP?
You can actually use two approaches to solve this problem. You can use the to find the number of moles of gas present in that sample, then use...
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Using the molar volume of a gas at STP , what is the volume (in L) occupied by 36.2 g of neon at STP?
STP is defined as 1 bar and 0 °C. The molar volume at STP is 22.71 L/mol. $"Moles of Ne" = 36.2 color(red)(cancel(color(black)("g Ne"))) × "1 mol Ne"/(20.18 color(red)(cancel(color(black)("g...
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How do you use the molar volume gas at STP to determine the volume (in L) of a occupied by 33.6 g of neon at STP?
So neon occupies 33.6 g First we find the number of moles of Ne= $(mass)/"molar mass"$ No. of moles= $(33.6)/"20"$ No. of moles= 1.68 mol Then, we can find volume...
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Ammonia gas decomposes according to the equation: $2NH_3(g) -> N_2(g) + 3H_2(g)$. If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?
The thing to remember about reactions that involve gases held under the same conditions for pressure and temperature is that the mole ratio that exists between the gaseous in the...
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Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200°C in a closed container, 1.05 atm of nitrogen gas is mixed with 2.02 atm of hydrogen gas. At equilibrium the total pressure is 2.02 atm. What is the partial pressure of hydrogen gas at equilibrium?
First, write the balanced chemical equation for the equilibrium and set up an ICE table. $color(white)(XXXXXX)"N"_2 color(white)(X)+color(white)(X)"3H"_2 color(white)(l)⇌ color(white)(l)"2NH"_3$ $"I/atm": color(white)(Xll)1.05 color(white)(XXXl)2.02 color(white)(XXXll)0$ $"C/atm": color(white)(X)-x color(white)(XXX)-3x color(white)(XX)+2x$ $"E/atm": color(white)(l)1.05- x...
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The total pressure is 600 mmHg after 0.50 moles of nitrogen gas, $N_2$, and 1.0 mole of nitrogen dioxide, $NO_2$, gas are mixed in a closed container. There is no reaction between the gases. What is the partial pressure of the nitrogen dioxide?
Old $"Dalton's Law of partial pressures"$ tells us that in a gaseous mixture, the exerted by a component gas is the same as the pressure it would exert if it...
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A sample of nitrogen gas has a volume of 32.4 L at 20°C. The gas is heated to 220°C at constant pressure. What is the final volume of nitrogen?
This is an example of which states that the volume of a gas held at constant pressure is directly proportional to the Kelvin temperature. The equation for Charles' law is...
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