Nitrogen and hydrogen combine to form ammonia via the following reaction: 1 N 2 (s) + 3 H 2 (g) → 2 NH 3 (g) What mass of nitrogen is required to completely react with 800.0 mL H 2 at STP?

Here in this practice question, it says, nitrogen and hydrogen combined to form ammonia via the following reaction. Here we have 1 mole of nitrogen solid plus 3 moles of hydrogen gas combining to form 2 moles of ammonia gas. Here we're told what mass of nitrogen is required to completely react with 800 milliliters h 2 at s t p. So they want us to find the grams of n 2. And the information they give to us, they give us the volume, temperature, and pressure of h 2. Thinking about the ideal gas law, p v equals nrt, divide both sides by r t, we're gonna see here that moles equals p v over r t. At s t p our pressure is 1 atmosphere, our volume is 0.800 liters, r is 0.08206 liters times atmospheres over moles times k. Our temperature is 273.15 Kelvin. When we do this we'll get the moles of h two gas, so that comes out to be 0.03569 moles of h two gas. Realize now since we know the moles of h two gas, we can use stoichiometry to find the moles of n 2. So we're gonna say here 0.03569 moles h 2. We're gonna go from moles of h 2 to moles of n 2. So we're gonna do a mole to mole comparison. So for every 3 moles of h 2, there's 1 mole of n 2. So moles h 2 go on the bottom, moles n 2 go on top, and then finally, we're gonna say for every 1 mole of n 2, it weighs 28.02 grams. That's the combined mass of both nitrogens found from the periodic table. So when we plug that in, we get 0.33 0 grams of n 2. Here our final answer has 4 sig figs because 800 has 4 sig figs. So this would be the final act that we get for the mass of nitrogen gas based on the given information.

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1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
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5. Classification & Balancing of Chemical Reactions3h 17m
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8. Gases, Liquids and Solids

Standard Temperature and Pressure

GOB Chemistry

8. Gases, Liquids and Solids

Standard Temperature and Pressure

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Multiple Choice

Nitrogen and hydrogen combine to form ammonia via the following reaction:

1 N₂ (s) + 3 H₂ (g) → 2 NH₃ (g)

What mass of nitrogen is required to completely react with 800.0 mL H₂at STP?

0.333 g

0.512 g

0.802 g

1.01 g

1.36 g

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Verified step by step guidance

First, understand the stoichiometry of the reaction: 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. This means the molar ratio of N2 to H2 is 1:3.

Next, recall that at STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters. Convert the volume of H2 from milliliters to liters: 800.0 mL = 0.800 L.

Calculate the number of moles of H2 using the volume at STP: \( \text{moles of } H_2 = \frac{0.800 \text{ L}}{22.4 \text{ L/mol}} \).

Using the stoichiometric ratio from the balanced equation, determine the moles of N2 required: \( \text{moles of } N_2 = \frac{1}{3} \times \text{moles of } H_2 \).

Finally, calculate the mass of nitrogen needed using its molar mass (28.02 g/mol): \( \text{mass of } N_2 = \text{moles of } N_2 \times 28.02 \text{ g/mol} \).