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How many grams of ammonia can be made by reacting 100 g of N2 with 20 g of ? What is the limiting reactant? How much of the excess reactant will be left over? N2(g) + 3H2(g) → 2NH3(g)
Molar mass of N2 = 28.0134100/28.0134 = 3.57molesMolar ratio of N2:NH3 = 1:23.57 × 2 = 7.14moles of NH3Molar mass of H2 = 2.01620/2.016 = 9.92molesMole ratio of H2:NH3 =...
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How many moles of ammonia are produced when 0.60 moles of nitrogen reacts with hydrogen? N2(g) + 3H2(g) => 2NH3(g)
=1.2moles of Ammonia
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If 54.0 grams of water are mixed with excess magnesium nitride, How many grams of ammonia (NH₃) are produced? Mg₃N₂ + 6H₂O --> 2NH₃ + 3Mg(OH)₂
Grams of ammonia (NH₃) produced=17.0g
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Nitrogen gas reacts with hydrogen gas to produce ammonia.
N2(g)+3H2(g)→2NH3(g)
How many grams of H2 are needed to react with 3.40 g of N2?
Thanks for your help!!
The balanced chemical eqiation is N2(g)+3H2(g)→2NH3(g) The mass of nitrogen is m(N2) = 3.40 g The amount of nitrogen is n(N2) = m(N2)/M(N2[]/sub) = 3.4/28.013 = 0.121 mol The reacion...
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Nitrogen and hydrogen combine at high temperature in the presence of a catalyst to produce ammonia assume .240 mol of N2 and .746 mol of H2 are present initially. N2(g)+3H2(g)—>2NH3(g)
Solution The nitrogen would react completely with 0.240 mol N2 (3 mol H2/1 mol N2) = 0.720 mol H2, producing ammonia in amount 0.240 mol N2 (2 mol NH3/1 mol...
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How many moles of NH3 can be produced from 3.76 moles of nitrogen in the following reaction: N2(g)+3H2(g)=>2NH3(g)
n(NH3)=n(N2)*2=3.76*2=7.52 moles(based on chemical reaction rates)
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N2 + 3H2= 2NH3
If a sample of 3 mole of hydrogen gas (H2) was reacted, how many miles of ammonia (NH3) gas would be produced ?
Solution:The equation of a chemical reaction:N2 + 3H2= 2NH3 According to the chemical equation: n(N2) = n(H2)/3 = n(NH3)/2.Consequently,n(H2)/3 = n(NH3)/2;n(NH3) = 2 * n(H2) / 3;n(NH3) = (2 * 3)...
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Nitrogen dioxide reacts with water to produce oxygen and ammonia:
4NO2(g)+6H2O(g)→7O2(g)+4NH3(g). How many grams of NH3 can be produced when 4.50 L of NO2 reacts at 435 ∘C and 695 mmHg ?
pV=nRT. n=pV/RT = 695 x 4500 / 62400 x 708= 0,0707912321 moles.0,0707912321 x 17 = 1,20345095 g.
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Consider the following reaction.
N2(g) + 3H2(g) ⭢ 2NH3(g)
If the rate of loss of hydrogen gas is 0.03mol L-1 s-1, what is the rate of production of ammonia?
Given reaction is N2(g) + 3H2(g) ––> 2NH3(g) If the reaction rate = r Then according to the above stoichiometric equation, Rate of reaction, r = –(d[H2]/dt) = (d[NH3]/dt)...
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when nitrogen gas reacts with hydrogen gas,ammonia gas is formed.How many grams of hydrogen gas are required to react completely with 3,5 L of nitrogen at STP?
Solution:A chemical equation must be balanced:N2 + 3H2 = 2NH3According to the reaction equation for 3 mol of H2 is needed 1 moles of N2.Therefore, mass of H2 = V...
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