Use the following reaction to answer the question below:
3H2(g) + N2(g) → 2NH3(g)
Determine the number of molecules of ammonia made when 7.65 g of hydrogen gas reacts with excess nitrogen.
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Use the following reaction to answer the question below: 3H2(g) + N2(g) → 2NH3(g) Determine the...
Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) Calculate the mass of ammonia produced when 32.0 g of nitrogen react with 13.5 g of hydrogen. ___________NH3 Which is the excess reactant and how much of it will be left over when the reaction is complete? hydrogen or nitrogen ________ g
Question Ammonia is made from a rxn of nitrogen and hydrogen: N2(g)+3H2(g)--> 2NH3 a) What mass of the ammonia is made from 2000g of N2 and 1000 g of H2? b) What is the mass of the excess reactant?
Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How many moles of NH3 can be produced from 18.0 mol of H2 and excess N2? Express the number of moles to three significant figures
26.) Ammonia is produced by the reaction of hydrogen and nitrogen as follows: N2(g)+3H2(g)→2NH3(g)ammonia Express the number of moles to two significant figures. (A.) How many moles of H2 are needed to react with 1.0 mol of N2? (B.) How many moles of N2 reacted if 0.50 mol of NH3 is produced? (C.) How many moles of NH3 are produced when 1.7 mol of H2 reacts?
The Haber process for production of ammonia is as follows: N2 (g) + 3H2(g) → 2NH3 (g) An experiment ran this process using 5.75 moles of N2 and excess hydrogen gas. The reaction produced 7.50 moles of NH3. Calculate the percent yield for this experiment. Round your answer to the nearest whole number. Do not use scientific notation. Do not include the percent sign!
Consider for the following reaction N2 + 3H2—> 2NH3 What mass in grams of ammonia will be produced if 12.0g of hydrogen react completely with excess amount of nitrogen?
Armonía is manufactured using the following
reaction:
N2 + 3H2 ----- 2NH3
How much ammonia can be produced in the reaction of
2.04x10^-3 moles of nitrogen and 6.83x10^-3 moles of hydrogen?
Ammonia is manufactured using the following reaction: N2 + 3H2 - 2NH3. How much ammonia can be produced in the reaction of 2.04 x 10 moles of nitrogen and 6.83 x 10 moles of hydrogen?
Be sure to answer all parts. Consider the reaction N2(g) + 3H2(g) 2NH3(g) Suppose that at a particular moment during the reaction, molecular hydrogen is reacting at the rate of -0.087 M/s. (a) At what rate is ammonia being formed? M/s (b) At what rate is molecular nitrogen consumed? M/s
Nitrogen gas (N2) and hydrogen gas (H2) react to make ammonia gas (NH3) N2(g)+3H2(g)-->2NH3(g) you know tat this process gives a 55% yield for ammonia. Your job is to make 610g of ammonia. what mass of nitrogen do you need?
pts) The synthesis of ammonia from nitrogen and hydrogen is exothermic N2(g) + 3H2(g) → 2NH3(g) + Heat )If heat is removed, will the forward rate of the reaction increase or decrease? Why? ) If nitrogen gas is added, will the forward rate of the reaction increase or decrease? Why? If the volume of the reaction container is increased, how will this affect the rate of the forward reaction? Why? )