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12 l of ammonia were produced by the Haber process How many liters of hydrogen were used during the reaction?
All gasses: 12 L NH3 * [3H / 1NH3] * [1H2 / 2H] = 12*3/2 = 18 L H2
If 6 liters of hydrogen gas are used how many liters of nitrogen gas will be needed for the above reaction at STP?
For the reaction N₂ + 3H₂ → 2NH₃, the mole ratio of hydrogen gas to nitrogen gas is 3:1. Since 6 liters of hydrogen gas is used, you would need 2 liters of nitrogen gas at STP for this reaction according to the stoichiometry of the reaction.
What is the decomposition reaction of Al2O3.3H20?
The decomposition reaction of Al₂O₃·3H₂O is: 2Al₂O₃·3H₂O → 4Al(OH)₃ + 3H₂O. This reaction involves breaking down the hydrated aluminum oxide into aluminum hydroxide and water through the loss of water molecules.
The correct symbol for an atom of tritium?
3H is probably the most common. Technically 31H (the 3 and the 1 should actually be "stacked", but HTML doesn't really allow that) is correct as well, though the 1 is redundant (the H already tells you it has 1 proton). Since T is not used as a symbol for any other element, you'll occasionally see that as well. However, it's not "official".
What mass of ammonia is formed when 3.80 g of nitrogen gas react with hydrogen?
To calculate the mass of ammonia formed, first write out the balanced chemical equation for the reaction between nitrogen and hydrogen to form ammonia: N₂ + 3H₂ → 2NH₃ Next, calculate the moles of nitrogen in 3.80 g using the molar mass of nitrogen (N₂). Then use the mole ratio from the balanced equation to determine the moles of ammonia formed. Finally, convert the moles of ammonia to grams using the molar mass of ammonia (NH₃) to find the mass formed.
1/3h - 4 (2/3h - 3) = 2/3h - 6?
simplify both sides of the equation: 1/3h+(-4)(2/3h)+(-4)(-3)=2/3h+-6 ~ distribute that 1/3h+-8/3h+12=2/3h+-6 (1/3h+-8/3h)+(12)=2/3h-6 ~ combine like terms for this -7/3h+12=2/3h-6 -7/3h+12=2/3h-6 subtract 2/3h from both sides: -7/3h+12-_2/3h=_2/3h-6-2/3h -3h+12=6 subtract 12 from both sides: -3h+12-12=-6-12 -3h=-18 divide both sides by -3 -3h/-3=-18/-3 h=6
How do you Solve the equation 3h plus 13 equals 7?
3h+13 = 7 3h = 7-13 3h = -6 h = -2
12 l of ammonia were produced by the Haber process How many liters of hydrogen were used during the reaction?
All gasses: 12 L NH3 * [3H / 1NH3] * [1H2 / 2H] = 12*3/2 = 18 L H2
What is the answer to this 3h - 5h2 3h3 3h - 6h2 7 - 5h 2h3?
To simplify the expression (3h - 5h^2 + 3h^3 + 3h - 6h^2 + 7 - 5h + 2h^3), first combine like terms. Grouping them gives: ( (3h + 3h - 5h) + (3h^3 + 2h^3) + (-5h^2 - 6h^2) + 7). This simplifies to (-5h^2 + 5h + 5h^3 + 7). The final expression is (5h^3 - 5h^2 + 5h + 7).
What is the for 8h-10h equals 3h plus 25?
h = -5 8h - 10h = 3h + 25 -2h = 3h + 25 -2h - 3h = 3h - 3h + 25 -5h = 25 h = -5 CHECK: 8(-5) - 10(-5) = 3(-5) + 25 -40 - -50 = -15 + 25 -40 + 50 = 10 10 = 10 CORRECT
8h-10h equals 3h plus 25?
8h - 10h = 3h + 25-2h = 3h + 25-5h = 25-h = 5h = -5
What is 3h-2(1 4h) in standard form?
To simplify the expression (3h - 2(1 + 4h)), first distribute the (-2) across the terms in the parentheses: [ 3h - 2 - 8h. ] Next, combine the like terms (3h) and (-8h): [ (3h - 8h) - 2 = -5h - 2. ] Thus, the expression in standard form is (-5h - 2).
What is -3h -2h plus 6h plus 9?
- 3h - 2h + 6h + 9 = h + 9
What is 3h plus 20-h plus 5?
3h + 20 - h + 5 = 2h + 25
What is the value of 4g-3h?
The value of 4g - 3h can't be determined since we are not given the value of g and h. The value of 4g - 3h is actually itself without the known values for g and h.
What is the balanced equation for nitrogen plus hydrogen -- nitrogen trihydride?
The compound which you call nitrogen trihydride is much better known as ammonia, and the formula is NH3.
If 6 liters of hydrogen gas are used how many liters of nitrogen gas will be needed for the above reaction at STP?
For the reaction N₂ + 3H₂ → 2NH₃, the mole ratio of hydrogen gas to nitrogen gas is 3:1. Since 6 liters of hydrogen gas is used, you would need 2 liters of nitrogen gas at STP for this reaction according to the stoichiometry of the reaction.
