What is the ratio of non in the given reaction 4nh3 6no5n2 6h2o?
The reaction is: 4NH3(g) + CaCl2(s) -------------------CaCl2.4NH3(s)
4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)
2[Ag(NH3)2]+ + CH3CHO + 3OH- --> 2Ag + 2H2O + 4NH3 + CH3COO-
The most practical application of the Tollen's reaction is to detect an aldehydic group in a compound. The reaction is as follows: RCHO + 3OH- + 2[Ag(NH3)2]+ --> RCOO- + 2H2O + 2Ag + 4NH3.
Ammonia reacts with oxygen gas to form nitrogen monoxide and water What is the balanced equation for this reaction?
this is the balanced equation 4NH3 + 5O2 = 4NO + 6H2O
How many grams of NO are required to produce 145g of N2 in the following reaction 4nh3 plus 6no 5n2 plus 6h20?
4NH3 + 6NO -> 5N2 + 6H2O 145 g N2 x (1 mol/28.0 g) x (6 mol NO/5 mol N2) x (30.0 g NO/1 mol NO) = 186.4285714 g NO rounds to 186 g NO due to significant figures
A molar ratio is the ratio of any two coefficients in a stoichiometric equation. So in this case, there are six possible combinations. 4:6, 4:5, 4:6, 6:5, 6:6, 5:6.
calcium ammonia chloride
4NH3 + 5O2 -----> 4NO + 6HOH
Which of the following is true for the gas phase reaction shown below 4nh3 g plus 5o2 g 4no g plus 6h2o g Δh equals 0.905 kj?
s is positive and g i s negative at all temperatures
4nh3 + 5o2 --> 4no + 6h2o
4no2 + 6h20 -> 7o2 + 4nh3
4NH3 + N2 = 3N2H4
I am conducting a through ivestigation of the combustion of ammonia gas: 4NH3 + 5O2 > 4NO + 6H2O The reaction will be monitored by the pressure of the gases present in a 5.400 L steel chamber that is at 25.00 degrees C initially but 75 degrees C after the reaction. The chamber is initially filled with 21.250 ATM of oqygen (in slight excess) and an additional 16.500 ATM of ammonia. This one just simply… Read More
3N2H4 equals 4NH3 plus N2
it is know as the silver mirror test, the overall half equation reaction is => CH2O + 2OH- ==> CH2O2 + H2O +2e- [Ag(NH3)2]+ + e- ==> Ag + 2NH3 CH2O + 2OH- + 2[Ag(NH3)2]+ ==> CH2O2 H2O + 2Ag +4NH3
Cu2+ + 4NH3 ----> [Cu(NH3)4]2-
3N2H4 --> 4NH3 + N2 is the correctly balanced equation.
RCHO + 2[Ag(NH3)2] + 2OH- -----> RCOOH + 2Ag0 + 4NH3 + H2O
nitrogen monoxide and Water The balanced equation is as follow: 4NH3 + 5O2-->4NO + 6H2O
What is the balanced equation for Iodine monobromide and ammonia combine to form nitrogen triiodide and ammonium bromide?
3IBr + 4NH3 --> NI3 + 3NH4Br
4NH3 + 5O2 -> 4NO + 6H2O I suspect NH3 limits. Let's see. 5.15 O2 ( 4 mole NH3/5 mole O2) = 4.12 mole NH3 you do not have that much ammonia, so it limits and drives the reaction. 3.80 mole NH3 (4 mole NO/4 mole NH3) = 3.80 moles of NO made
4NH3(g)+5O2(g) --> 4NO(g)+6H2O(g)
A concentrated solution of ammonia is added to a solution of copper II nitrate 4NH3(c) + Cu2+ --> [Cu(NH3)4]2+
it does not produce N2, it produces NO. i think this will help you to balance your equation well in the problem i have, i got: 4 NH3(g) + 3 O2(g) yields 2 N2(g) + 6 H2O(g) No N2 will be produce... This will only produce NO and H2O the balanced equation is 4NH3 + 5O2 --> 4NO + 6H2O this is an equilibrium reaction.
Half equations: CH2O + 2OH- ---> CH2O2 + H2O + 2e [Ag(NH3)2]+ + e ---> Ag + 2NH3 Full equation: CH2O + 2OH- + 2[Ag(NH3)2]+ ---> CH2O2 + H2O + 2Ag + 4NH3 The aldehyde shown is methanal. Same equation for any aldehyde, just replace CH2O with the relevant molecule and balance.
12 2 Mg3N2 + 12 H2O = 6 Mg (OH)2 + 4NH3
Nitrogen trihydride is NH3 Nitrogen monoxide is NO Therefore, NH3 + NO = N2 + H2O 4NH3 + 6NO = 5N2 + 6H2O
Ammonia NH3 burns in oxygen to produce nitrogen dioxide NO2 and water. If 20.3 litres of ammonia are burned how many litres of oxygen are required?
Use dimensional analysis -------------------------------------------------------------------------------------------------------------- The reaction stoichiometry is given by: 4NH3 + 7O2 -> 4NO2 + 6H2O Assuming the reaction is performed in the gas phase at room conditions (1 bar, 298 K) the molar volume of the gases is equal to: Vm = V/n = (RxT)/P = (8.314x10^-2 x 298)/1 = 24.8 L/mol (where R = 8.314x10^-2 bar.L/mol.K) For every 4 moles of NH3 burned 7 moles of O2 are needed. In the performed… Read More
RNO2 + 4[H] +Zn+ NH4Cl ----> RNHOH +H2O RNHOH + 2Ag(NH3)2OH ----> RNO + 2H2O + 2Ag + 4NH3
What is the balanced formula for Gaseous ammonia NH3 reacts with gaseous oxygen to form gaseous nitrogen monoxide and gasesous water?
Key points to know are Ammonia and oxygen from the air are react together to make nitrogen monoxide and water. 4NH3 + 5O2 --------> 4 NO + 6 H2O Or at a higher temperature the first reaction happens followed by the nitrogen monoxide is reacted with more oxygen from the air to make nitrogen dioxide which is a brown poisonous gas. 2 NO + O2----------> 2NO2
When an Ammonium solution (NH4OH or simply NH3 with water) is added to Copper Sulfate (CUSO4), it forms what we call a "complex". It is called the Tetraamminecuprate(II) complex. The color of the soultion is deep blue and may form a white precipitate. Here's the reaction: Cu2+ + 4NH3 -----> Cu(NH3)4 (with a 2- charge) Only copper reacts with the ammonium, so there is no need to include the sulfate (SO4) and the hydroxide (OH-)
Yes - there are equal values of nitrogen (4) and hydrogen (12) on both sides of this equation, and all molecular formulas are in empirical form.
4NH3 + 3O2 -----> 2N2 + 6H2O 4 moles of ammonia react with 3 of oxygen. So 10 moles of ammonia requires 7.5 moles of oxygen.
Ammonia can be mixed with fuel to make a simple but large explosion. This acts as a chemical catalyst in the explosion. But I don't think the ATF or FBI would like us to discuss this in detail. well, my dad's in the FBI and he's the one who told me about it. --------------------------------------------------------------------------------------------------------- Ammonia in combustion produces a very large amount of energy and produces a large volume of gas. both the rapidity and… Read More
How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH3? 4NH3(g) + 5O2(g) => 4NO(g) + 6H2O(g)
In basic conditions copper typically forms a hydroxide precipitate (copper (II) is hexadentate and so is octadehral). Alkalis (such as NaOH) and dilute lewis bases (such as ammonia) will produce the precipitate. The net reaction could be summarised: Cu(s) + 2OH-+ 4H2O → [Cu(H2O)4(OH)2](s) The aqueous copper can ligate with lewis bases. Excess ammonia would produce the following reaction: [Cu(H2O)4(OH)2](s) + 4NH3 → [Cu(NH3)4(H2O)2]2+(aq)+ 2OH- + 2H2O In a similar way copper metal can react… Read More
CoCl3 + 6NH3 -> [Co(NH3)6]3+(Cl-)3 CoCl3 + 5NH3 -> [Co(NH3)5(Cl)]2+(Cl-)2 CoCl3 + 4NH3 -> [Co(NH3)4(Cl)2]1+(Cl-)1 CoCl3 + 3NH3 -> [Co(NH3)3(Cl)3]
How many grams of H2O can be made by the combustion of 42.5g of NH3 according to the following equation 4NH3 5O2 4NO 6H2O?
42.5 g of NH3 is equivalent to around 2.5 moles. Since there are 3 moles of H2O produced for every 2 moles of NH3 used, 3.75 moles of H2O are produced. This around 3.79 g of water.
4.50 moles NO2 X (46 grams NO2) / (1 mole NO2) x (4 moles NO2) / (7 moles O2) x (1 mole O2) / (32 gm O2) = 3.70 grams O2
The equation is as follows: CH2OH(CHOH)4CHO(aq) + 2Ag(NH3)2+(aq) + 3OH- (aq) → (Glucose) (Tollen's Reagent, Ammoniacal Silver Nitrate) 2Ag(s) + CH2OH(CHOH)4COO-(aq) + 4NH3(aq) + 2H2O(l) (Silver metal, (Gluconic acid) which forms silver mirror)
How many grams of H2O can be made by the combustion of 42.5g of NH3 according to the following equation 4NH3 5O2 equals 4NO 6H2O?
Using the molar mass of nh3, we find that we have 2.5 moles of nh3. Since 3 moles of h2o are produced per 2 moles of nh3, we see that we will produce 3.75 moles of h2o. This is equivalent to around 3.79 g.
If the temperature and pressure are constant, then the volumes of gases are equivalent to moles. 4NH3(g) + 6NO (g) --> 5N2(g) +6H2O (g) shows that for every 4 L of NH3 used, so are 6 L of NO. 30.0 L (4 L NH3/ 6 L NO) = 20.0 L of NH3.
A Copper (II) Nitrate Solution is Mixed with an Ammonia Solution, @ Equilibrium the Solution is Clear & Deep Blue in Color. Cu(H2O)42+ (aq) + 4NH3 (aq) <=======> Cu(NH3)42+ (aq) + 4H2O (l) Clear & Pale Blue Clear & Colorless Clear & Deep Blue Clear & Colorless see related link "How to Balance Equations"
How many moles of H2O can be formed when 4.5 moles of NH3 react with 3.2 moles of O2 NH3 plus O2 yields NO plus H2O?
4NH3 + 5O2 ==> 4NO + 6H2O balanced equation for the reaction4.5 moles NH3/4 = 1.125 3.2 moles O2/5 = 0.64 THIS IS THE LIMITING REACTANT moles of H2O formed = 3.2 moles O2 x 6 moles H2O/5 moles O2 = 3.84 moles H2O formed
Zinc(II) ion reacts with aqueous ammonia to precipitate white gelatinous Zn(OH)2: Zn2+(aq) + 2NH3(aq) + 2H2O(l) <==> Zn(OH)2(s) + 2NH4+(aq) The zinc(II) hydroxide precipitate dissolves in excess ammonia: Zn(OH)2(s) + 4NH3(aq) <==> [Zn(NH3)4]2+(aq) + 2OH-(aq) The zinc(II) hydroxide precipitate also dissolves in hydroxide: Zn(OH)2(s) + 2OH-(aq) <==> [Zn(OH)4]2-(aq) It also react with acids!
Each Amino Acid has an alpha carbon, that carbon is attached to a hydrogen, a carboxyl group, amine and an R-group (side chain). The first three constituents are pretty much always the same throughout the amino acids, therefore, what makes each amino acid unique, is its R-group. For example, the R group of Alanine is a methyl while the R group of say Lysine is a (CH2)4NH3+ .. big difference. However, Proline, which is technically… Read More
First you can observe the colour of the solution which has to be tested. If the solution shows no colour, it can be straightly concluded that there is no Copper(II) ions present. If it shows a colour, carry out the following tests. Bubble hydrogen sulfide gas through the solution, a black precipitate MAY be formed from Copper(II) ions. Add a solution of sodium hydroxide followed by heating. At first there will be a greenish blue… Read More